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Case Study and Passage Based Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations

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In CBSE Class 10 Science Paper, Students will have to answer some questions based on Assertion and Reason . There will be a few questions based on case studies and passage based as well. In that, a paragraph will be given, and then the MCQ questions based on it will be asked.

Here, we have provided case based/passage based questions for Class 10 Science Chapter 1 Chemical Reactions and Equations.

Case Study and Passage Based Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations

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Case Study/Passage Based Questions on Chemical Reactions and Equations

Case Study/Passage Based Questions

Question 1:

Corrosion is the phenomenon of deterioration of surface of metal in presence of air and moisture. It is a natural process and in the presence of a moist atmosphere, chemically active metals get corroded. This is an oxidation reaction. Rusting is the process where iron corrodes due to exposure to the atmosphere. The main circumstance of corrosion occurs with iron because it is a structural material in construction, bridges, buildings, rail transport, ships, etc. Aluminium is also an important structural metal, but even aluminium undergoes oxidation reactions. However, aluminium doesn’t corrode or oxidize as rapidly as its reactivity suggests. Copper (Cu) corrodes and forms a basic green carbonate.

(i) What is rusting?

(ii) Which two metals do not corrode easily?

(iii) Write the chemical name of the compound formed on corrosion of silver.

(iv) Corrosion is (a) a redox reaction (b) a reduction reaction (c) a displacement reaction (d) an oxidation reaction

Also read: Assertion Reason Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations

Question 2:

Oxidation is the process of gaining of oxygen, or losing of hydrogen. Reduction is the process of losing of oxygen or gaining of hydrogen. The substance which undergoes oxidation is the reducing agent while the substance which undergoes reduction is known as the oxidising agent. Oxidation and reduction always take place together and these type of reactions are known as redox reactions. Some of the examples of redox reactions are given below:

class 10 chapter 1 case study questions science

(i) Give two examples of oxidation reaction from your everyday life.

(ii) Write the oxidising agent in the reaction III and VI.

(iii) Which of the following is an oxidising agent? (a) LiAlH 4 (b) Alkaline KMnO 4 (c) Acidified K 2 Cr 2 O 7 (d) Both (b) and (c)

(iv) Out of oxidation and reduction, which reaction takes place at anode?

Also read: Extra Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations

Question 3:

A chemical reaction is a representation of chemical change in terms of symbols and formulae of reactants and products. There are various types of chemical reactions like combination, decomposition, displacement, double displacement, oxidation and reduction reactions. Reactions in which heat is released along with the formation of products are called exothermic chemical reactions. All combustion reactions are exothermic reactions.

(i) The chemical reaction in which a single substance breaks down into two or more simpler substances upon heating is known as (a) thermal decomposition reaction (b) photo decomposition reaction (c) electric decomposition reaction (d) both (a) and (c)

(ii) The massive force that pushes the rocket forward through space is generated due to the (a) combination reaction (b) decomposition reaction (c) displacement reaction (d) double displacement reaction

(iii) A white salt on heating decomposes to give brown fumes and yellow residue is left behind. The yellow residue left is of (a) lead nitrate (b) nitrogen oxide (c) lead oxide (d) oxygen gas

(iv) Which of the following reactions represents a combination reaction? (a) CaO (s) + H 2 O (l) → Ca(OH) 2 (aq) (b) CaCO 3 (s) → CaO (s) + CO 2 (g) (c) Zn(s) + CuSO 4 (aq) → ZnSO 4 (aq) + Cu(s) (d) 2FeSO 4 (s) → Fe 2 O 3 (s) +SO 2 (g) + SO 3 (g)

(v) Complete the following statements by choosing correct type of reaction for X and Y. Statement 1: The heating of lead nitrate is an example of ‘X’ reaction. Statement 2: The burning of magnesium is an example of ‘Y’ reaction. (a) X- Combination, Y- Decomposition (b) X- Decomposition, Y-Combination (c) X- Combination, Y-Displacement (d) X- Displacement, Y-Decomposition

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3 thoughts on “ Case Study and Passage Based Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations ”

Good examples! But can you please available practical types and equations type of case based questions which we can read and learn an then they help us to solve the Boards examm. Pleaseeww🙂🙂🙂

would love to see more equation based questions. nevertheless, it proved quite useful in my revision!

after going through the above content child should develops ideas to answer based on knowledge acquired.

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Case Study Questions Class...

Case Study Questions Class 10 Science

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Download the app to get CBSE Sample Papers 2023-24, NCERT Solutions (Revised), Most Important Questions, Previous Year Question Bank, Mock Tests, and Detailed Notes.

Download Case study questions for CBSE class 10 Science in PDF format from the myCBSEguide App . We have the new pattern case study-based questions for free download. Class 10 Science case study questions

This article will guide you through:

What are case study questions?

Sample Papers with Case Study questions
Class 10 Science Case Study question examples
How to get case-based questions for free?
How to attempt the case-based questions in Science?

Questions based on case studies are some real-life examples. The questions are asked based on a given paragraph i.e. Case Study. Usually, 4-5 questions are asked on the basis of the given passage. In most cases, these are either MCQs or assertion & reason type questions. Let’s take an example to understand. There is one paragraph on how nitrogen is generated in the atmosphere. On the basis of this paragraph, the board asks a few objective-type questions. In other words, it is very similar to the unseen passages given in language papers. But the real cases may be different. So, read this article till the end to understand it thoroughly.

What is CBE?

CBSE stands for competency-based education. The case study questions are part of this CBE. The purpose of CBE is to demonstrate the learning outcomes and attain proficiency in particular competencies.

Questions on Real-life Situations

As discussed the case study questions are based on real-life situations. Especially for grade 10 science, it is very essential to have the practical knowledge to solve such questions. Here on the myCBSEguide app, we have given many such case study paragraphs that are directly related to real-life implications of the knowledge.

Sample Papers with Case Study Questions

Class 10 Science Sample Papers with case study questions are available in the myCBSEguide App . There are 4 such questions (Q.No.17 to 20) in the CBSE model question paper. If you analyze the format, you will find that the MCQs are very easy to answer. So, we suggest you, read the given paragraph carefully and then start answering the questions. In some cases, you will find that the question is not asked directly from the passage but is based on the concept that is discussed there. That’s why it is very much important to understand the background of the case study paragraph.

CBSE Case Study Sample Papers

You can download CBSE case study sample papers from the myCBSEguide App or Student Dashboard. Here is the direct link to access it.

Case Study Question Bank

As we mentioned that case study questions are coming in your exams for the last few years. You can get them in all previous year question papers issued by CBSE for class 1o Science. Here is the direct link to get them too.

Class 10 Science Case Study Question Examples

As you have already gone through the four questions provided in the CBSE model question paper , we are proving you with other examples of the case-based questions in the CBSE class 10 Science. If you wish to get similar questions, you can download the myCBSEguide App and access the Sample question papers with case study-type questions.

Case-based Question -1

Read the following and answer any four questions: Salt of a strong acid and strong base is neutral with a pH value of 7. NaCl common salt is formed by a combination of hydrochloride and sodium hydroxide solution. This is the salt that is used in food. Some salt is called rock salt bed of rack salt was formed when seas of bygone ages dried up. The common salt thus obtained is an important raw material for various materials of daily use, such as sodium hydroxide, baking soda, washing soda, and bleaching powder.

Phosphoric acid
Carbonic acid
Hydrochloric acid
Sulphuric acid
Blue vitriol
Washing soda
Baking soda
Bleaching powder

Case-based Question -2

V 1 + V 2 + V 3
V 1 – V 2 +V 2
None of these
same at every point of the circuit
different at every point of the circuit
can not be determined
20 3 Ω 203Ω
15 2 Ω 152Ω

Case-based Question -3

pure strips
impure copper
refined copper
none of these
insoluble impurities
soluble impurities
impure metal
bottom of cathode
bottom of anode

How to Attempt the Case-Based Questions in Science?

Before answering this question, let’s read the text given in question number 17 of the CBSE Model Question Paper.

All living cells require energy for various activities. This energy is available by the breakdown of simple carbohydrates either using oxygen or without using oxygen.

See, there are only two sentences and CBSE is asking you 5 questions based on these two sentences. Now let’s check the first questions given there.

Energy in the case of higher plants and animals is obtained by a) Breathing b) Tissue respiration c) Organ respiration d) Digestion of food

Now let us know if you can relate the question to the paragraph directly. The two sentences are about energy and how it is obtained. But neither the question nor the options have any similar text in the paragraph.

So the conclusion is, in most cases, you will not get direct answers from the passage. You will get only an idea about the concept. If you know it, you can answer it but reading the paragraph even 100 times is not going to help you.

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Case Study Chapter 1 Chemical Reactions and Equations

Please refer to Chapter 1 Chemical Reactions and Equations Case Study Questions with answers provided below. We have provided Case Study Questions for Class 10 Science for all chapters as per CBSE, NCERT and KVS examination guidelines. These case based questions are expected to come in your exams this year. Please practise these case study based Class 10 Science Questions and answers to get more marks in examinations.

Case Study Questions Chapter 1 Chemical Reactions and Equations

Case/Passage – 1 The reaction between MnO 2 with HCl is depicted in the following diagram. It was observed that a gas with bleaching abilities was released .

Case Study Chapter 1 Chemical Reactions and Equations

Question: Identify the correct statement from the following: (a) MnO2 is getting reduced whereas HCl is getting oxidized (b) MnO2 is getting oxidized whereas HCl is getting reduced. (c) MnO2 and HCl both are getting reduced. (d) MnO2 and HCl both are getting oxidized.

Question: Chlorine gas reacts with _____ to form bleaching powder. (a) dry Ca(OH) 2 (b) dil. solution of Ca(OH) 2 (c) conc. solution of Ca(OH) 2 (d) dry CaO

Question: In the above discussed reaction, what is the nature of MnO2? (a) Acidic oxide (b) Basic oxide (c) Neutral oxide (d) Amphoteric oxide

Question: The chemical reaction between MnO2 and HCl is an example of: (a) displacement reaction (b) combination reaction (c) redox reaction (d) decomposition reaction.

Question: What will happen if we take dry HCl gas instead of aqueous solution of HCl? (a) Reaction will occur faster. (b) Reaction will not occur. (c) Reaction rate will be slow. (d) Reaction rate will remain the same.

Case/Passage – 2

Chemistry in Automobiles: For an internal combustion engine to move a vehicle down the road, it must convert the energy stored in the fuel into mechanical energy to drive the wheels. In your car, the distributor and battery provide this starting energy by creating an electrical “spark”, which helps in combustion of fuels like gasoline. Below is the reaction depicting complete combustionof gasoline in full supply of air: 2C 8 H 18 (I) + 25O 2 (g) → 16 ‘X’ + Y Question: Which of the following are the products obtained from the reaction mentioned in the above case? Product ‘ X’ Product ‘Y’ (a) CO 2 H 2 O 2 (b) H 2 O CO (c) CH 3 OH H 2 O (d) CO 2 H 2 O

Question: On the basis of evolution/absorption of energy, which of the following processes are similar to combustion of fuel? (i) Photosynthesis in plants (ii) Respiration in the human body (iii) Decomposition of vegetable matter (iv) Decomposition of ferrous sulphate. (a) (ii) & (iii) (b) (i) & (ii) (c) (iii) & (iv) (d) (ii) & (i)

Question: ‘Although nitrogen is the most abundant gas in the atmosphere, it does not take part in combustion’. Identify the correct reason for this statement. (a) Nitrogen is a reactive gas (b) Nitrogen is an inert gas (c) Nitrogen is an explosive gas (d) Only hydrocarbons can take part in combustion

Question: Identify the types of chemical reaction occurring during the combustion of fuel: (a) Oxidation & Endothermic reaction (b) Decomposition & Exothermic reaction (c) Oxidation & Exothermic reaction (d) Combination & Endothermic reaction

Question: ‘A student while walking on the road observed that a cloud of black smoke belched out from the exhaust stack of moving trucks on the road.’ Choose the correct reason for the production of black smoke: (a) Limited supply of air leads to incomplete combustion of fuel. (b) Rich supply of air leads to complete combustion of fuel. (c) Rich supply of air leads to a combination reaction. (d) Limited supply of air leads to complete combustion of fuel.

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Class 10 Science Case Study Questions PDF Download

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Are you searching for a comprehensive resource to improve your understanding and problem-solving skills in Class 10 Science? Look no further! In this article, we will explore the world of Class 10 Science case study questions and provide you with an opportunity to download a PDF resource containing a collection of case study questions designed specifically for this subject. Let’s dive in and enhance your knowledge!

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CBSE Class 10th – SCIENCE: Chapterwise Case Study Question & Solution

Case study questions provide a practical and real-life context for applying scientific concepts and principles. These questions require you to analyze a given scenario, identify relevant information, and utilize your scientific knowledge to solve problems or draw conclusions. Case study questions assess your ability to think critically, make connections, and apply scientific principles in a practical setting.

Chapterwise Case Study Questions for Class 10 Science

To support your preparation for Class 10 Science examinations, we have created a comprehensive PDF resource containing a collection of case study questions designed specifically for this subject. This PDF includes a variety of case studies covering different topics in Physics, Chemistry, and Biology. It will provide you with ample practice opportunities to enhance your analytical and problem-solving skills.

Case Study Questions for Chapter 1 Chemical Reactions and Equations
Case Study Questions for Chapter 2 Acids, Bases, and Salts
Case Study Questions for Chapter 3 Metals and Non-Metals
Case Study Questions for Chapter 4 Carbon and Its Compounds
Case Study Questions for Chapter 5 Periodic Classification of elements
Case Study Questions for Chapter 6 Life Processes
Case Study Questions for Chapter 7 Control and Coordination
Case Study Questions for Chapter 8 How do organisms reproduce?
Case Study Questions for Chapter 9 Heredity and Evolution
Case Study Questions for Chapter 10 Light reflection and refraction
Case Study Questions for Chapter 11 Human eye and colorful world
Case Study Questions for Chapter 12 Electricity
Case Study Questions for Chapter 13 Magnetic effects of current
Case Study Questions for Chapter 15 Our Environment

The above Case studies for Class 10 Science will help you to boost your scores as Case Study questions have been coming in your examinations. These CBSE Class 10 Science Case Studies have been developed by experienced teachers of schools.studyrate.in for the benefit of Class 10 students.

Class 10th Maths Case Study Questions

Benefits of Case Study Questions

Engaging with case study questions in Class 10 Science offers several benefits. Let’s explore some of them:

Real-life application: Case study questions allow you to apply scientific concepts to real-life situations, enhancing your understanding of their practical relevance.
Critical thinking skills: Analyzing case studies promotes critical thinking by challenging you to evaluate information, identify patterns, and draw logical conclusions.
Problem-solving abilities: Case study questions require you to identify problems, propose solutions, and make informed decisions based on scientific evidence.
Holistic learning: By examining different aspects of a case, you gain a broader perspective on scientific concepts and their interconnections.
Preparation for higher education: Case study questions prepare you for future academic pursuits by developing skills necessary for scientific research and analysis.

Understanding the Structure of Case Study Questions

Case study questions typically present a scenario or a problem related to a scientific concept. The questions may require you to analyze data, interpret graphs, or propose solutions based on the given information. It is important to read the case study carefully, identify key details, and understand the context before attempting to answer the questions.

Tips for Analyzing and Answering Case Study Questions

To effectively analyze and answer case study questions, consider the following tips:

Read the case study thoroughly: Take your time to understand the scenario, paying attention to key details and any scientific concepts mentioned.
Identify the problem or objective: Determine the main question or objective that the case study aims to address. This will guide your analysis and help you stay focused.
Break down the questions: Carefully read each question and break it down into smaller parts. Identify the specific information or data required to answer each question accurately.
Apply scientific knowledge: Utilize your understanding of scientific principles and concepts to analyze the case study. Make connections between the given information and relevant scientific theories.
Support your answers: Whenever possible, support your answers with scientific evidence or reasoning. Refer to specific data, graphs, or concepts from the case study to justify your conclusions.

Subject-wise Approach to Case Study Questions

Let’s explore how to approach case study questions in the subjects of Physics, Chemistry, and Biology.

In Physics case study questions, focus on understanding the principles and laws governing the given scenario. Analyze the data provided and apply relevant formulas and concepts to solve the problem. Consider factors such as motion, forces, energy, and electrical circuits, depending on the context of the case study.

Chemistry case study questions often involve analyzing chemical reactions, properties of substances, or experimental data. Pay attention to the details of the case study, such as reactants, products, conditions, and observations. Apply your knowledge of chemical reactions, bonding, and periodic trends to interpret and solve the problem.

Biology case study questions revolve around biological processes, organisms, and ecological relationships. Analyze the provided information, such as species interactions, environmental factors, or experimental results. Apply your understanding of biological concepts, such as genetics, evolution, ecosystems, and cellular processes, to address the questions effectively.

Importance of Practicing Case Study Questions

Practicing case study questions in Class 10 Science is crucial for several reasons:

Application of knowledge: Case study questions enable you to apply scientific knowledge to real-life situations, enhancing your understanding and practical skills.
Analytical thinking: Regular practice of case study questions hones your analytical thinking skills by challenging you to analyze complex scenarios and make informed decisions.
Comprehensive understanding: Engaging with case studies offers a holistic understanding of scientific concepts, allowing you to grasp their practical implications and interconnections.
Exam preparation: Practicing case study questions familiarizes you with the question patterns and formats commonly seen in Class 10 Science examinations, boosting your confidence and performance.

Case study questions offer a valuable opportunity to apply scientific knowledge in practical contexts. By engaging with these questions, you can develop critical thinking, problem-solving, and analytical skills necessary for success in Class 10 Science. Remember to carefully analyze the case study, apply your scientific understanding, and justify your answers with relevant evidence. Regular practice of case study questions will greatly enhance your overall performance in examinations.

Where can I find Class 10 Science case study questions?

You can download a comprehensive PDF resource containing Class 10 Science case study questions from schools.studyrate.in This resource is specifically designed to provide you with ample practice material.

Why is practicing case study questions important for exam preparation?

Regular practice of case study questions enhances your ability to apply scientific knowledge in practical contexts, improving your analytical thinking and problem-solving abilities. This ultimately contributes to better performance in Class 10 Science examinations.

How should I approach Class 10 Science case study questions?

Read the case study carefully, identify the problem or objective, and analyze the given information. Apply your scientific knowledge to address the questions and support your answers with relevant evidence.

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CBSE Class 10th - SCIENCE : Chapterwise Case Study Question & Solution

In board exams, students will find the questions based on assertion and reasoning. Also, there will be a few questions based on case studies. In that, a paragraph will be given, and then the MCQ questions based on it will be asked. For Science subjects, there would be 5 case-based sub-parts questions, wherein a student has to attempt 4 sub-part questions.

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CBSE Class 10 Science Case Study Questions Download Free PDF

If you are looking for the CBSE Class 10 Science Case Study Questions in PDF, then you are in the right place. CBSE 10th Class Case Study for the Science Subject is available here. These Case studies can help the students to solve the different types of questions that are based on the case study.

CBSE Board will be asking case study questions based on Science subjects in the upcoming board exams. Thus, it becomes an essential resource to study.

The Science Subject case study for class 10th covers a wide range of chapters from the Science. Students willing to score good marks in their board exams can use it. The questions are highly interactive and it allows students to use their thoughts and skills to solve such kinds of questions.

Case Study Questions Class 10 Science

Case Study Questions for Chapter 1 Chemical Reactions and Equations
Case Study Questions for Chapter 2 Acids, Bases, and Salts
Case Study Questions for Chapter 3 Metals and Non-Metals
Case Study Questions for Chapter 4 Carbon and Its Compounds
Case Study Questions for Chapter 5 Periodic Classification of elements
Case Study Questions for Chapter 6 Life Processes
Case Study Questions for Chapter 7 Control and Coordination
Case Study Questions for Chapter 8 How do organisms reproduce?
Case Study Questions for Chapter 9 Heredity and Evolution
Case Study Questions for Chapter 10 Light reflection and refraction
Case Study Questions for Chapter 11 Human eye and colorful world
Case Study Questions for Chapter 12 Electricity
Case Study Questions for Chapter 13 Magnetic effects of current
Case Study Questions for Chapter 15 Our Environment

The above Case studies for CBSE Class 10 Science will help you to score good marks in the Case Study questions that have been coming in your examinations. These CBSE Class 10 Science Case Study have been developed by experts of cbseexperts.com for benefit of Class 10 students.

Class 10 Science Assertion and Reason Questions

Case Study Type Questions in Science Class 10

Case Study Type Questions in Science Class 10 include the information or data. Students willing to solve them are required to read the passage carefully and then solve them. While solving the paragraph the ideal way is to highlight the key information or given data.

Because later it will ease them to write the final answers. Science Case study type questions consist of 4 to 5 questions that should be answered in an MCQ manner.

While reading the paragraph students will get the clue in between about the possible answer of the question. They should definitely highlight those questions. This is the best way to solve such kind of Case study Type Questions.

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Important Questions for CBSE Class 10 Science Chapter 1 - Chemical Reactions and Equations 2024-25

CBSE Class 10 Science Chapter 1 Chemical Reactions and Equations Important Questions - Free PDF Download

Class 10 board examination is the most crucial exam in every students’ life. Their future studies and career depend on the mark secured in the board exams. Every student works hard to score well in Class 10 CBSE examinations . Science among all the subjects of Class 10 has a vital role in every students’ career. Science teaches us how the world and our environment is made. The students can secure better marks in the science subject if they want to become a doctor or an engineer in future. It is important that they should prepare and study hard for this subject, so they don’t lose marks. Chapter 1 of Class 10 Science , which is on chemical reactions and equations, is challenging for the students to understand. Students should revise and practise the Important Questions of Class 10 Science Chapter 1 to secure good marks. These questions aim at providing a better understanding of the chapter to the students. Vedantu is a platform that provides free CBSE Solutions (NCERT) and other study materials for students. Maths Students who are looking for the better solutions, they can download Class 10 Maths NCERT Solutions to help you to revise complete syllabus and score more marks in your examinations.

Download CBSE Class 10 Science Important Questions 2024-25 PDF

Also, check CBSE Class 10 Science Important Questions for other chapters:

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Study Important Questions for Class 10 Science Chapter 1 – Chemical Reactions and Equations

Very Short Answer Questions (1 Mark)

1. Some crystals of copper sulphate were dissolved in water. The colour of the solution obtain would be

Ans: (c) Blue

2. When dilute \[HCl\] is added to zinc pieces taken in a test tube

No change takes place

The colour of the solution becomes yellow.

A pungent smelling gas gets liberated

Small bubbles of \[{{H}_{2}}\] gas appear on the surface of zinc pieces

Ans: (d) Small bubbles of \[{{H}_{2}}\] gas appear on the surface of zinc pieces.

3. \[PbS\] reacts with ozone ( \[{{O}_{3}}\] ) and forms \[PbS{{O}_{4}}\] . As per the balanced equation, molecules of ozone required for every one molecule of \[PbS\] is/are

Ans: (a) \[4\]

4. Chemically rust is

Hydrated ferrous oxide

Hydrated ferric oxide

Only ferric oxide

None of these

Ans: (b) Hydrated ferric oxide

5. Which of the following reactions is not correct

\[Zn+CuS{{O}_{4}}\to ZnS{{O}_{4}}+Cu\]

\[2Ag+Cu{{(N{{O}_{3}})}_{2}}\to 2AgN{{O}_{3}}+Cu\]

\[Fe+CuS{{O}_{4}}\to FeS{{O}_{4}}+Cu\]

\[Mg+2HCl\to MgC{{l}_{2}}+{{H}_{2}}\]

Ans: (b) \[2Ag+Cu{{(N{{O}_{3}})}_{2}}\to 2AgN{{O}_{3}}+Cu\]

6. Copper displaces which of the following metals from its salt solution:

\[ZnS{{O}_{4}}\]

\[FeS{{O}_{4}}\]

\[AgN{{O}_{3}}\]

\[NiS{{O}_{4}}\]

Ans: (c) \[AgN{{O}_{3}}\]

7. In an electrolytic cell where electrolysis is carried, anode has:

Positive change

Negative charge

Connected to negative terminal of the battery

None of these is correct.

Ans : (a) Positive change

8. The reaction \[{{H}_{2}}+C{{l}_{2}}\to 2HCl\] represents:

Oxidation

Reduction

Decomposition

Combination

Ans: (d) combination

9. In the reaction \[PbO+C\to Pb+CO\]

\[PbO\] is oxidised

\[C\] acts as an oxidising agent

\[C\] acts as a reduction agent

Reaction does not represent redox reaction.

Ans: (c) \[C\] acts as a reduction agent.

10. A substance which oxidizes itself and reduces other is known as

Oxidising agent

reducing agent

Both (a) and (b)

None of these.

Ans: (b) Reducing agent

11. Take about \[5\] ml of dil. \[HCl\] in a test tube and add a few pieces of fine granules to it. Which gas is evolved?

Chlorine

Hydrogen

Nitrogen

Ans: (b) Hydrogen

12. Dissolving sugar is an example of-

Physical change

Chemical change

Redox Reaction

Ans: (a) Physical change

13. Heat is evolved diving

Endothermic Reaction

Displacement Reaction

Combustion Reaction

Combination Reaction

Ans: (c) Combustion Reaction

14. Which of the following is not a balanced equation?

\[Fe+C{{l}_{2}}\to FeC{{l}_{3}}\]

\[Mg+CuS{{O}_{4}}\to MgS{{O}_{4}}+{{C}_{4}}\]

\[NaOH+HCl\to NaCl+{{H}_{2}}O\]

\[Zn+S\to ZnS\]

Ans: (a) \[Fe+C{{l}_{2}}\to FeC{{l}_{3}}\]

15. The reaction between lead nitrate and potassium iodide present in aqueous solutions is an example of

Decomposition Reaction

Double Displacement Reaction

Neutralisation Reaction

Ans: (c) Double Displacement Reaction

16. What happens when dilute hydrochloric acid is added to iron filling? Tick the correct answer

Hydrogen gas and iron chloride are produced.

Chlorine gas and iron hydroxide are produced

No reaction takes place

Iron salt and water are produced

Ans: (a) Hydrogen gas and iron chloride are produced.

Short Answer Questions (2 Marks)

1. Identify the type of chemical reaction

i. \[A\to B+C\]

Ans: \[A\to B+C\] is a decomposition reaction.

ii. \[AD+CD\to AD+CB\]

Ans: \[AD+CD\to AD+CB\] is a double displacement reaction.

2. Why does not silver evolve hydrogen on reacting with dil \[{{H}_{2}}S{{O}_{4}}\] ?

Ans: Silver does not evolve hydrogen on reacting with dil. \[{{H}_{2}}S{{O}_{4}}\] as silver is a less reactive metal than hydrogen.

3. Why do diamond and graphite, the two allotropic forms of carbon, evolve different amounts of heat on combustion?

Ans: Diamond and graphite are the two allotropes of carbon but they evolve different amounts of heat on combustion because the arrangement of carbon atoms and thus their shapes are different from one another.

4. What is the role of oxidizing agent in a reaction?

Ans: The role of oxidizing agent in a reaction is that it supplies the oxygen or removes the hydrogen in the reaction.

5. What happens chemically when quick lime is added to water?

Ans: When quick lime is added to water a lot of heat is evolved and calcium hydroxide (or slaked lime) is formed with a hissing sound. The chemical reaction involved is

\[CaO(s)+{{H}_{2}}O(\text{quicklime})\to Ca{{(OH)}_{2}}+\text{Heat(shakedLime)}\]

6. Why a combustion reaction an oxidation reaction?

Ans: Combustion reaction is an oxidation reaction because it is always carried out in the presence of oxygen. The chemical reaction involved is:

\[C{{H}_{4}}(g)+2{{O}_{2}}(g)\to C{{O}_{2}}(g)+2{{H}_{2}}O(l)\]

7. Why are food particle preferably packed in aluminium foil?

Ans: Food particles are preferably packed in aluminium foil because it does not corrode in atmosphere. A protective coating of aluminium oxide ( \[A{{l}_{2}}{{O}_{3}}\] ) is formed on the surface of the foil and it stops any further reaction of the metal with air and water so even if it is kept for a long time food particles do not get spoiled.

8. What happens to lime water when \[C{{O}_{2}}\] gas is bubbled through it in excess?

Ans: When \[C{{O}_{2}}\] gas is bubbled through lime water in excess then initially it becomes milky but after some time its milkiness disappears. This is because initially calcium carbonate is formed which causes the lime water to turn milky and when further \[C{{O}_{2}}\] is passed calcium bicarbonate is formed which turns the solution colourless.

9. Why is a Combustion reaction an oxidation reaction?

Ans: Combustion is an oxidation reaction as it is always carried out in the presence of oxygen. In an oxidation reaction, oxygen is added to or removed from a compound. For example,

\[C{{H}_{4}}+2{{O}_{2}}\to C{{O}_{2}}+2{{H}_{2}}O\]

10. Identify the type of chemical reaction

i. \[A+B\to C\]

Ans: This is a combination reaction in which a single product is formed from multiple reactants.

ii. \[A+BC\to AC+B\]

Ans: It is a displacement reaction in which a more reactive reactant displaces a less reactive element in the compound.

11. Why cannot a chemical change be normally reversed?

Ans: Chemical change cannot be normally reversed because products so formed in a chemical reaction are quite different from the reactants.

12. Identify the substance oxidized and reduced in the reaction.

\[CuO(s)+Zn(s)\to ZnO(s)+Cu(s)\]

Ans: The substance oxidized is Zinc and the substance reduced is copper oxide.

13. A student took two-three g of a substance $X$ in a glass beaker & poured water over it slowly. He observed bubbles along with hissing noise. The beaker becomes quite hot. Identify $X$ . What type of reaction is it?

Ans: In the given experiment where the student took two-three g of a substance $X$ in a glass beaker and poured water over it slowly. He observed bubbles along with hissing noise and the beaker became quite hot after the reaction. Therefore, here $X$ is Calcium oxide (or Quick lime) and the reaction is a type of combination reaction.

14. A substance $X$ used for coating iron articles is added to a blue solution of a reddish-brown metal $Y$ , the colour of the solution gets discharged. Identify $X$ and $Y$ & also the type of reaction.

Ans: Here, a substance $X$ used for coating iron articles is added to a blue solution of a reddish-brown metal $Y$ , the colour of the solution gets discharged . Therefore, $X$ is Iron ( \[Fe\] ) $Y$ is Copper ( \[Cu\] ). Also, it is a type of a displacement reaction.

15. A student burnt a metal \[A\] found in the form of ribbon. The ribbon burnt with a dazzling Flame & a white powder \[B\] is formed which is basic in nature. Identify \[A\] & \[B\] . Write the Balanced chemical equation.

Ans: The balanced chemical reaction for the given experiment is:

$X=Mg,Y=MgO,Mg+{{O}_{2}}\to 2MgO$

16. Why should a magnesium ribbon be cleaned before burning in air?

Ans: A magnesium ribbon should be cleaned before burning in air in order to remove the protective layer of basic magnesium carbonate from the surface of magnesium ribbon.

17. Write the balanced chemical equation with state symbols for the following reactions?

Ans: Balance chemical reaction with state symbols are:

i. $BaC{{l}_{2}}(aq)+N{{a}_{2}}S{{O}_{4}}(aq)\to BaS{{O}_{4}}(s)+2NaCl(aq)$

ii. $NaOH(aq)+HCl(aq)\to NaCl(aq)+{{H}_{2}}O$

18. A solution of a substance ‘ $X$ ’ is used for white washing

i. Name the substance ‘ $X$ ’ and writes its formula.

Ans: The substance used for white washing is calcium oxide and its formula is $CaO$

ii. Write the reaction of the substance ‘ $X$ ’ named in (i) above with water.

Ans: The reaction for $CaO$ with water is: $CaO(s)+{{H}_{2}}O\to Ca{{(OH)}_{2}}(s)$

19. Which of the following statement about the reaction below are incorrect? $2PbO(s)+C(s)\to 2Pb(s)+C{{O}_{2}}(g)$

Lead is getting reduced.

Carbon dioxide is getting oxidized

Carbon is getting oxidized

Lead oxide is getting reduced

i. (a) and (b)

ii. (a) and (c)

iii. (a), (b) and (c)

iv. All

Ans: (i) Gain of oxygen is oxidation and loss of oxygen is reduction. Therefore, the statements (a) and (b) are incorrect and thus option (i) is correct.

20. In refining of silver, the recovery of silver from silver nitrate solution involved displacement by copper metal. Write down the reaction involved.

Ans: The reaction involved in refining of silver is $Cu(s)+2AgN{{O}_{3}}(aq)\to Cu{{(N{{O}_{3}})}_{2}}(aq)+2Ag(s)$

21. What do you mean by a precipitation reaction? Explain by giving examples.

Ans: A chemical reaction occurring in an aqueous solution in which an insoluble substance (precipitate) is formed is called precipitation reaction. For example, precipitation of silver chloride when aqueous silver nitrate is added to a solution containing potassium chloride.

$AgN{{O}_{3}}+NaCl\to AgCl+NaN{{O}_{3}}$

22. A shiny brown coloured element ‘ $X$ ’ on heating in air becomes black in colour. Name the element ‘ $X$ ’ and the black coloured compound formed.

Ans: The shiny brown coloured element ‘ $X$ ’ is copper. On heating in air, it forms copper oxide, which is black in colour. The chemical reaction for the above situation is:

$2CuS+{{O}_{2}}\to 2CuO$

23. Why do we apply paint on iron articles?

Ans: We apply paint on iron articles in order to prevent rusting. Due to this layer of paint, iron articles do not come in contact of atmospheric oxygen and react with it to form iron oxide. Thus, rusting is prevented.

24. Oil and fat containing food items are flushed with nitrogen. Why?

Ans: Oil and fat containing food items get rancid due to oxidation with atmospheric oxygen due to which the food gets an odour because of the formation of small volatile fatty acid molecules. To prevent this rancidity, food items are flushed with nitrogen. Nitrogen, being an inert gas, does not react with oil and fat containing items and therefore, acts as an antioxidant.

Short Answer Questions (3 Marks)

a). Define Rusting.

Ans: The formation of reddish-brown ferric oxides on the surface of iron when exposed to air for a long period of time in the presence of water at low temperature is called rusting.

b). Why do you apply paint on iron articles?

Ans: We apply paint on iron articles so that it forms a protective coating on the surface of iron and not come in contact directly with oxygen and water. It protects them against rusting.

2. White the balanced reactions for the following

A. \[\text{PotassiumBromide(aq)+Bariumiodide(aq)}\to \text{Potassiumiodide(aq)+BariumBromide(aq)}\]

Ans: $2KBr(aq)+Ba{{I}_{2}}(aq)\to 2KI(aq)+BaB{{r}_{2}}(aq)$

B. $\text{Zinccarbonate(s)}\to \text{Zincoxide(s)+carbondioxide(g)}$

Ans: $ZnC{{O}_{3}}(s)\to ZnO(s)+C{{O}_{2}}(g)$

C. $\text{Hydrogen(g)+chlorine(g)}\to \text{Hydrogenchloride}$

Ans: ${{H}_{2}}(g)+C{{l}_{2}}(g)\to 2HCl(g)$

3. The reaction is given by

$Zn+{{H}_{2}}S{{O}_{4}}\to ZnS{{O}_{4}}+{{H}_{2}}$

i. White the ionic equation for the reaction.

Ans: The ionic equation is: \ [Zn+2{{H}^{+}}\to Z{{n}^{2+}}+{{H}_{2}}\]

ii. The ionic equations can be represented by two half equations. Write these equations.

Ans: The two halves of the ionic equation representing one at cathode and another at anode are:\[Zn\to Z{{n}^{2+}}+2{{e}^{-}}\] \[2{{H}^{+}}+2{{e}^{-}}\to {{H}_{2}}\]

iii. Explain why this is a redox reaction.

Ans: A redox reaction is the one in which oxidation and reduction occur simultaneously. Here, from Zinc there is loss of electrons representing oxidation process and gain of electrons in hydrogen represent reduction. Therefore, this is a redox reaction.

4. What are neutralization reactions? Why are they named so? Give one example?

Ans: A neutralization reaction is the chemical reaction between an acid and a base. The products formed are water and salt.

Neutralization reactions are named so because acid and base neutralize each other in this type of reaction. For example, formation of sodium chloride and water by the reaction of \[HCl\] and \[NaOH\] .

\[HCl+NaOH\to NaCl+{{H}_{2}}O\]

5. Identify the type of reaction in the following

a). $ZnC{{O}_{3}}+2HCl\left( aq \right)\to ZnC{{l}_{2}}\left( aq \right)+{{H}_{2}}C{{O}_{3}}\left( aq \right)$

Ans: Double decomposition reaction.

b). $2NaBr\left( aq \right)+Cl\left( g \right)\to 2NaCl\left( aq \right)+B{{r}_{2}}\left( aq \right)$

Ans: Displacement reaction.

c). $2CuO\left( s \right)\underrightarrow{Heat}2Cu\left( s \right)+{{O}_{2}}\left( g \right)$

Ans: Decomposition reaction.

6. A student dropped few pieces of marble in dilute hydrochloric acid contained in a test tube. The evolved gas was then passed through lime water. What change would be observed in lime water? Write balanced chemical equation for both the change observed?

Ans: If a student dropped few pieces of marble in dilute hydrochloric acid contained in a test tube. Carbon dioxide gas is evolved. If this gas is passed through lime water insoluble Calcium carbonate is formed which turns the lime water milky. The solution will turn colourless after some time due to the formation of Calcium bicarbonate. The reactions involved are: \[CaC{{O}_{3}}\left( s \right)+2HCl\left( aq \right)\to CaC{{l}_{2}}\left( aq \right)+{{H}_{2}}O\left( l \right)+C{{O}_{2}}\left( g \right)\]

\[Ca{{\left( OH \right)}_{2}}+C{{O}_{2}}\left( g \right)\to CaC{{O}_{3}}+{{H}_{2}}O\left( l \right)\]

\[CaC{{O}_{3}}\left( s \right)+C{{O}_{2}}\left( g \right)+{{H}_{2}}O\left( l \right)\to Ca{{\left( HC{{O}_{3}} \right)}_{2}}\left( aq \right)\]

7. In the reaction $Mn{{O}_{2}}+4HCl\to MnC{{l}_{2}}+{{H}_{2}}O+C{{l}_{2}}$

a) Name the substance oxidised.

Ans: In the given reaction \[HCl\] is oxidised to \[C{{l}_{2}}\] .

b) Name the oxidising agent.

Ans: The oxidising agent is \[Mn{{O}_{2}}\]

c) Name the reducing agent and the substance reduced.

Ans: The reducing agent is \[HCl\] and here, \[Mn{{O}_{2}}\] is oxidised to \[MnC{{l}_{2}}\].

8. Give one example each of

a) Thermal decomposition

Ans: An example of Thermal decomposition is

\[MgC{{O}_{3}}\left( s \right)\underrightarrow{Heat}MgO\left( s \right)+C{{O}_{2}}\left( g \right)\]

b) Electrolytic decomposition

Ans: An example of Electrolytic decomposition is \[2{{H}_{2}}O\left( l \right)\underrightarrow{ElectricCurrent}2{{H}_{2}}\left( g \right)+{{O}_{2}}\left( g \right)\]

c) Photo decomposition

Ans: An example of Photo decomposition is \[2{{H}_{2}}{{O}_{2}}\left( l \right)\underrightarrow{Light}{{H}_{2}}O\left( l \right)+{{O}_{2}}\left( g \right)\]

9. Write three equations for decomposition reaction where energy is supplied in the form of heat, light and electricity?

Ans: The three equations for decomposition reaction where energy is supplied in the form of heat, light and electricity are:

i. \[MgC{{O}_{3}}\left( s \right)\underrightarrow{Heat}MgO\left( s \right)+C{{O}_{2}}\left( g \right)\]

ii. \[2AgCl\underrightarrow{Light}2Ag+C{{l}_{2}}\]

iii. \[2NaCl\underrightarrow{Electricity}2Na+C{{l}_{2}}\]

10. When you mix solutions of lead (II) nitrate and potassium iodide,

i. What is the colour of the precipitate formed? Name the compound evolved?

Ans: The precipitate formed here is lead(II) Iodide which is yellow in colour.

ii. Write a balanced chemical reaction?

Ans: The balanced chemical reaction is: \[Pb{{\left( N{{O}_{3}} \right)}_{2}}\left( aq \right)+2KI\left( aq \right)\to Pb{{I}_{2}}\left( s \right)+2KN{{O}_{3}}\left( aq \right)\]

iii. Is this a double displacement reaction?

Ans: Yes, this is a double displacement reaction because both the compounds are getting displaced.

11. Transfer the following into chemical equations and balance them.

i. Hydrogen gas combines with nitrogen to from ammonia.

Ans: \[3{{H}_{2}}+{{N}_{2}}\to 2N{{H}_{3}}\]

ii. Hydrogen sulphide gas burns in air to give water and sulphur dioxide.

Ans: \[2{{H}_{2}}S+3{{O}_{2}}\to 2{{H}_{2}}O+2S{{O}_{2}}\]

iii. Potassium metal reacts with water to give potassium hydroxide and hydrogen gas.

Ans: \[2K+2{{H}_{2}}O\to 2KOH+{{H}_{2}}\].

12. Balance the equations

i. $HN{{O}_{3}}+Ca{{\left( OH \right)}_{2}}\to Ca{{\left( N{{O}_{3}} \right)}_{2}}+{{H}_{2}}O$

Ans: $2HN{{O}_{3}}+Ca{{\left( OH \right)}_{2}}\to Ca{{\left( N{{O}_{3}} \right)}_{2}}+2{{H}_{2}}O$

ii. $NaCl+AgN{{O}_{3}}\to AgCl+NaN{{O}_{3}}$

Ans: $NaCl+AgN{{O}_{3}}\to AgCl+NaN{{O}_{3}}$

iii. $BaC{{l}_{2}}+{{H}_{2}}S{{O}_{4}}\to BaS{{O}_{4}}+HCl$

Ans: $BaC{{l}_{2}}+{{H}_{2}}S{{O}_{4}}\to BaS{{O}_{4}}+2HCl$

13. A compound ‘ $X$ ’ is used for drinking, has $pH=7$ . Its acidified solution undergoes decomposition in presence of electricity to produce gases ‘ $Y$ ’ and ‘ $Z$ ’. The volume of $Y$ is double than $Z$ . $Y$ is highly combustible whereas $Z$ is supporter of combustion. Identify $X$ , $Y$ & $Z$ and write the chemical reactions involved.

Ans: In the given situation, $X={{H}_{2}}O$ , $Y={{H}_{2}}$ and $Z={{O}_{2}}$ . The chemical reaction involved is: $2{{H}_{2}}O\left( l \right)\to {{H}_{2}}\left( g \right)+{{O}_{2}}\left( g \right)$

14. An aqueous solution of metal nitrate $P$ reacts with sodium bromide solution to form yellow ppt of compound $Q$ which is used in photography. $Q$ on exposure to sunlight undergoes decomposition reaction to form metal present in $P$ along with reddish brown gas. Identify $P$ & $Q$ . Write the chemical reaction & type of chemical reaction.

Ans: In the given situation, $P=AgN{{O}_{3}}$ , $Q=AgBr$ . The chemical reaction involved is a photochemical reaction which is as follows: $2AgBr\left( s \right)\to 2Ag\left( s \right)+B{{r}_{2}}\left( g \right)$

15. Bhawana took a pale green substance $A$ in a test tube. And heated it over the flame of a burner. A brown coloured residue $B$ was formed along with evolution of two gases with burning smell of sulphur. Identify $A$ & $B$ . Write the chemical reaction involved.

Ans: In the given situation, $A=FeS{{O}_{4}}$ , $B=F{{e}_{2}}{{O}_{3}}$ . The chemical reaction involved is: $2FeS{{O}_{4}}\left( s \right)\to F{{e}_{2}}{{O}_{3}}\left( s \right)+S{{O}_{2}}\left( g \right)+S{{O}_{3}}\left( g \right)$

16. A reddish-brown vessel developed a green-colored solid $X$ . When left open in air for a long time. When reacted with $dil.{{H}_{2}}S{{O}_{4}}$ , it forms a blue-colored solution along with brisk efficient due to colourless & odourless gas $Z$ . $X$ decomposes to form black-colored oxide $Y$ of a reddish-brown metal along with gas $Z$ , Identify $X$ , $Y$ , & $Z$ .

Ans: In the given situation, $X=CuC{{O}_{3}}$ , $Y=CuO$ and $Z=C{{O}_{2}}$ .

17. A student has mixed the solutions of lead (II) nitrate and potassium iodide.

i. What was the colour of the precipitate formed? Can you name the compound?

ii. Write the balanced chemical equation for this reaction.

iii. What type of reaction is it?

Ans: This is a double displacement reaction because both the compounds are getting displaced.

18. Name the type of reaction seen in the diagram below. Write the reaction for the same.

Ans: The type of reaction is displacement reaction. \[Fe\left( s \right)+CuS{{O}_{4}}\to FeS{{O}_{4}}\left( aq \right)+Cu\]

19. A student dropped few pieces of marble in $dil.HCl$contained in a test tube. The gas evolved was passed through lime water. What change would be observed in lime water? Write chemical reactions for both the changes observed.

20. Astha has been collecting silver coins and copper coins. One day she observed a black Coating on silver coins and a green coating on copper coins. Which chemical phenomenon is responsible for these coatings? Write the chemical name of black and green coatings?

Ans: Corrosion is responsible for the black coating on silver and green coating on copper. The chemical name of the black coating formed is $A{{g}_{2}}S$ and the green coating formed is due to $CuC{{O}_{3}}.Cu{{\left( OH \right)}_{2}}$ .

21. Write the balance equation for the following reactions.

i. Hydrogen + Chlorine -> Hydrogen chloride

Ans: ${{H}_{2}}+C{{l}_{2}}\to 2HCl$

ii. Barium chloride + Aluminium sulphate -> Barium sulphate + Aluminium chloride

Ans: $3BaC{{l}_{2}}+A{{l}_{2}}{{\left( S{{O}_{4}} \right)}_{3}}\to 3BaS{{O}_{4}}+2AlC{{l}_{3}}$

iii. Sodium + water -> Sodium hydroxide + water

Ans: $2Na+2{{H}_{2}}O\to 2NaOH+{{H}_{2}}$

22. $F{{e}_{2}}{{O}_{3}}+2Al\to A{{l}_{2}}{{O}_{3}}+2Fe$

The above reaction is an example of a

combination reaction

double displacement reaction

decomposition reaction

displacement reaction

Ans: (d) This is an example of displacement reaction because $Fe$ in $Fe{{O}_{3}}$ has been displaced by $Al$ .

23. What is balanced chemical equation? Why should chemical equation be balanced?

Ans: The representation of a chemical reaction in which the number of atoms of each element is equal on the reactant side and product side is called balanced chemical equation. Chemical reaction should be balanced because only a balanced equation tells us the relative quantities of different reactants and products involved in the reaction.

24. Why respiration is considered an exothermic reaction? Explain.

Ans: Reactions which release heat or energy are called exothermic reactions. Respiration is considered an exothermic reaction because when we breathe out heat is liberated. During respiration, we inhale oxygen from the atmosphere which reacts with glucose in your body cells to produce carbon dioxide and water.

Long Answer Questions (5 Marks)

1. You are given with

$CuS{{O}_{4}}$ solution

$BaC{{l}_{2}}$

$Cu$ Powder

Ferrous sulphate crystal

Quick lime.

Make five reactions that can take place from these materials.

Ans: Five reactions possible from the given materials are:

i. $BaC{{l}_{2}}\left( aq \right)+CuS{{O}_{4}}\left( aq \right)\to BaS{{O}_{4}}\left( s \right)+CuC{{l}_{2}}\left( aq \right)$

ii. $2Cu\left( s \right)+{{O}_{2}}\left( g \right)\to 2CuO\left( s \right)$

iii. $2FeS{{O}_{4}}\left( s \right)\underrightarrow{heat}F{{e}_{2}}{{O}_{3}}+S{{O}_{2}}+S{{O}_{3}}$

iv. $2FeS{{O}_{4}}.7{{H}_{2}}O\underrightarrow{heat}Ca{{\left( OH \right)}_{2}}\left( s \right)+Heat$

v. $CaO\left( s \right)+{{H}_{2}}O\to Ca{{\left( OH \right)}_{2}}\left( s \right)+Heat$

2. A metal is heated with $dil.{{H}_{2}}S{{O}_{4}}$ . The gas evolved is collected by the method shown in the figure: Answer the following

Name the gas.

Ans: The gas evolved is ${{H}_{2}}$ .

Name the method of collection of gas.

Ans: Gas is collected by downward displacement method.

Is the gas soluble or insoluble in water?

Ans: The gas is insoluble in water since it is collected over water and does not get dissolved.

Is the gas lighter or heavier than air?

Ans: The gas is lighter than air as it floats above.

3. With the help of an activity show that iron is more reactive than copper?

Ans: To show that iron is more reactive than copper, take a test tube and pour some copper sulphate solution into it. Now, drop some iron nails into this solution and wait for some time. You will notice that the solution turns blue and the nails become reddish-brown. This is because of the displacement of copper from copper sulphate solution. The brown deposit is of copper. The chemical reaction involved in this experiment is:

\[Fe\left( s \right)+CuS{{O}_{4}}\to FeS{{O}_{4}}\left( aq \right)+Cu\]

4. Observe the following activity & answer the questions

Do you observe anything happening around the zinc granules?

Ans: Bubbles of hydrogen gas evolve around zinc granules.

Is there any change in its temperature?

Ans: Yes, temperature will increase after reaction.

Why is glass tube not dipped in $dil.{{H}_{2}}S{{O}_{4}}$ ?

Ans: If glass tube is dipped in $dil.{{H}_{2}}S{{O}_{4}}$ , then the level of ${{H}_{2}}S{{O}_{4}}$ will rise in the glass tube preventing hydrogen gas to evolve.

How is ${{H}_{2}}$ gas collected by downward displacement or upward displacement of water?

Ans: Hydrogen gas is collected by downward displacement of water.

Is ${{H}_{2}}$ gas soluble or insoluble in water?

Ans: Hydrogen gas is insoluble in water.

Is ${{H}_{2}}$ gas heavier or lighter than air?

Ans: Hydrogen gas is lighter than air.

5. A reddish-brown metal $X$ when heated in presence of oxygen forms a black compound $Y$ Which is basic in nature when heated with hydrogen gas gives back X. Identify $X$ & $Y$ . Write the chemical reaction between $Y$ & ${{H}_{2}}$ . Identify the substance being oxidized & reduced.

Ans: Here, $X=Cu$ and $Y=CuO$ .

Chemical reaction between copper oxide and hydrogen is

\[2Cu\left( s \right)+{{O}_{2}}\left( g \right)\to 2CuO\left( s \right)\]

\[CuO+{{H}_{2}}\underrightarrow{heat}Cu+{{H}_{2}}O\]

During this reaction, copper oxide is getting reduced as it is losing oxygen and hydrogen is getting oxidised as it is gaining oxygen.

6. Why does the colour of copper sulphate solution change when an iron nail is dipped in it?

Ans: The colour of copper sulphate solution change when an iron nail is dipped in it because of the displacement of copper from copper sulphate solution and formation of iron sulphate solution. The brown deposit is of copper. The chemical reaction involved in this experiment is: \[Fe\left( s \right)+CuS{{O}_{4}}\to FeS{{O}_{4}}\left( aq \right)+Cu\]

7. Identify the substances that are oxidized and the substances that are reduced in the following reactions.

a. $4Na\left( s \right)+{{O}_{2}}\left( g \right)\to 2N{{a}_{2}}O\left( s \right)$

Ans: In this reaction, sodium is oxidised because it is combined with oxygen and oxygen molecule is reduced because it is losing an oxygen atom to convert into sodium oxide.

b. $CuO\left( s \right)+{{H}_{2}}\to Cu\left( s \right)+{{H}_{2}}O\left( l \right)$

Ans: In this reaction, hydrogen is getting oxidised because it is combined with oxygen to form water and copper oxide is reduced because it is losing an oxygen atom to convert into copper.

8. Translate the following statements into chemical equations and then balance them.

a) Hydrogen gas combines with nitrogen to form ammonia.

Ans: The balanced chemical equation is:

\[3{{H}_{2}}+{{N}_{2}}\to 2N{{H}_{3}}\]

b) Hydrogen sulphide gas burns in air to give water and Sulphur dioxide.

\[2{{H}_{2}}S+3{{O}_{2}}\to 2{{H}_{2}}O+2S{{O}_{2}}\]

c) Barium chloride reacts with aluminium sulphate to give aluminium chloride and precipitate of barium sulphate.

\[3BaC{{l}_{2}}+A{{l}_{2}}{{\left( S{{O}_{4}} \right)}_{3}}\to 2AlC{{l}_{3}}+3BaS{{O}_{4}}\]

9. Balance the following chemical equations:

a) $HN{{O}_{3}}+Ca{{\left( OH \right)}_{2}}\to Ca{{\left( OH \right)}_{2}}.Ca{{\left( N{{O}_{3}} \right)}_{2}}+{{H}_{2}}O$

$2HN{{O}_{3}}+Ca{{\left( OH \right)}_{2}}\to Ca{{\left( OH \right)}_{2}}.Ca{{\left( N{{O}_{3}} \right)}_{2}}+2{{H}_{2}}O$

c) $NaOH+{{H}_{2}}S{{O}_{4}}\to N{{a}_{2}}S{{O}_{4}}+{{H}_{2}}O$

$2NaOH+{{H}_{2}}S{{O}_{4}}\to N{{a}_{2}}S{{O}_{4}}+2{{H}_{2}}O$

d) $NaCl+AgN{{O}_{3}}\to AgCl+NaN{{O}_{3}}$

$NaCl+AgN{{O}_{3}}\to AgCl+NaN{{O}_{3}}$

e) $BaC{{l}_{2}}+{{H}_{2}}S{{O}_{4}}\to B{{a}_{2}}S{{O}_{4}}+HCl$

$BaC{{l}_{2}}+{{H}_{2}}S{{O}_{4}}\to B{{a}_{2}}S{{O}_{4}}+2HCl$

10. Write the balanced chemical equations for the following reactions.

a) Calcium hydroxide + Carbon dioxide -> Calcium carbonate + Water

b) Zinc + Silver nitrate -> Zinc nitrate + Silver

$Zn+2AgN{{O}_{3}}\to Zn{{\left( N{{O}_{3}} \right)}_{2}}+2Ag$

c) Aluminum + Copper chloride -> Aluminum chloride +Copper

$2Al+3C{{l}_{2}}\to 2AlC{{l}_{3}}+3Cu$

d) Barium chloride + Potassium sulphate -> Barium sulphate + potassium chloride

\[BaC{{l}_{2}}+{{K}_{2}}S{{O}_{4}}\to BaS{{O}_{4}}+2KCl\]

11. Write the balanced chemical equation for the following and identify the type of reaction in each case.

a) Potassium bromide (s) + Barium iodide (aq) -> Potassium iodide (aq) + Barium bromide(s)

\[2KBr\left( aq \right)+Ba{{I}_{2}}\to 2KI\left( aq \right)+B{{r}_{2}}\]

This is a displacement reaction.

b) Zinc carbonate (s) -> Zinc oxide (s) + Carbon dioxide (g)

\[Zn{{O}_{3}}\left( s \right)\to ZnO\left( s \right)+C{{O}_{2}}\left( g \right)\]

This is a decomposition reaction.

c) Hydrogen (g) + Chlorine (g) -> Hydrogen chloride (g)

\[{{H}_{2}}\left( g \right)+C{{l}_{2}}\left( g \right)\to 2HCl\]

This is a combination reaction.

d) Magnesium (s) + Hydrochloric acid (aq) -> Magnesium chloride (aq) + Hydrogen (g)

\[Mg\left( s \right)+2HCl\left( aq \right)\to MgC{{l}_{2}}+{{H}_{2}}\left( g \right)\]

12. What does one mean by exothermic and endothermic reactions? Give examples.

Ans: A reaction in which energy is released in the form of heat or light is called exothermic reaction. For example,

\[C{{H}_{4}}+2{{O}_{2}}\to C{{O}_{2}}+2{{H}_{2}}O+heat\]

\[2Al+Fe{{O}_{3}}\to A{{l}_{2}}{{O}_{3}}+Fe+heat\]

A reaction in which energy is absorbed from the surrounding and cooling is produced is called endothermic reaction. For example,

\[CaC{{O}_{3}}\to CaO+C{{O}_{2}}\]

\[{{N}_{2}}+{{O}_{2}}\to 2NO\]

13. Why decomposition reactions are called the opposite of combination reactions? Write equations for these reactions.

Ans: In a decomposition reaction, a single substance breaks down into two or more substances while in a combination reaction, two or more substances react to produce one substance. Therefore, decomposition reactions are called opposite of combination reactions.

For example,

Decomposition reaction: \[CaC{{O}_{3}}+CuS{{O}_{4}}\to ZnS{{O}_{4}}+Cu\]

Combination reaction: \[CaO+{{H}_{2}}O\to Ca{{\left( OH \right)}_{2}}\]

14. Write one equation each for decomposition reactions where energy is supplied in the form of heat, light or electricity.

Ans: The equation for decomposition reaction by heat is:

\[CaC{{O}_{3}}+heat\to CaO+C{{O}_{2}}\]

The equation for decomposition reaction by light is:

\[2AgBr+light\to 2Ag+B{{r}_{2}}\]

The equation for decomposition reaction by electricity is:

\[2{{H}_{2}}O+electricity\to 2{{H}_{2}}+{{O}_{2}}\]

15. What is difference between displacement and double displacement reactions? Write equations for these reactions.

Ans: In displacement reaction, more reactive element displaces the less reactive element from its compound. For example,

$Zn(s)+CuS{{O}_{4}}\left( aq \right)\to ZnS{{O}_{4}}(aq)+Cu(s)$

Whereas in double displacement reaction, exchange of ions takes place between the compounds. For example,

$HCl\left( aq \right)+AgN{{O}_{3}}\left( aq \right)\to AgCl\left( s \right)+HN{{O}_{3}}\left( aq \right)$

16. Explain the following in terms of gain and loss of oxygen with two examples each?

a) Oxidation

Ans: The process of addition of oxygen or removal of hydrogen in a chemical reaction is called oxidation reaction. For example,

\[2Cu\left( s \right)+{{O}_{2}}\left( g \right)\to 2CuO\left( s \right)\] , here copper is oxidised into copper oxide

\[2Mg\left( s \right)+{{O}_{2}}\left( g \right)\to 2MgO\left( s \right)\] , here magnesium is oxidised into magnesium oxide

b) Reduction

Ans: The process of addition of hydrogen or removal of oxygen in a chemical reaction is called oxidation reaction. For example,

\[CuO+{{H}_{2}}\left( g \right)\to Cu+{{H}_{2}}O\] , here copper oxide is reduced to copper

\[{{H}_{2}}S+C{{l}_{2}}\to 2HCl+S\] , here chloride is reduced to hydrogen chloride

17. Explain the following terms with one example each.

a) Corrosion

Ans: Corrosion is defined as a process where a metal reacts with water, air or acid to form oxides and carbonates. This is also known as rusting. For example, black coating on silver in the presence of air or atmosphere.

b) Rancidity

Ans: Rancidity is the process of oxidation of fats and oils when kept in open or in presence of oxygen for a long time. Due to this change in taste and odour of food can be observed. To prevent rancidity food items are flushed with nitrogen or kept in airtight containers. For example, the taste and smell of butter changes when kept for long.

Chemical Reactions and Equations Class 10 Important Questions - Free PDF Download

Students who are weak in studies find science subjects confusing and challenging. Sometimes you find it challenging to understand the chemical symbols and chemical equations. Chapter 1 of science is full of theories and different types of chemical equations and reactions, which makes it confusing for you to understand the chapter without proper notes and study material. The equations are sometimes difficult to understand and bars you from securing good marks in the exams. The best way to get hold of the chapter is by practising the important question. So, we at Vedantu have designed the Class 10 Science Ch 1 Important Question with answers PDF for your betterment. These important questions are prepared as per the chapter requirement and according to the CBSE guidelines.

Students who are confused and face difficulty in Chapter 1 of Science can refer to the Chemical reactions and equations important questions. It will clarify their doubts as well as help them understand the pattern of examination.

Class 10 Chapter 1 Science Important Questions

Chapter 1 Chemical reactions and equations of science, will explain the students about various types of reactions that take place in our surroundings. This chapter will also explain the students, the ways to write a chemical equation using words as well as symbols. By practising the Important Questions of Chemical Reactions and Equations Class 10, students can get a detailed overview of the chapter. Some topics that the chapter cover are as follows:

Physical Changes and Chemical Changes

Chemical Change - A chemical change is a type of change where one or more new substances are formed with different physical and chemical properties. Generally, this type of change is irreversible and permanent in nature.

For example, when iron reacts with copper sulphate solutions, ferrous sulphate and copper are obtained as the by-product of the reaction.

Physical Change - A change where no new substance is formed. In this type of change, only the physical properties such as colour, shape or size are of the reactants change. These changes are reversible and temporary in nature.

For example, boiling of water, where water changes into water vapour on boiling.

Chemical Reaction

A chemical reaction is when one or more substances react and give rise to one or more substances as a product. The substances so formed can either be chemical elements or compounds. After undergoing a chemical reaction, the reactant’s atomic constitution changes to develop a different substance.

The Determinant of a Chemical Reaction

There are several factors that can help us determine a chemical reaction, and they are:

In a chemical reaction, there can be an evolution of gas.

In a chemical reaction, there can be a significant change in temperature.

A precipitate is formed in a chemical reaction.

Change in colour of the reactants.

Change in the state of the reactants.

Types of Chemical Reaction

There are various types of chemical reactions depending upon multiple factors. The chemical reactions are as follows:

Combination reaction.

Decomposition reaction.

Single Displacement reaction.

Double Displacement reaction.

Redox Reaction.

Endothermic reaction.

Exothermic reaction.

Neutralisation reaction.

Precipitation reaction.

Chemical Equations

A Chemical equation is a symbolic representation of chemical reactions that involve chemical formulas and symbols. It involves both the reactants and products. The reactants are written on the left side, while the products are written on the right side of the equation.

Chemical Symbols and Valencies

Chemical Symbol is a chemical representation given to an element. Each chemical symbol has two letters which are the abbreviated form of the element’s name.

For example, The chemical symbol of Zinc is Zn.

Valency refers to the combining capacity of an element. It can be defined as the number of electrons gained or lost by an atom while it undergoes a chemical reaction.

Writing a Chemical Equation

While writing a chemical reaction, we should keep some rules in mind, and those rules are as follows:

The reactants are written on the left side of the equation.

The products are written on the right side of the equation.

For solids, we write (s).

For liquids, we write (l).

For gas, we write (g).

For aqueous solution, we write (aq).

If gas is produced in a reaction, we represent it by (↑).

If a precipitate is produced in a reaction, we represent it by (↓).

Balanced Chemical Equation

A chemical equation is said to be balanced when the number of atoms of the elements on the reactant side is equal to the number of atoms of the elements on the product side. There are certain steps that you can follow to balance a chemical equation, and they are:

Make a list of each element involved in the equation.

Then identify the number of atoms present in each element on both reactant and product side.

Multiply the number of atoms to make both reactants and product side equal.

Place the coefficient in front of the reactants and product elements, so obtained from the multiplication.

Check the equation to assure that it is balanced.

Unbalanced Chemical Equation - CaCo 3 + H 3 PO 4 → Ca 3 (PO 4 ) 2 + H 2 Co 3

Balanced Chemical Equation - 3CaCo 3 + 2H 3 Po 4 → Ca 3 (Po 4 ) 2 + 3H 2 Co 3

Important Questions of Chapter 1 Science Class 10

To provide you with a proper understanding of what to study for science, we have provided some Important Questions for Class 10 Science Chapter 1 in this article. You can refer to these questions and boost your exam preparation.

What is a Chemical Change?

What is a Physical Change?

What do you mean by a chemical reaction?

What are the different types of Chemical reactions?

What is a Neutralisation reaction?

What do you mean by double displacement reaction?

Give an example of Decomposition reaction.

What is the meaning of the combination reaction?

Write in brief about the endothermic reaction.

Explain with an example, the meaning of exothermic reaction.

What is the meaning of redox reaction?

What is a Single Displacement reaction? Give an example.

Differentiate between single displacement and double displacement reaction.

What are the steps to write a chemical equation?

What do you mean by a precipitation reaction?

How to balance a chemical equation?

What is the meaning of a word equation?

Benefits of Class 10 Science Chapter 1 Important Questions

The Chemical Reactions and Equations Class 10 Important Questions are the most useful study material that you can refer to for securing better maks. These questions are prepared by experts at Vedantu to provide the students with a proper explanation of the chapter.

Our expert team has done proper research before preparing these important question, so the questions have a high probability of coming in the examinations.

The questions are provided with proper answers which will help the students to understand the chapter and secure better grades.

By referring to these questions and answers, the students can have a good grip on the chapter.

Lastly, the important questions cover all the necessary topics and are prepared as per the latest guidelines of the CBSE board . It makes these questions a reliable and trustable source of information.

The Class 10 Science Ch 1 Important Questions are simplified, and most suitably designed study material for class 10 students. These questions cover each topic given under the chapter and will help make the learning process easier for the students. The questions are in an orderly manner and will make it easier for the students to understand the chapter. Referring to these questions will give you a competitive edge in the examination and will help you secure better grades. By practising these questions, the students can know the pattern of questions and the type of questions that might come in the examination. So, download the important questions PDF from the Vedantu portal now and start your exam preparations.

Important Related Links for CBSE Class 10 Science

FAQs on Important Questions for CBSE Class 10 Science Chapter 1 - Chemical Reactions and Equations 2024-25

1. What are the important questions of Chapter 1 of Class 10 Science?

Ans: The following are the important questions of Chapter 1 of Class 10 Science-

Differentiate between single displacement and double displacement reactions.

What is the meaning of the redox reaction?

Give an example of a Decomposition reaction.

For Important Questions of Chapter 1 of Class 10 Science, visit Vedantu website or mobile app and download it free of cost.

2. What is the first Chapter of Class 10 Science?

Ans: Chapter 1 “Chemical Reactions and Science Equations” will teach students about the different types of reactions that occur in our environment. This section will also educate them on how to create chemical formulas using both words and symbols. Students may gain a thorough grasp of the subject by practicing the Important Questions of Chapter 1-Chemical Reactions and Equations of Class 10 Science. You will learn about the chemical and physical changes that occur as a result of a reaction.

3. What is a chemical change?

Ans: A chemical change occurs when one or more new compounds with differing physical and chemical characteristics are created. If two elements react with each other to form a new compound. Both element’s individual properties are lost. The resultant compound has its own new properties which can be similar to the reactants or completely different. In most cases, this sort of alteration is irreversible and permanent. When iron interacts with CuSO 4 solutions, for example, ferrous sulphate and copper are produced as by-products.

4. What is a chemical reaction?

Ans: When one or more chemicals react and produce one or more substances as a product, this is known as a chemical reaction. Reactants react in such a form that they are chemically combined in order to find a new compound. Chemical elements or compounds can be produced as a result of this process. The atomic composition of the reactant changes when it undergoes a chemical reaction, resulting in the formation of new material. For more information about this topic, visit Vedantu .

5. What are Chemical Symbols and Valencies?

Ans: A chemical symbol is a description of an element's chemical properties. Each chemical symbol consists of two characters that represent the element's name in an altered version. Magnesium, for example, has the chemical symbol Mg while Carbon has the chemical symbol C. The joining capability of an element is referred to as valency. The number of electrons acquired or lost by an atom during a chemical reaction is known as the number of electrons gained or lost.

CBSE Class 10 Science Important Questions

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CBSE 10th Standard Science Subject Case Study Questions

By QB365 on 21 May, 2021

QB365 Provides the updated CASE Study Questions for Class 10 , and also provide the detail solution for each and every case study questions . Case study questions are latest updated question pattern from NCERT, QB365 will helps to get more marks in Exams

QB365 - Question Bank Software

10th Standard CBSE

Final Semester - June 2015

Redox reactions are those reactions in which oxidation and reduction occur Simultaneously. A redox reaction is made up of two half reactions. In the first half reaction, oxidation takes place and in second half reaction, reduction occurs. Oxidation is a process in which a substance loses electrons and in reduction, a substance gains electrons. The substance which gains electrons is reduced and acts as an oxidising agent. On the other hand, a substance which loses electrons is oxidised and acts as a reducing agent. (i) Which of the following is a redox reaction?

(ii) Identify the reaction in which H2 02 is acting as a reducing agent.

(iii) For the following reactions, identify the one in which H 2 S acts as a reducing agent.

(iv) For the following reaction, identify the correct statement. $\mathrm{ZnO}+\mathrm{CO} \longrightarrow \mathrm{Zn}+\mathrm{CO}_{2}$

(v) In the following reaction, which substance is reduced? $\mathrm{PbS}+4 \mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow \mathrm{PbSO}_{4}+4 \mathrm{H}_{2} \mathrm{O}$

(ii) If the pH of a solution is 8, then its [H + ] ion is

(iii) In terms of acidic strength, which one of the following is in the correct increasing order?

(iv) Which of the following compounds does not give H + ions in aqueous solution?

(v) Four solutions labelled as P, Q, Rand Shave pH values 1, 9, 3 and 13 respectively. Which of the following statements about the given solutions is incorrect?

Baking powder produces carbon dioxide on heating, so it is used in cooking to make the batter spongy. Although, baking soda also produces CO 2 on heating, but it is not used in cooking because on heating, baking soda produces sodium carbonate along with carbon dioxide. Sodium carbonate, thus, produced, makes the taste bitter. Baking powder is the mixture of baking soda and a mild edible acid. Generally, tartaric acid is mixed with baking soda to make baking powder. When baking powder is heated, NaHCO 3 decomposes to give CO 2 which makes bread and cake fluffy. Tartaric acid helps to remove bitter taste due to formation of sodium tartrate. $2 \mathrm{NaHCO}_{3}+ \ \ \mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{6} \quad \longrightarrow \quad 2 \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{Na}_{2} \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{6}$ Baking soda Tartaric acid Carbon dioxide Sodium tartrate (i) On passing excess CO 2 gas in aqueous solution of sodium carbonate, the substance obtained is

(ii) When sodium hydrogen carbonate is added to acetic acid, it evolves a gas. Which of the following statements are true about the gas evolved? (I) It turns lime water milky (II) It extinguishes a burning splinter (III) It dissolves in a solution of sodium hydroxide (IV) It has a pungent odour

(iii) Select the correct statement regarding sodium hydrogen carbonate.

(iv) Acetic acid was added to a solid X kept in a test tube. A colourless and odourless gas was evolved. The gas was passed through lime water which turned milky. It was concluded that

(v) Which of the following statements are correct regarding baking soda? (I) Baking soda is sodium hydrogen carbonate (II) On heating, baking soda gives sodium carbonate (III) It is used for manufacture of soap (IV) It is an ingredient of baking powder

The chemical reactivity of an element depends upon its electronic configuration. All elements having less than eight electrons in the outermost shell show chemical reactivity. During chemical reactions, atoms of all elements tend to achieve a completely filled valence shell. Metals are electropositive in nature. They have tendency to lose one or more electrons present in the valence shell of their atoms to form cations and achieve nearest noble gas configuration. The compounds formed by the transfer of electrons from one element to other are known as ionic or electrovalent compounds. (i) The electronic configurations of three elements X, Y and Z are: X : 2 Y: 2, 8, 7 Z : 2, 8, 2 Which of the following is correct regarding these elements?

(ii) Element X reacts with element Y to form a compound Z. During the formation of compound Z, atoms of X lose one electron each whereas atoms of Y gain one electron each. Which of the following properties is not shown by compound Z?

(iii) Which of the following is correct representation of formation of magnesium chloride?

(iv) The electronic configuration of sodium ion is

(v)Which of the following represents an electropositive element?

A hydrocarbon (P) has the molecular formula C 10 H 22 .A hydrocarbon (Q) has two carbon atoms less than (P) and belong to the same homologous series. A hydrocarbon (R) has two carbon atoms more than (P) and belong to the same homologous series. (i) What is the molecular formula of (Q) ?

(ii) To which homologous series do the compound (P), (Q) and (R) belong?

(iii) What is the molecular formula of (R) ?

(iv) Identify the correct statement about compounds (P), (Q) and (R) .

(v) Compounds (P), (Q) and (R) are

The recurrence of properties of the elements after a certain regular intervals, when they are arranged in the increasing order of their atomic numbers, is called periodicity. There are a number of physical properties such as atomic size, metallic and non -metallic character, etc. which show periodic variation. In periodic table, various properties vary differently from moving left to right in a period and going down in a group. In a period, properties vary because from moving left to right in a period, number of shells remain same but valence electron increases by one number hence nuclear charge increases. In a group, on going down, number of valence shells increases while number of valence electrons remains same. (i) From top to bottom in a group of the periodic table, the electropositive character of the element

(ii) Which element has the largest size in the second period?

(iii) Which of the following elements has three valence electrons?

(iv) In the periodic table, the metallic character of elements (a) decreases from left to right and decreases down the group (b) decreases from left to right and increases down the group (c) increases from left to right and increases down the group (d) increases from left to right and decreases down the group (v) Which of the following increases along the period?

The small intestine is the longest part of the alimentary canal. It is a narrow tube of about 6 metres which lies coiled in the abdomen. The length of small intestine varies in different animals depending on the type of food they eat. (i) Humans are not able to digest cellulose whereas they are able to digest starch due to

(iii) Butter cannot be digested in the stomach as lipase and bile are(a) released in small intestine

(iv) Which of the following is a correct statement? (a) Herbivores have shorter small intestine as they eat grasses (b) Carnivores have larger small intestine as they eat meat (c) Herbivores have larger small intestine as they eat grasses (d) None of these (v) Various types of movements are generated by the ______ layer of the small intestine.

(iii) Which of the following animals shows double circulatory pathway?

(v) Select the option which properly represents pulmonary circulation in humans. $\text { (a) Left auricle } \frac{\text { Deoxygenated }}{\text { blood }}{\longrightarrow} \text { Lungs } \frac{\text { Oxygenated }}{\text { blood }} \text { Right ventricle }$ $\text { (b) Left auricle } \frac{\text { Oxygenated }}{\text { blood }}{\longrightarrow} \text { Lungs } \frac{\text { Deoxygenated }}{\text { blood }}{\longrightarrow} \text { Right ventricle }$ $\text { (c) Right ventricle } \frac{\text { Deoxygenated }}{\text { blood }}{\longrightarrow} \text { Lungs } \frac{\text { Oxygenated }}{\text { blood }} \rightarrow \text { Left auricle }$ $\text { (d) Right ventricle } \frac{\text { Oxygenated }}{\text { blood }}>\text { Lungs } \frac{\text { Deoxygenated }}{\text { blood }} \gg \text { Left auricle }$

Spore formation, method of asexual reproduction is used by unicellular as well as multicellular organisms.Spores are microscopic units which could be air borne or are present in soil, etc. (i) A slice of bread kept in open for sometime shows growing white cottony mass which later turns black. This happens because (a) bacterial spores present in air germinate on the surface of bread slice (b) fungal spores present in air germinate on the surface of bread slice (c) protozoan microbes start feeding on bread slice (d) none ef these. (ii) Spore formation can be seen in

(iii) Bulb like structure at top of erect hyphae where spores are produced is

Gregor Mendel conducted hybridisation experiments on garden peas for seven years and proposed the laws of inheritance in living organisms. He investigated characters in the garden pea plant that were manifested as two opposing traits, e.g., tall or dwarf plants, yellow and green seeds, etc. (i) Among the seven pairs of contrasting traits in pea plant as studied by Mendel, the number of traits related to flower, pod and seed respectively were

(ii) The colour based contrasting traits in seven contrasting pairs, studied by Mendel in pea plant were

(iii) Refer to the given table of contrasting traits in pea plants studied by Mendel.

Which of the given traits is correctly placed? (a) (i), (ii) and (iii) only (b) (ii), (iii) and (iv) only (c) (ii) and (iii) only (d) (i), (ii), (iii) and (iv) (iv) Some of the dominant traits studied by Mendel were (a) round seed shape, green seed colour and axial flower position (b) terminal flower position, green pod colour and inflated pod shape (c) violet flower colour, green pod colour and round seed shape (d) wrinkled seed shape, yellow pod colour and axial flower position. (v) Which of the following characters was not chosen by Mendel?

(ii) The angle between the incident ray and the emergent ray is called

(iii) When a ray is refracted through a prism, then

(iv) The angle of deviation depends on

(v) The rectangular surfaces of a prism are known as

Some harmful non-biodegradable chemicals, i.e., pesticides (e.g., DDT) and heavy metals (e.g., mercury, arsenic cadmium, etc.) enter the bodies of organism through the food chain and go on concentrating at each trophic level. This phenomenon is called bio-magnification or biological magnification. (i) Refer to the given food chain Phytoplankton $\longrightarrow$ Zooplankton $\longrightarrow$ Small fish $\longrightarrow$ Large fish $\longrightarrow$ Fish eating birds If concentration of DDT in small fish is estimated to be 0.5 ppm, then amount of DDT in zooplankton and large fish would respectively be

(ii) Refer to the given table.

According to the given data. The correct order in a food chain will be

(iv) Higher amount of DDT disturb calcium metabolism of birds. This results in

(v) When animals are sprayed with poisons, they may die immediately, but their bodies still contain the poison. The poison in their bodies will then be passed on to the animals which eat them. What would be the consequence of a mass poisoning of the rabbit population in a grazing food chain and why? (a) Plants would die quickly as they are eaten by rabbits (b) Grasshopper would die quickly as all the animals in the food web would be affected (c) Western rattlesnakes would quickly become poisoned as they eat rabbits (d) Hawk would become poisoned as they feed on rabbits

(v) Greenhouse effect is due to

Energy flow is the key function of an ecosystem. It is determined by the two basic laws of thermodynamics. Flow of energy in our ecosystem is unidirectional. Green plants capture approximately about 1% of the solar energy incident on the earth to carry out the process of photosynthesis. In an ecosystem, transfer of energy follows 10 percent law, i.e., only 10% energy is transferred from one trophic level to another and remaining 90% of energy is lost in respiration. (i) Read the given statements and select the incorrect one(s). I. At each trophic level organisms utilise energy in respiration. II. Only 10 percent of the solar radiations that fall on earth is used by green plants. III. Green plants are the ultimate source of entire energy as most of the food chain begin with them. IV. A food chain usually consist of 3-4 trophic levels.

(ii) Refer to the given flow chart. Plants $\rightarrow$ Rat $\rightarrow$ Snake 20 units 2 units 0.2 unit The given flow chart states that (a) flow of energy in an ecosystem is unidirectional (b) as we move along in a food chain the number of individuals at each trophic level decreases (c) only 10% of the total energy becomes available to next trophic level (d) both (a) and (c). (iii) Nearly 90% of the energy is wasted while moving from one trophic level to other. This energy is used in

(v) Which of the following correctly states the processes involved in energy transfer between the trophic levels?

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Cbse 10th standard science subject case study questions answer keys.

(I) (b) : H 2 is oxidised to HCI while Cl 2 is reduced to HCl. (ii) (c) $(iii) (c): 2 \mathrm{Fe} \mathrm{Cl}_{3}+\mathrm{H}_{2} \mathrm{~S} \longrightarrow 2 \mathrm{FeCl}_{2}+2 \mathrm{HCl}+\mathrm{s}$ H 2 Sitself gets oxidised to Sand reduces FeCl 3 to FeCI 2 (iv) (a ): ZnO is reduced to Zn and CO is oxidised to CO 2 (v) (b) : H 2 O 2 is reduced to water by removal of oxygen.

(i) (c): As the pH value increases from 7 to 14, it represents decrease in H+ ion concentration in the solution. (ii) (c) : pH = -log l0 [H + ] = 8 log l0 [H + ] =-8 [H + ] = 10 - 8 mol/L (iii) (a) (iv) (b): C 2 H 5 OH is not an ionic compound, it is a covalent compound and hence does not give H + ions in aqueous solution. (v) (c) : (a) Lower the pH of the solution, more acidic is the solution and higher is the [H + ] ions Thus, solution P (pH = 1) has higher [H + ] ions than solution R (pH = 3). (b) Higher the pH of the solution, more basic is the solution and higher is the [OH - ] ions Thus, solution Q (pH = 9) has lower [OH - ] ions than solution S (pH = l3). (c) Solution P (pH = 1) is acidic which turns blue litmus solution red whereas solution Q (pH = 9) is basic which turns red litmus solution blue. (d) Solution P (pH = 1) is highly acidic while solution S (pH = l3) is highly basic and solution Q (pH = 9) is weakly basic.

${ (i) }(\mathrm{b}): \mathrm{Na}_{2} \mathrm{CO}_{3}+\mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2} \longrightarrow 2 \mathrm{NaHCO}_{3}$ (ii) (b) : $\mathrm{NaHCO}_{3}+\mathrm{CH}_{3} \mathrm{COOH} \longrightarrow \mathrm{CH}_{3} \mathrm{COONa}$ $+\mathrm{CO}_{2} \uparrow+\mathrm{H}_{2} \mathrm{O}$ Carbon dioxide gas is evolved which turns limewater milky. It extinguishes a burning splinter since it is not a supporter of combustion. It dissolves in sodium hydroxide solution and it is an odourless gas. ${ (iii) }(\mathrm{c}): 2 \mathrm{NaHCO}_{3} \stackrel{\text { Heat }}{\longrightarrow} \mathrm{Na}_{2} \mathrm{CO}_{3}+\mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2}$ NaHCO 3 is soluble in water. ${ (iv) }(\mathbf{b}): \mathrm{NaHCO}_{3}+\mathrm{CH}_{3} \mathrm{COOH} \longrightarrow$ $\mathrm{CH}_{3} \mathrm{COONa}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}$ (v) (c): It is not used in manufacture of soap .

(i) (d) (Ii) (b): '2' is an ionic compound ${ (iii) }(\mathrm{a}): \mathrm{Mg} \longrightarrow \mathrm{Mg}^{2+}+2 e^{-}$ $\mathrm{Cl}+e^{-} \longrightarrow \mathrm{Cl}^{-}$ $\mathrm{Mg}^{2+}+2 \mathrm{Cl}^{-} \longrightarrow \mathrm{MgCl}_{2}$ 2,8,2 2,8 2,8,7 2,8,8 $(\text { iv })(\mathrm{d}): \mathrm{Na} \longrightarrow \mathrm{Na}^{+}+e^{-}$ 2,8,1 2,8 (v) (c): (a) and (d) represent electronegative elements and (b) represents a noble gas.

(i) (c) : Molecular formula of (Q) is CSH1Sas it has two carbon atoms less than (P). (ii) (c): Compounds (P), (Q) and (R) are alkanes having general formula C n H 2n+2 . (iii) (a): Molecular formula of (R) is C 12 H 26 as it has two carbon atoms more than (P) (iv) (b): Compound (P), (Q) and (R) belong to same homologous series so they have different physical properties but similar chemical properties. They have same general formula C n H 2n+2 .They . differ by 2 carbon atoms and 4 hydrogen atoms. (v) (a)

(i) (a): As the size of the atom increases down the group, electropositive character increases. (ii) (c): Li is the first element of the second period. As the size decreases in the period from left to right, therefore, Li is the largest atom in the period. (iii) (c): Al (Z = 13) : 2, 8, 3 (iv) (b): Metallic character of elements decreases from left to right and increases down the group. (v) (a): As we move from left to right along a period, the number of valence electrons increases from 1 to 8.

(i) (a): In human, cellulose is indigestible as it cannot be broken into smaller molecules due to absence of cellulase enzyme. (ii) (b): Finger-like projections that come out from mucosa of intestine form villi. Cells lining the villi produce numerous microscopic projections called microvilli giving a brush border appearance which increase the surface area for absorption enormously. Villi has a good supply of capillaries and a large lymph vessel for absorption of nutrients. If the inner lining of the small intestine will be smooth, the surface for absorption will be reduced. (iii) (a) (iv) (c) (v) (b)

(i) (c): A- Artery: Carries blood from heart to different body parts. It is thick-walled and elastic. It acts as a "pressure reservoir" for maintaining the blood flow. B - Capillary : Nutrients, hormones, gases, etc. can diffuse into tissue cells through capillaries and vice versa. It is thin-walled, and only one cell layer thick resting on basement membrane. C - Vein: Brings blood from different body parts to the heart. It is thin-walled and act as low-resistance conduct for blood flow. D - Pulmonary vein: Two pulmonary veins from each lung transport the oxygenated blood to the left atrium. (ii) (d): In amphibians, the left atrium receives oxygenated blood from the gills/lungs/skin and the right atrium gets the deoxygenated blood from other body parts. However, they get mixed up in the single ventricle which pumps out mixed blood i.e., incomplete double circulation (iii) (d): Whale is a mammal and in mammals, two separate circulatory pathways are found - systemic circulation and pulmonary circulation. Oxygenated and deoxygenated bloods received by the left and right atria respectively pass on to the left and right ventricles. Thus, oxygenated and deoxygenated bloods are not mixed. This is referred to as double circulation. (iv) (a) (v) (c): Pulmonary circulation is the movement of blood between heart and lungs. During this pathway deoxygenated blood entering the right atrium, moves into the right ventricle. From here it moves through the pulmonary arch into the lungs for oxygenation. Then from lungs the oxygenated blood moves into the left atrium through pulmonary veins.

(i) (b): The tiny spores of bread mould (Rhizopus) are always present in air. On coming in contact with moist surface of bread slice they settle on it and germinate to form new fungal hyphae which first look like white cottony mass and later turns black. (ii) (a): Mucor (fungus) reproduces asexually through spore formation. (iii) (d) (iv) (c) : Bacteria produce endospore which is a dormant and tough structure that enables bacteria to remain dormant for extended periods under unfavorable conditions. (v) (d)

(i) (a) : Characters studied by Mendel are as follows:

(i) (a): The angle between the two refracting surfaces of a prism is called angle of prism. (ii) (b): The angle between the incident ray and the emergent ray is called angle of deviation. (iii) (d): As the ray of light enters from rarer medium (air) to denser medium (glass), the angle of incidence is more than angle of refraction. (iv) (c): More be the refractive index, more be the angle of deviation and it also depends on the refractive index of prism. (v) (c): The refraction of light takes place through rectangular surfaces.

(i) (c): No two magnetic field lines are found to cross each other. If two field lines crossed each other, it would mean that at the point of intersection, the compass needle would point in two directions at the same time, which is not possible. (ii) (d): The magnetic field and hence the magnetic line of force exist in all the planes all around the magnet. (iii) (d): The relative strength of the magnetic field is shown by the degree of closeness of the field lines and the direction of the magnetic field is obtained by tangent to the field lines at the point of intersect. (iv) (d): The magnetic field lines due to a bar magnet are closed continuous curves directed from N to S outside the magnet and directed from S to N inside the magnet. Hence option (d) is correct. v) (d): Inside a bar magnet, the direction of field lines is from south pole to north pole

(i) (a): Due to bio-rnagnification, the concentration of DDT will always be less in zooplanktons than large fish (ii) (c) (iii) (b) : Due to bio-rnagnification the nonbio-degradable chemicals such as DDT accumulate and go on concentrating at each trophic level. (iv) (d) : Higher amounts of DDT disturb calcium metabolism of birds resulting in thinning of egg shells and their prematllre breaking that kills the embryos. (v) (d)

( i) (b) : In the given pie chart, gases P, Q, Rand S respectively are CO 2 , CH 4 , CFCs and N 2 O. Methane is produced by incomplete combustion of biomass. (ii) (c): Methane (gas Q) is produced by incomplete biomass combustion and incomplete decomposition mostly by anaerobic methanogens. Flooded paddy fields, marshes and cattles are the major source of this gas. (iii) (c) : CO 2 is the principal greenhouse gas that helps to keep the earth warm. (iv) (d) (v) (c)

(i) (b): 1% of solar radiation is captured by plants. Sun is the ultimate source of all energy. (ii) (d) (iii) (d) (iv) (d): The given pyramid is pyramid of energy that shows the two basic laws of thermodynamics. (v) (c): Light energy from the sun is converted to chemical energy in producers via photosynthesis. This chemical energy is then transferred to primary consumer, then subsequently to secondary consumer via feeding.

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NCERT Solutions for Class 10
NCERT Class 10 Science
Chapter 1 Chemical Reactions And Equation

NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations

Ncert solutions for class 10 science chapter 1 – cbse download free pdf.

Download Exclusively Curated Chapter Notes for Class 10 Science Chapter – 1 Chemical Reactions and Equations

Download most important questions for class 10 science chapter – 1 chemical reactions and equations.

Chapter 1 of NCERT Solutions for Class 10 Science mainly deals with writing chemical equations and writing and balancing chemical equations. Also, in this chapter, students learn the basics of chemical reactions, their types and the effects of a chemical oxidation reaction in our daily lives. The NCERT Solutions Class 10 Science Chapter 1 provides an overview of the main concepts in the chapter and help them to get well-versed in important topics such as writing chemical equations and balancing them.

The NCERT Solutions for Class 10 Science Chapter 1 have good weightage, and there will be around 4 questions asked from this chapter every year. The types of questions that appear in this chapter are mostly practice-based questions. Thorough knowledge and good practice will help learners score full marks on the questions asked in this chapter.

Chapter 2 Acids, Bases and Salts
Chapter 3 Metals and Non-metals
Chapter 4 Carbon and Its Compounds
Chapter 5 Periodic Classification of Elements
Chapter 6 Life Processes
Chapter 7 Control and Coordination
Chapter 8 How Do Organisms Reproduce?
Chapter 9 Heredity and Evolution
Chapter 10 Light Reflection and Refraction
Chapter 11 The Human Eye and Colourful World
Chapter 12 Electricity
Chapter 13 Magnetic Effects of Electric Current
Chapter 14 Sources of Energy
Chapter 15 Our Environment
Chapter 16 Management of Natural Resources

NCERT Solutions for Class 10 Science Chapter

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Access answers to NCERT Class 10 Science Chapter 1 – Chemical Reactions and Equations

In-text questions set 1 Page number – 6

1. Why should a magnesium ribbon be cleaned before burning in the air?

Magnesium ribbon should be cleaned before burning in air because Magnesium metal reacts with the atmospheric oxygen and forms Magnesium Oxide (MgO) layer which is a very stable compound. In order to prevent further reactions with Oxygen, it is therefore necessary to clean the ribbon by to remove the layer of MgO.

2. Write a balanced equation for the following chemical reactions.

i) Hydrogen + Chloride —-> Hydrogen chloride

ii) Barium chloride + Aluminium sulphate —-> Barium sulphate + Aluminium chloride

iii) Sodium + Water —-> Sodium hydroxide + Hydrogen

i) H 2 + Cl 2 → 2HCl

ii) 3BaCl 2 + Al 2 (SO 4 ) 3 →3BaSO 4 + 2AlCl 3

iii) 2Na + 2H 2 O → 2NaOH + H 2

3. Write a balanced chemical equation with state symbols for the following reactions

i) Solutions of Barium chloride and Sodium sulphate in water react to give insoluble Barium sulphate and solution of Sodium chloride.

ii) Sodium hydroxide solution in water reacts with the hydrochloric acid solution to produce Sodium chloride solution and water.

i) BaCl 2 + Na 2 SO 4 → BaSO 4 + 2NaCl

ii) NaOH + HCl → NaCl + H 2 O

In-text questions set 2 Page number – 10

1. A solution of a substance, ‘X,’ is used for whitewashing.

(i) Name the substance ‘X’ and write its formula.

(ii) Write the reaction of the substance ‘X’ named in (i) above with water.

i) The substance ‘X’ which is used in whitewashing is quick lime or Calcium Oxide and its formula is CaO .

ii) CaO + H 2 O → Ca(OH) 2

2. Why is the amount of gas collected in one of the test tubes in Activity 1.7 double the amount collected in the other? Name this gas.

In activity 1.7, gas collected in one of the test tubes is double of the amount collected in the other because water gets hydrolysed to release H 2 and O 2 gas. Here, after electrolysis two molecules of Hydrogen and one molecule of oxygen gas are released; hence, the amount of Hydrogen collected would be double than that of oxygen.

In-text questions set 3 Page number – 13

1. Why does the colour of copper sulphate solution change when an iron nail is dipped in it?

When an iron nail is dipped in the copper sulphate solution, iron displaces copper from the copper sulphate because iron is more reactive than copper. Therefore, the colour of the copper sulphate solution changes. The reaction is

Fe + CuSO 4 → FeSO 4 + Cu

2. Give an example of a double displacement reaction other than the one given in Activity 1.10.

Solution:

Reaction Between silver nitrate (AgNO 3 ) and Sodium chloride (NaCl) is an example of a double displacement reaction. During the reaction, negative and positive ions trade positions as a result of the formation of white silver chloride precipitate. The chemical reaction is given below.

Ag + + NO 3 – + Na + + Cl – → AgCl + Na + + NO 3 –

3. Identify the substances that are oxidised and that are reduced in the following equation.

i) 4Na(s) + O 2 (g) → 2Na 2 O(s)

ii) CuO(s) + H 2 (g) → Cu(s) + H 2 O(l)

The Sodium (Na) in the first equation is getting oxidized with the addition of Oxygen (O 2 ), and the Copper (Cu) in the second equation is reduced due to the addition of Hydrogen (H 2 ).

Exercise Questions Page number – 14-16

1. Which of the statements about the reaction below are incorrect?

2PbO(s) + C(s) → 2Pb(s) + CO 2 (g)

(a) Lead is getting reduced

(b) Carbon Dioxide is getting oxidised

(d) Lead oxide is getting reduced

(i) (a) and (b)

(ii) (a) and (c)

(iii) (a), (b) and (c)

(iv) all the above

(i) (a) and (b)

Explanation: (a) Because Oxygen is being removed and (b) Because the removed oxygen from Lead is added to the elemental Carbon.

2. Fe 2 O 3 + 2Al → Al 2 O 3 + 2Fe

The above reaction is an example of a

Combination reaction

Double displacement reaction

Decomposition reaction

Displacement reaction

The answer is 4. Displacement reaction.

Explanation: The Oxygen from the Ferrous oxide is getting displaced to the Aluminium metal to form Aluminium Oxide. In this reaction, Aluminum is a more reactive metal than Fe. Therefore, Al will displace Fe from its oxide. This type of chemical reaction, called displacement reaction, is in which one of the elements displaces another. Here, less reactive metal is displaced by more reactive metal. Since one-time displacement is occurring, it is called a single displacement reaction.

3. What happens when dilute hydrochloric acid is added to iron fillings? Tick the correct answer.

Hydrogen gas and Iron chloride are produced.
Chlorine gas and Iron hydroxide are produced.
No reaction takes place.
Iron salt and water are produced.

Explanation: The Chlorine from Hydrogen chloride is displaced by the Iron fillings to undergo the following reaction.

2HCl + Fe → FeCl 2 + H 2

4. What is a balanced chemical equation? Why should a chemical equation be balanced?

A balanced equation is the one in which number of different atoms on both the reactant and product sides are equal. Balancing chemical equations is necessary for the reaction should obey The Law of Conservation of mass. Balancing the chemical equation has no defined method and is purely a trial-and-error attempt.

5. Translate the following statements into chemical equations and balance them.

(a) Hydrogen gas combines with nitrogen to form ammonia.

(b) Hydrogen sulphide gas burns in the air to give water and sulphur dioxide.

(d) Potassium metal reacts with water to give potassium hydroxide and Hydrogen gas.

(a) Unbalanced: H 2 + N 2 → NH 3

Balanced: 3H 2 + N 2 → 2NH 3

(b) Unbalanced: H 2 S + O 2 → H 2 O + SO 2

Balanced: 2H 2 S + 3O 2 → 2H 2 O + 2SO 2

BaCl 2 + Al 2 (SO 4 ) 3 → AlCl 3 + BaSO 4

Balanced: 3BaCl 2 + Al 2 (SO 4 ) 3 → 2AlCl 3 + 3BaSO 4

(d) Unbalanced: K + H 2 O → KOH + H 2

Balanced: 2K + 2H 2 O → 2KOH + H 2

6. Balance the following chemical equations.

(a) HNO 3 + Ca(OH) 2 → Ca(NO 3 ) 2 + H 2 O

(b) NaOH + H 2 SO 4 → Na 2 SO 4 + H 2 O

(d) BaCl 2 + H 2 SO 4 → BaSO 4 + HCl

(a) 2HNO 3 + Ca(OH) 2 → Ca(NO 3 ) 2 + 2H 2 O

(b) 2NaOH + H 2 SO 4 → Na 2 SO 4 + 2H 2 O

(d) BaCl 2 + H 2 SO 4 → BaSO 4 + 2HCl

7. Write the balanced chemical equation for the following reactions.

Calcium hydroxide + Carbon dioxide —-> Calcium carbonate + Water

Zinc + Silver nitrate —-> Zinc nitrate + Silver

Aluminium + Copper chloride —-> Aluminium chloride + Copper

Barium chloride + Potassium sulphate —-> Barium sulphate + Potassium chloride

2Ca(OH) 2 + 2CO 2 → 2CaCO 3 + 2H 2 O

Zn + 2AgNO 3 → Zn(NO 3 ) 2 + 2Ag

2Al + 3CuCl 2 → 2AlCl 3 + 3Cu

BaCl 2 + K 2 SO 4 → BaSO 4 + 2KCl

8. Write a balanced chemical equation for the following and identify the type of reaction of each case.

KBr + BaI 2 → KI + BaBr 2

ZnCO 3 → ZnO + CO 2

H 2 + Cl → HCl

Mg + HCl → MgCl 2 + H 2

2KBr + BaI 2 → 2KI + BaBr 2 (Double Displacement Reaction)

ZnCO 3 → ZnO + CO 2 (Decomposition Reaction)

H 2 + Cl → 2HCl (Combination Reaction)

Mg + 2HCl → MgCl 2 + H 2 (Displacement Reaction)

9. What is meant by exothermic and endothermic reactions? Give examples.

An endothermic reaction occurs when energy is absorbed from the surroundings in the form of heat (For example, Photosynthesis, melting of ice, evaporation). Conversely, an exothermic reaction is one in which energy is released from the system into the surroundings (Examples: Explosions, concrete setting, nuclear fission and fusion).

10. Why is respiration considered to be an exothermic reaction?

For the survival of life, we require energy. We obtain this energy from the food we eat. The food molecules, through the process of digestion, is broken down into simpler molecule like glucose. These substances come in contact with the Oxygen present in our body cells to form Carbon dioxide and water along with a certain amount of energy (Respiration process). Since the energy is in the form of heat (that maintains our body temperature), respiration is considered to be an exothermic reaction. The reaction taking place is:

C 6 H 12 O 6 + 6O 2 → 6CO 2 + 6H 2 O + Energy

11. Why are decomposition reactions called the opposite of Combination reactions? Write equations for decomposition reactions.

Combination reaction is said to be the reaction between two or more molecules to form a larger molecule; whereas the decomposition reaction is defined as the splitting of larger molecules into two or more smaller molecules. This essentially explains that the decomposition reaction is the opposite of the combination reaction.

In most cases, the decomposition reaction is endothermic since the heat from the surrounding or induced heat is used to break the bonds of the larger molecule. A few examples of decomposition reactions are

CaCO 3 + Energy → CaO + CO 2

2HgO → 2Hg + O 2

12. Write one equation each for decomposition reactions in which energy is supplied in the form of heat, light or electricity.

(a) Thermal decomposition reaction (Thermolysis)

Decomposition of potassium chlorate: When heated strongly, potassium chlorate decomposes into potassium chloride and oxygen. This reaction is used for the preparation of oxygen.

2KClO 3 + Heat → 2KCl + 3O 2

(b) Electrolytic decomposition reaction (Electrolysis)

Decomposition of sodium chloride: On passing electricity through molten sodium chloride, it decomposes into sodium and chlorine.

NCERT Solution Class 10 Science Chapter 1-1

Decomposition of hydrogen peroxide: In the presence of light, hydrogen peroxide decomposes into water and oxygen.

NCERT Solution Class 10 Science Chapter 1-2

13. What is the difference between displacement and double displacement reactions? Write relevant equations for the above.

A displacement reaction is one when a more reactive substance displaces a less reactive one from its salt solution, whereas a double displacement reaction is one where a mutual exchange of ions happens between two compounds.

In a displacement reaction, only a single displacement takes place, whereas in the double displacement reaction, as the name suggests, two displacement takes place between the molecules.

Mg + 2HCl → MgCl 2 + H 2

2KBr + BaI 2 → 2KI + BaBr 2

14. In the refining of Silver, the recovery of silver from Silver nitrate solution involves displacement reaction by Copper metal. Write down the reaction involved.

Cu(s) + 2AgNO 3 (aq) → Cu(NO 3 ) 2 (aq) + 2Ag(s)

15. What do you mean by a precipitation reaction? Explain by giving examples.

When two solutions containing soluble salts are combined, a double displacement reaction takes place in which the ions are exchanged between the compounds. When one of such compounds formed is in solid form (that is insoluble in aqua), then it settles down at the bottom of the container. This solid is known as the precipitate and the respective reaction is termed as the precipitation reaction. A few examples of precipitation reactions are

CdSO 4 (aq) + K 2 S(aq) → CdS(s) + K 2 SO 4 (aq)

2NaOH(aq) + MgCl 2 (aq) → 2NaCl(aq) + Mg(OH) 2 (s)

16. Explain the following in terms of the gain of oxygen with two examples each.

(a) Oxidation

(b) Reduction

(a) In a chemical reaction, when the oxygen is added to the element to form its respective oxide it is the element being oxidised. Example:

4Na(s) + O 2 (g) → 2Na 2 O(s)

H 2 S + O 2 → H 2 O + SO 2

(b) In a chemical reaction, when the oxygen is removed from the compound, then it is said to be reduced. Example:

CuO(s) + H 2 (g) → Cu(s) + H 2 O(l)

17. A shiny brown coloured element ‘X’ on heating in the air becomes black in colour. Name the element ‘X’ and the black-coloured compound formed.

The shiny brown-coloured element is Copper metal (Cu). When the metal is heated in air, it reacts with atmospheric oxygen to form copper oxide. Hence, the black-coloured compound is copper oxide.

2Cu(s) + O 2 (g) → 2CuO(s)

18) Why do we apply paint on iron articles?

Iron articles are painted to prevent them from rusting. When left unpainted, the metal surface comes in contact with the atmospheric oxygen and in the presence of moisture it from Iron(III) oxide. But if painted, the surface does not come in contact with moisture and air, thus prevents Rusting.

19) Oil and Fat containing food items are flushed with Nitrogen. Why?

The main purpose of flushing Nitrogen into food packets that contain oil and fat items is to prevent Rancidity which occurs when the oil or fat reacts with the oxygen letting out an unpleasant smell and taste. Therefore, by flushing Nitrogen, an unreactive surrounding is created, thus preventing rancidity.

20) Explain the following terms with one example each.

(a) Corrosion

(b) Rancidity

(a) Corrosion is a process where a refined metal is oxidised by atmospheric oxygen to form a more stable compound, such as oxides. The metal gradually degrades during the corrosion process. Rusting of iron is a good example of corrosion where the iron is converted to Iron oxide. Millions of dollars are spent annually in preventing rusting from bridges and other monuments.

(b) The condition produced by the aerial oxidation of the oil and fat present in the food material that produces an unpleasant taste and smell. The rancidity is retarded when the food is kept inside the refrigerator since the low temperature does not promote the oxidation reaction.

Topics Covered under Class 10 Chapter 1 Science Chemical Reactions and Equations

Chemical Reactions and equations is a very fundamental chapter that deals with basic knowledge of chemical reactions and equations. Students are advised to get tuned in with this chapter to avoid any sort of difficulty in understanding advanced topics of chemistry. If you are planning to take science in your higher secondary school, this is one of the important chapters you have to memorise for a very long period of time.

Features of NCERT Solutions for Class 10 Chapter 1 Science Chemical Reactions and Equations

Students can get comprehensive practice in balancing different kinds of equations.
NCERT Solutions will help students write different chemical equations appropriately
Help them get a thorough practice of solving questions of varied difficulty before facing the CBSE examination.

A chemical reaction is an important phenomenon in our lives. We come across various chemical reactions like rusting of iron, curdling of milk, respiration, digestion and growth. In order to score good marks in the CBSE Class 10 examination, students must practise the NCERT Solution for Class 10 Science Chapter 1 provided here.

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Case Study Questions Class 10 Science Life Processes

Case study questions class 10 science chapter 6 life processes.

At Case Study Questions there will given a Paragraph. In where some Important Questions will made on that respective Case Based Study. There will various types of marks will given 1 marks, 2 marks, 3 marks, 4 marks.

CBSE Case Based Questions Class 10 Science Chemistry Chapter 6

CASE STUDY : 1

Carbon and energy requirements of the autotrophic organism are fulfilled by photosynthesis. It is the process by which autotrophs take in substances from the outside and convert them into stored forms of energy. This material is taken in the form of carbon dioxide and water which is converted into carbohydrates in the presence of sunlight and chlorophyll. Carbohydrates are utilised for providing energy to the plant.

i) Write a chemical reaction which occur during photosynthesis?

Ans: 6CO2 +12H2O + Chlorophyll & sunlight👉 C6H12O6 + 6O2 + 6H2O

ii) In which form of carbohydrates does the plant stored in them?

Ans: The carbohydrates are stored in the form of starch as the internal energy.

iii) What is stomata?

Ans: The process present in the surface of a leaf or the stem of a plant to allow the exchange of gases.

iv) What are the functions of stomata?

Ans: i) Exchange of gases i.e oxygen and CO2

ii) Transpiration

v) What is Chloroplast?

Ans: Chloroplast is a cell organelles which contains photosynthetic pigment called as chlorophyll which help in the absorption of sunlight.

CASE STUDY : 2

The alimentary canal is basically a long tube extending from the mouth to the anus. In Fig. 6.6, we can see that the tube has different parts. Various regions are specialised to perform different functions.

We eat various types of food which has to pass through the same digestive tract. Naturally the food has to be processed to generate particles which are small and of the same texture. This is achieved by crushing the food with our teeth

i) Which enzyme is present in our mouth to digest starch?

Ans: Salivary amylase from salivary glands.

ii) What are the types of enzymes released by our stomach?

Ans: Hydrochloric acid, pepsin and a mucus.

iii) Which is the longest part of our alimentary canal in our body?

Ans: Small intestine

iv) What are villi?

Ans: Villi are finger like projection present inside the inner lining of the small intestine which increases the surface area for absorption.

v) What are the enzymes that are released by pancreas?

Ans: Enzyme released by pancreas – • trypsin- Digestion of protein

lipase – breakdown of emulsified fats

CASE STUDY : 3

The food material taken in during the process of nutrition is used in cells to provide energy for various life processes. Diverse organisms do this in different ways – some use oxygen to break-down glucose completely into carbon dioxide and water, some use other pathways that do not involve oxygen (Fig. 6.8). In all cases, the first step is the break-down of glucose, a six-carbon molecule, into a three-carbon molecule called pyruvate. This process takes place in the cytoplasm.

i) What is anaerobic respiration?

Ans: The conversion of pyruvate into ethanol, CO2 & energy take place in the absence of air(oxygen), it is called anaerobic respiration.

ii) Explain the process which happen in our muscle cells?

Ans- The conversion of pyruvate to lactic acid( 3 carbon molecule) and energy due to the lack of oxygen.

iii) In which form our body used the energy?

Ans: It is in the form of ATP molecule i.e Adenosine Triphosphate.

iv) Why there is a faster breathing rate of aquatic animals then the terrestrial animals?

Ans- The amount of O2 dissolved in water is low as compared to amount of O2 present in air. Therefore, aquatic animals have faster breathing rate.

v) Write the name of organ used for respiration by different organism- fish, frog?

Ans- i) fish- gills

ii) frog- skin, lungs

CASE STUDY : 4

The excretory system of human beings includes a pair of kidneys, a pair of ureters, a urinary bladder and a urethra. Kidneys are located in the abdomen, one on either side of the backbone. Urine produced in the kidneys passes through the ureters into the urinary bladder where it is stored until it is released through the urethra.

i) What is the purpose of making urine?

Ans: Urine is to filter out the blood i e to remove waste product from the blood such as urea.

ii) What is Bowman’s capsule?

Ans: A cup shaped end of a coiled tube which is associated with capillaries to collect filterate.

iii) What is dialysis?

Ans: To remove nitrogenous waste from your blood by using machine when kidney does not its function i.e in case of kidney failure.

iv) What is the function of urinary bladder?

Ans: It is used to stored urine until the pressure comes from the brain to pass it out.

v) What are the different parts of nephrons?

Ans: Renal artery, Bowman’s capsule, glomerulus, tubular part of nephron and a collecting duct.

CASE STUDY : 5

The heart is a muscular organ which is as big as our fist. Because both oxygen and carbon dioxide have to be transported by the blood, the heart has different chambers to prevent the oxygen-rich blood from mixing with the blood containing carbon dioxide. The carbon dioxide-rich blood has to reach the lungs for the carbon dioxide to be removed, and the oxygenated blood from the lungs has to be brought back to the heart. This oxygen-rich blood is then pumped to the rest of the body.

i) How many chambers are present in the heart of mammals and reptiles?

Ans: Mammals- 4 chamber heart and reptiles- 3 chambered heart

ii) Who carry deoxygenated blood from body to heart?

Ans: Vena cava carries deoxygenated blood from body to heart.

iii) What do you meant by the term double circulation?

Ans: The blood goes through the heart twice during each cycle known as double circulation.

iv) What is hypertension?

Ans: The force that blood experts against the wall of a vessels is called hypertension or high blood pressure.

V) Which device measured blood pressure?

Ans: Sphygmomanometer

CASE STUDY : 6

Plant transport systems will move energy stores from leaves and raw materials from roots. These two pathways are constructed as independently organised conducting tubes. One, the xylem moves water and minerals obtained from the soil. The other, phloem transports products of photosynthesis from the leaves where they are synthesised to other parts of the plant

i) What are the different parts of xylem?

Ans: vessels, tracheids, xylem parenchyma and fibres.

ii) What do you meant by the term transpiration?

Ans: The loss of water in the form of vapour from the aerial parts of the plant.

iii) What are the advantages of transpiration?

Ans: i) help in the absorption and the upward movement of water

ii) temperature regulation

iv) What is translocation?

Ans: The transport of soluble products of photosynthesis is called translocation.

v) How does plant remove their waste product?

Ans: They remove their waste product in the form of fallen leaves, resins and gums.

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Case Study Questions for Class 10 Science Chapter 1

Case Study Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations provided below is very helpful to understand the new format of Board Exams. Case Study Questions for class 10 Chemistry is a very trustable source for practice. Class 10 Science Chapter 1 Case Study Questions is provided to you by NCERT HUB.

Solve the given Case Study Questions for Class 10 Science Chapter 1 to enhance your performance in the upcoming Board Exam. Case Study Questions for Class 10 Chemical Reactions and Equations is very important as these types of questions will be asked in the Board Exam.

Case Study Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations

1. Read the following and answer the questions from 1.1 to 1.5 :

Amit took a lime solution and passed a gas ‘X’ through it. The solution becomes turgid. This solution was then divided into two parts. In the first part, more of gas ‘X’ was passed. While in the second part concentrated sulphuric acid was added. A white precipitate was formed in second part.

Case Study Questions for Class 10 Science Chapter 1

1.1) The gas mentioned in above passage is : (a) O₂ (b) H₃S (c) CO₂ (d) H₂ Answer

1.2) Lime water and chlorine reacts to form : (a) CaCl₂ (b) CaOCl₂ (c) CaO (d) CaCO Answer

1.3) A solution of a substance X is used for white washing. Identify X : (a) CaO (b) Ca(OH)₂ (c) CaCO₃ (d) CO₂

1.4) Ca(HCO₃) is : (a) insoluble in water (b) soluble in water (c) partially soluble in water (d) partially insoluble in water Answer

1.5) Lime water turns milky in the reaction due to the : (a) oxygen gas is evolved (b) formation of calcium bicarbonate (c) CO₂ gas is evolved (d) formation of calcium carbonate Answer

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2. Read the following and answer the questions from 2.1 to 2.5 :

In decomposition reactions, a single reactant breaks down to form two or more products. Decomposition reaction is opposite to combination reaction. Thermal decomposition reactions use the energy in form of heat for decomposition of reactants. Electrolytic decomposition reactions involve the use of electrical energy for the decomposition of reactant molecules. Photolysis or or photochemical decomposition involves the use of light energy for the purpose of decomposition.

2.1) Which of the following reactions is a decomposition reaction ? (a) NaOH + HCl → NaCl + H₂O (b) NH₄CNO → H₂NCONH₂ (c) 2KClO₃ → 2KCl + 3O₂ (d) H₂ + I₂ → 2HI Answer

2.2) 2Pb(NO3 )2 → 2PbO + nA + O₂. What is nA in the given reaction ? (a) NO₂ (b) 2PbNO₂ (c) 4NO₂ (d) 4NO Answer

2.3) Amino acid is formed by the decomposition of which component of our diet ? (a) Fat (b) Protein (c) Starch (d) Carbohydrate Answer

2.4) Silver chloride on exposure to sunlight for a long duration turns grey due to (i) the formation of silver by decomposition of silver chloride (ii) Sublimation of silver chloride (iii) decomposition of chlorine gas from silver chloride (iv) Oxidation of silver chloride. The correct statement(s) is / are :

(a) Only (iv) (b) Only (i) and (iii) (c) Only (ii) and (iii) (d) Only (i) and (ii) Answer

2.5) What type of chemical reaction takes place when electricity is passed through water ? (a) Displacement reaction (b) Photochemical decomposition (c) Electrolytic decomposition (d) Thermal decomposition Answer

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3. Read the following and answer the questions from 3.1 to 3.5 :

Redox reactions are those reactions in which oxidation and reduction occur simultaneously. A redox reaction is made up of two half reactions. In the first half reaction, Oxidation takes place and in second half reaction, reduction occurs. Oxidation is a process in which a substance loses electrons and in reduction, a substance hydrogen to a substance and removal of oxygen from a substance.

The substance which gives oxygen to another substance or removes hydrogen from another substance in an oxidation reaction is known as oxidising agent, while the substance which gives hydrogen to another substance or removes oxygen from another substance in a reduction reaction is known as reducing agent.

3.1) Which of the following is a redox reaction? (a) CaCO₃ → CaO + CO₂ (b) CaO + 2HCl → CaCl₂ + H₂O (c) H₂ + Cl₂ → 2HCl (d) NaOH + HCl → NaCl + H₂O Answer

3.2) Identify the reaction in which H₂O₂ is acting as a reducing agent. (a) Cl₂ + H₂O₂ → 2HCl + O₂ (b) 2FeCl₂ + 2HCl + H₂O₂ → 2FeCl₃ + 2H₂O (c) H₂SO₃ + H₂O₂ → H₂SO₄ + H₂O (d) 2HI + H₂O₂ → 2H₂O + I₂ Answer

3.3) For the following reaction, identify the correct statement.

ZnO + CO → Zn + CO₂

(a) CO₂ is being oxidised. (b) ZnO is being reduced. (c) ZnO is being oxidised. (d) CO is being reduced. Answer

3.4) In the following reaction, which substance is reduced ?

PbS + 4H₂O₂ → PbSO₄ + 4H₂O (a) PbSO₄ (b) PbS (c) H₂O (d) H₂O₂ Answer

3.5) For the following reactions, identify the one in which H₂S acts as a reducing agent . (a) CuSO₄ + H₂S → CuS + H₂SO₄ (b) Cd(NO₃)₂ + H₂S → CdS + 2HNO₃ (c) 2FeCl₃ + H₂S → 2FeCl₂ + 2HCl + S (d) None of these Answer

Practice Case Study Questions for Class 10 Science Chapter 1 to boost your score in Board Exam.

4. Read the following and answer the questions from 4.1 to 4.5 :

In a chemical reaction, reactants are converted into products. The conversion of reactants into products in a chemical reaction is often accompanied by some features. These features which take place as a result of chemical reaction are known as characteristics of chemical reactions. Some important characteristics of chemical reactions are : evolution of heat, change in colour, change in temperature etc.

4.1) Reaction of magnesium with air is : (a) exothermic reaction (b) substitution reaction (c) endothermic reaction (d) reversible reaction Answer

4.2) Which law is satisfied by a balanced chemical equation ? (a) Law of multiple proportions (b) Law of constant proportions (c) Law of conservation of mass (d) Law of conservation of chemical Answer

4.3) Which one of the following processes involve chemical reactions ? (a) Storing of Oxygen gas under pressure in a gas cylinder (b) Liquefication of air (c) Keeping petrol in china dish in the open (d) Heating copper wire in the presence of air at high temperature Answer

4.4) In which of the following reactions, high amount of heat energy will be evolved ? (a) Electrolysis of water (b) Burning of LPG (c) Decomposition of AgBr in the presence of light (d) Dissolution of NH₄Cl in water Answer

4.5) What type of chemical reaction takes place when electricity is passed through water ? (a) Thermal decomposition (b) Photochemical decomposition (c) Water decomposition (d) Electrolytic decomposition Answer

5. Read the following and answer the questions from 5.1 to 5.5 :

You must have observed that iron articles are shiny when they are new, but get coated with a reddish brown powder when left for sometime. This process is commonly known as rusting of iron. Some other metals also get tarnished in the same manner. When a metal is attacked by substances around it such as moisture, its said to corrode and this process is called corrosion. The black coating on silver and the green coating on copper are some examples of corrosion.

5.1) Chemically rust is : (a) hydrated ferrous oxide (b) hydrated ferric oxide (c) only ferric oxide (d) None of these Answer

5.2) Rusting of iron involves a chemical reaction which is a combination of : (a) Oxidation as well as combination reactions (b) Reduction as well as displacement reactions (c) Oxidation as well as displacement reactions (d) Reduction as well as combination reactions Answer

5.3) Rusting of iron takes place in : (a) ordinary water (b) distilled water (c) Both (a) and (b) (d) None of these Answer

5.4) Silver articles turns black when kept in the open for a few days due to formation of : (a) Ag₂S (b) H₂S (c) AgS (d) AgSO₄ Answer

5.5) Copper objects lose their shine and form green coating of : (a) copper oxide (b) copper carbonate (c) basic copper carbonate (d) copper hydroxide and copper oxide Answer

We hope the given Case Study Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations provided below is very helpful to understand the new format of Board Exams. Case Study Questions for class 10 Chemistry Chapter 1 is a very trustable source for practice. If you have any queries regarding Case Study Questions for Class 10 Science Chapter 1, contact us and we will get back to you soon.

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