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Use chemistry problems as a tool for mastering chemistry concepts. Some of these examples show using formulas while others include lists of examples.
Acids, Bases, and pH Chemistry Problems
Learn about acids and bases. See how to calculate pH, pOH, K a , K b , pK a , and pK b .
- Practice calculating pH.
- Get example pH, pK a , pK b , K a , and K b calculations.
- Get examples of amphoterism.
Atomic Structure Problems
Learn about atomic mass, the Bohr model, and the part of the atom.
- Practice identifying atomic number, mass number, and atomic mass.
- Get examples showing ways to find atomic mass.
- Use Avogadro’s number and find the mass of a single atom .
- Review the Bohr model of the atom.
- Find the number of valence electrons of an element’s atom.
Chemical Bonds
Learn how to use electronegativity to determine whether atoms form ionic or covalent bonds. See chemistry problems drawing Lewis structures.
- Identify ionic and covalent bonds.
- Learn about ionic compounds and get examples.
- Practice identifying ionic compounds.
- Get examples of binary compounds.
- Learn about covalent compounds and their properties.
- See how to assign oxidation numbers.
- Practice drawing Lewis structures.
- Practice calculating bond energy.
Chemical Equations
Practice writing and balancing chemical equations.
- Learn the steps of balancing equations.
- Practice balancing chemical equations (practice quiz).
- Get examples finding theoretical yield.
- Practice calculating percent yield.
- Learn to recognize decomposition reactions.
- Practice recognizing synthesis reactions.
- Practice recognizing single replacement reactions.
- Recognize double replacement reactions.
- Find the mole ratio between chemical species in an equation.
Concentration and Solutions
Learn how to calculate concentration and explore chemistry problems that affect chemical concentration, including freezing point depression, boiling point elevation, and vapor pressure elevation.
- Get example concentration calculations in several units.
- Practice calculating normality (N).
- Practice calculating molality (m).
- Explore example molarity (M) calculations.
- Get examples of colligative properties of solutions.
- See the definition and examples of saturated solutions.
- See the definition and examples of unsaturated solutions.
- Get examples of miscible and immiscible liquids.
Error Calculations
Learn about the types of error and see worked chemistry example problems.
- See how to calculate percent.
- Practice absolute and relative error calculations.
- See how to calculate percent error.
- See how to find standard deviation.
- Calculate mean, median, and mode.
- Review the difference between accuracy and precision.
Equilibrium Chemistry Problems
Learn about Le Chatelier’s principle, reaction rates, and equilibrium.
- Solve activation energy chemistry problems.
- Review factors that affect reaction rate.
- Practice calculating the van’t Hoff factor.
Practice chemistry problems using the gas laws, including Raoult’s law, Graham’s law, Boyle’s law, Charles’ law, and Dalton’s law of partial pressures.
- Calculate vapor pressure.
- Solve Avogadro’s law problems.
- Practice Boyle’s law problems.
- See Charles’ law example problems.
- Solve combined gas law problems.
- Solve Gay-Lussac’s law problems.
Some chemistry problems ask you identify examples of states of matter and types of mixtures. While there are any chemical formulas to know, it’s still nice to have lists of examples.
- Practice density calculations.
- Identify intensive and extensive properties of matter.
- See examples of intrinsic and extrinsic properties of matter.
- Get the definition and examples of solids.
- Get the definition and examples of gases.
- See the definition and examples of liquids.
- Learn what melting point is and get a list of values for different substances.
- Get the azeotrope definition and see examples.
- See how to calculate specific volume of a gas.
- Get examples of physical properties of matter.
- Get examples of chemical properties of matter.
- Review the states of matter.
Molecular Structure Chemistry Problems
See chemistry problems writing chemical formulas. See examples of monatomic and diatomic elements.
- Practice empirical and molecular formula problems.
- Practice simplest formula problems.
- See how to calculate molecular mass.
- Get examples of the monatomic elements.
- See examples of binary compounds.
- Calculate the number of atoms and molecules in a drop of water.
Nomenclature
Practice chemistry problems naming ionic compounds, hydrocarbons, and covalent compounds.
- Practice naming covalent compounds.
- Learn hydrocarbon prefixes in organic chemistry.
Nuclear Chemistry
These chemistry problems involve isotopes, nuclear symbols, half-life, radioactive decay, fission, fusion.
- Review the types of radioactive decay.
Periodic Table
Learn how to use a periodic table and explore periodic table trends.
- Know the trends in the periodic table.
- Review how to use a periodic table.
- Explore the difference between atomic and ionic radius and see their trends on the periodic table.
Physical Chemistry
Explore thermochemistry and physical chemistry, including enthalpy, entropy, heat of fusion, and heat of vaporization.
- Practice heat of vaporization chemistry problems.
- Practice heat of fusion chemistry problems.
- Calculate heat required to turn ice into steam.
- Practice calculating specific heat.
- Get examples of potential energy.
- Get examples of kinetic energy.
- See example activation energy calculations.
Spectroscopy and Quantum Chemistry Problems
See chemistry problems involving the interaction between light and matter.
- Calculate wavelength from frequency or frequency from wavelength.
Stoichiometry Chemistry Problems
Practice chemistry problems balancing formulas for mass and charge. Learn about reactants and products.
- Get example mole ratio problems.
- Calculate percent yield.
- Learn how to assign oxidation numbers.
- Get the definition and examples of reactants in chemistry.
- Get the definition and examples of products in chemical reactions.
Unit Conversions
There are some many examples of unit conversions that they have their own separate page!
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Discover Frequently Asked Chemistry Questions and Their Answers
- Formula for Cd2+ and PO43- ? also whats its name
- What is the Lewis structure for a perchlorate ion?
- Which of these structures has dipole-dipole interactions? Water (H2O), ethyl alcohol (CH3CH2OH), and hexane (C6H14).
- Is a single molecule of oxygen held together by two nonpolar covalent bonds?
- Why do the alkali metals have to be stored under oil?
- How do you know the number of electrons in the outermost energy level of an atom?
- How do you define a valence electron? How do you determine the valence number of an atom?
- Do ionic bonds occur between atoms from adjacent groups?
- Why are the melting point and boiling point of graphite so remarkably high?
- Which statement is INCONSISTENT with Dalton's atomic theory?
- What is Ka for #HClO_4#?
- How do you rank Bronsted acids?
- Which is the stronger acid in each of the following pair #H_2SeO_3# or #H_2SeO_4#?
- Which is the stronger acid in each of the following pair #HBrO_2# or #HBrO#?
- How do you draw the cis and trans isomers for 1-ethyl-3-methylcyclobutane?
- How does a hydrolysis reaction separate a polymer into its monomers?
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- What does it mean for a molecule to be optically active?
- What is the most stable conformer for 3,3-dimethylhexane, viewed along the #C_3-C_4# bond using Newman projections?
- Which group contains a chiral carbon? #A.# #"1-bromopropane"#. #B.# #"2-bromopropane"#. #C.# #H_3C−CH_2CHBrCH_2CH_3#. #D.# #"cyclohexyl bromide"#
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Chemistry Steps
General Chemistry Practice Problems
Chemistry Steps offers thousands of practice problems on topics of general chemistry such as atoms, molecules, isotopes, mole, molar mass, the stoichiometry of chemical reactions, and related molar calculations including limiting reactant and percent yield.
Over 1000 Practice Questions
Significant Figures Practice Problems
Dimensional Analysis Practice Problems
Naming Ionic and Covalent Compounds
Lewis Structures Practice Problems
VSEPR Theory Practice Problems
Calculating Different Concentrations
Colligative Properties Practice Problems
Kinetics Practice Problems
Chemical Equilibrium Practice Problems
Acids and Bases Practice Problems
Buffer Solutions Practice Problems
K sp and Molar Solubility Practice Problems
Thermodynamics, Δ H , Δ S , and Δ G Practice Problems
General Chemistry Quizzes
You read all the articles of the chapter and watched lots of videos, but need to assess your skills before the general chemistry exam?
Multiple choice quizzes might be the “easy” way of glancing through the key concepts and getting feedback on what you need to work on more.
Here are the general chemistry quizzes available to practice the following topics:
Quiz: Matter, Chemical and Physical Properties
Nomenclature and formulas quiz, atomic structure, mass, and isotopes quiz, significant figures quiz, dimensional analysis in chemistry quiz, mass, moles, and number of particles quiz, the stoichiometry of chemical reactions quiz, reactions in aqueous solutions quiz, oxidation state and redox reactions quiz, a multiple-choice quiz on gases, thermochemistry quiz, electronic structure of atoms quiz, periodic table and periodic trends, chemical bonding and lewis structures quiz, geometry and hybridization quiz, chemical kinetics quiz, chemical equilibrium quiz, acids and bases quiz, chemical thermodynamics quiz, electrochemistry quiz.
Example Questions
Each question has a hint including the related articles and the Study guide for the given topic!
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The quizzes are available to Chemistry Steps General and Semester subscribers .
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Chemistry: 1001 Practice Problems For Dummies Cheat Sheet
Chemistry: 1001 practice problems for dummies (+ free online practice).
Sign up for the Dummies Beta Program to try Dummies' newest way to learn.
Solving chemistry problems is a great way to master the various laws and calculations you encounter in a typical chemistry class. This Cheat Sheet provides some basic formulas, techniques, and tips you can refer to regularly to make solving chemistry problems a breeze (well, maybe not a breeze, but definitely easier).
Keeping track of units in chemistry calculations
When completing a chemistry calculation, always write the number with the unit. Number, unit — it’s like having a first and last name.
Consistently writing down the units allows you to see what cancels and helps you spot an error when units don’t cancel. For example, look at the following conversion from miles to kilometers. The correct setup gives you an answer in kilometers. The incorrect setup gives you an answer in square miles per kilometer, which doesn’t make sense.
Balancing chemical equations
A chemical equation shows what happens in a chemical reaction. As in any equation, the elements on the left side of the equation (the reactants) must equal the elements on the right (the products). Here are just a few things to remember when balancing chemical equations:
Same elements in equal numbers: For an equation to be balanced, it must have the same number of each element on each side of the equation. The mass of the reactants has to equal the mass of the products — remember the law of conservation of mass?
Same charge: If there’s a net charge on one side of the equation, the other side of the equation must have the same charge.
Unchanged chemical formulas: Most importantly, never alter a chemical formula! Subscripts (and superscripts for that matter) do not magically change. Change only the coefficients.
Formulas for solving problems dealing with acids and bases
Acid-base reactions and their associated calculations play a primary role in many chemical, biological, and environmental systems. Whether you’re determining hydrogen ion concentration, [H + ]; hydroxide ion concentration, [OH ˗ ]; pH; or pOH, an equation and a calculator are important tools to have in your toolbox. Following are some handy formulas for solving acid/base problems.
Calculating hydrogen or hydroxide ion concentration
The following equation allows you to calculate the hydrogen ion concentration, [H + ], at 25°C if you know the hydroxide ion concentration, [OH – ]; you can also find [OH – ] if you know [H + ]. Just divide 1 × 10 – 14 by the concentration given, and you get the concentration that you need.
To use scientific notation on your calculator, use the EE or EXP key (followed by the exponent) rather than the × 10^ keys.
Calculating hydrogen or hydroxide ion concentration from the pH or pOH
Be familiar with how to solve for [H + ] or [OH – ] when given the pH or pOH (or vice versa). Use the following formulas:
Many scientific and graphing calculators differ in how they handle inputting values and taking logarithms, so know the proper keystroke order for your calculator. Be sure to review your calculator manual or look online.
Calculating pH when given the pOH
Calculating pH when you know the pOH (or vice versa) is probably the easiest of the acid-base calculations. Here’s the formula:
pH + pOH = 14
Simply subtract the given value from 14 (keeping significant digits in mind) to get the value that you need.
Doing titration calculations with a 1:1 acid-to-base ratio
When you’re given titration calculations where the acid and base are reacting in a 1:1 ratio according to the balanced equation, the following equation offers a quick and easy way to solve for either the concentration of one of the substances or the volume necessary to complete the titration:
M A V A = M B V B
If the acid and base aren’t reacting in a 1:1 ratio, use stoichiometry (or dimensional analysis) to solve for your unknown quantity. By the way, stoichiometry works for the 1:1 ratio questions, too; it just takes one or two more steps.
Keep track of your units! Cancel what you need to get rid of and make sure that you still have the units you need in your final answer.
Writing electron configurations
An electron configuration is a description of the relative locations of electrons in an atom or ion. Electron configurations are based primarily on three principles: the Aufbau principle, the Pauli exclusion principle, and the Heisenberg uncertainty principle.
The most important thing to remember is that electrons fill orbitals from lowest energy to highest energy. Think about a hotel with many floors and a broken elevator; getting to the highest floor takes energy — lots of energy. Electrons conserve energy so that the lowest-energy level orbitals fill first.
You can use the following diagram, which is sometimes referred to as the diagonal rule, as an aid when writing electron configurations. Notice that putting an electron in a 3d orbital takes more energy than putting one in a 4s orbital, because 3d orbitals are more complex.
There are other ways to remember the order in which orbitals fill — you can memorize the sequence or use a periodic table.
You may have to write an electron configuration for an ion instead of an atom. If you need to write a configuration for a cation (positive ion), remember to subtract the number of electrons equal to the charge from the total number of electrons before starting. Likewise, if you’re writing a configuration for an anion (negative ion), remember to add the number of electrons equal to the charge to the total number of electrons before starting.
Electron configurations only get more difficult as you choose elements with higher numbers of electrons. You can generally check your work by adding up all the superscripts to make sure that you have the right number of electrons. But note that some elements are exceptions to the diagonal rule.
Your instructor or book should mention these elements and let you know if you’re responsible for knowing how to write their configurations.
About This Article
This article is from the book:.
- Chemistry: 1001 Practice Problems For Dummies (+ Free Online Practice) ,
About the book authors:
Heather Hattori has taught both high school and college level chemistry during her 30+ years in education.
Richard H. Langley, PhD, is on the faculty of Stephen F. Austin State University in Nacogdoches,Texas, where he teaches chemistry.
Richard H. Langley , PhD, is on the faculty of Stephen F. Austin State University in Nacogdoches,Texas, where he teaches chemistry.
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How to Solve a Chemistry Problem
Last Updated: February 15, 2024
This article was co-authored by Anne Schmidt . Anne Schmidt is a Chemistry Instructor in Wisconsin. Anne has been teaching high school chemistry for over 20 years and is passionate about providing accessible and educational chemistry content. She has over 9,000 subscribers to her educational chemistry YouTube channel. She has presented at the American Association of Chemistry Teachers (AATC) and was an Adjunct General Chemistry Instructor at Northeast Wisconsin Technical College. Anne was published in the Journal of Chemical Education as a Co-Author, has an article in ChemEdX, and has presented twice and was published with the AACT. Anne has a BS in Chemistry from the University of Wisconsin, Oshkosh, and an MA in Secondary Education and Teaching from Viterbo University. This article has been viewed 19,668 times.
Chemistry problems can vary in many different ways. Some questions are conceptual and others are quantitative. Each problem requires its own approach, and each has a different way to solve it correctly. What you can do is make a set of steps that can help us with any problems that you come across in the field of chemistry. Using these steps should help give you a guideline to working on any chemistry problem you encounter.
Starting the Problem
Finishing the Problem
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A List of Common General Chemistry Problems
Worked Examples and Worksheets
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This is a collection of worked general chemistry and introductory chemistry problems, listed in alphabetical order.
Alphabetical Index of Chemistry Problem Types
Included in this list are printable pdf chemistry worksheets so you can practice problems and then check your answers. You may also browse chemistry problems according to the type of problem.
A: Absolute Error to B: Boyle's Gas Law
- Absolute Error
- Accuracy Review
- Acid-Base Titration
- Activation Energy Calculation
- Angle Between Two Vectors
- Aqueous Solution Dilutions
- Atomic Mass Overview
- Atomic Mass & Isotopic Abundance
- Atomic Mass from Atomic Abundance
- Atomic Weight Calculation
- Average of a Set of Numbers
- Avogadro's Law
- Avogadro's Gas Law
- Avogadro's Number—Finding Mass of a Single Atom
- Avogadro's Number—Mass of a Known Number of Molecules
- Avogadro's Number—Finding Number of Molecules in a Known Mass
- Balancing Chemical Equations—Tutorial
- Balancing Chemical Equations—Example
- Balancing Redox Reactions—Example and Tutorial
- Balancing Redox Reactions in a Basic Solution—Example
- Balancing Redox Equations—Tutorial
- Bohr Atom Energy Levels
- Bohr Atom Energy Change
- Boiling Point Elevation
- Bond Energies & Enthalpies
- Bond Polarity
- Boyle's Law
- Boyle's Gas Law
C: Calorimetry & Heat Flow to D: Dilutions From Stock Conversions
- Calorimetry & Heat Flow
- Carbon-14 Dating
- Celsius to Kelvin Temperature Conversion
- Charles' Gas Law
- Clausius-Clapeyron Equation
- Concentration and Molarity—Determine a Concentration From A Known Mass of Solute
- Concentration and Molarity—Preparing a Stock Solution
- Concentration and Molarity—Finding Concentration of Ions in an Aqueous Solution
- Covalent Bond Examples
- Dalton's Law of Partial Pressures
- de Broglie Wavelength Calculation
- Density Calculation
- Density of a Solid and a Liquid
- Density Example Problem—Finding Mass From Density
- Density of an Ideal Gas
- Diamagnetism
- Dilutions from Stock Solutions
E: Electron Configuration to G: Guy-Lussac's Gas Law
- Electron Configuration
- Electron Volt to Joule Conversion
- Electronegativity
- Empirical Formula
- Calculate Empirical and Molecular Formula of a Compound
- Enthalpy Change - Enthalpy Change of a Reaction
- Enthalpy Change - Enthalpy Change of a Reaction of a Given Mass
- Enthalpy Change - Enthalpy Change of Water
- Entropy Calculation
- Entropy Change
- Entropy of Reaction
- Equation of a Line
- Equilibrium Constant
- Equilibrium Constant for Gaseous Reactions
- Equilibrium Concentration
- Experimental Error
- Feet to Inches Conversion
- Free Energy and Pressure
- Free Energy and Reaction Spontaneity
- Formal Charge - Lewis Structure Resonance Structures
- Freezing Point Depression
- Frequency to Wavelength Conversion
- Graham's Law
- Gram to Mole Conversion
- Guy-Lussac's Gas Law
H: Half-Life to Joule to E: Electron Volt Conversion
- Heats of Formation
- Henderson-Hasselbalch Equation
- Henry's Law
- Ideal Gas Example Problem
- Ideal Gas Law
- Ideal Gas—Constant Pressure
- Ideal Gas—Constant Volume
- Ideal Gas Example Problem—Partial Pressure
- Ideal Gas Example Problem–Unknown Gas
- Ideal Gas vs Real Gas—van der Waals Equation
- Ionic Bond Examples
- Ionic Bond from Electronegativity
- Isotopes and Nuclear Symbols—Example 1
- Isotopes and Nuclear Symbols—Example 2
- Joule to Electron Volt Conversion
L: Law of Multiple Proportions to M: Molecular Mass Calculations
- Law of Multiple Proportions
- Length Conversion—Angstroms to Meters
- Length Conversion—Angstroms to Nanometers
- Length Conversion—Centimeters to Meters
- Length Conversion—Feet to Kilometers
- Length Conversion—Feet to Meters
- Length Conversion—Kilometers to Meters
- Length Conversion—Miles to Kilometers
- Length Conversion — Millimeters to Centimeters
- Length Conversion — Millimeters to Meters
- Length Conversion — Micrometers to Meters
- Length Conversion — Nanometers to Meters
- Length Conversion — Nanometers to Angstroms
- Length Conversion — Yards to Meters
- Draw a Lewis Structure
- Draw a Lewis Structure — Octet Rule Exception
- Limiting Reactant & Theoretical Yield
- Mass Conversions — Kilograms to Grams
- Mass Conversions — Pounds to Kilograms
- Mass Conversions — Ounces to Grams
- Mass — Energy Relations in Nuclear Reactions
- Mass of Liquid from Density
- Mass Percent Composition
- Mass Percent Composition—Example 2
- Mass Relations in Balanced Equations
- Mean of a Set of Numbers
- Mean, Median, Mode and Range Example
- Molarity to PPM Conversion
- Mole — Gram Conversions
- Mole Relations in Balanced Equations
- Moles of C Atoms in 1 Mol Sucrose
- Molecular Formula from Simplest Formula
- Molecular Mass Calculations
N: Nernst Equation to P: Protons, Neutrons, and Electrons
- Nernst Equation
- Neutralizing a Base with an Acid
- Osmotic Pressure
- Oxidation and Reduction
- Oxidation or Reduction?
- Assigning Oxidation States
- Paramagnetism
- Percent Composition by Mass
- Percent Error
- pH Calculation
- pH Calculation — Example 2
- pH of a Strong Acid
- pH of a Strong Base
- Phosphate Buffer Preparation
- pOH Calculation
- Polyprotic Acid pH
- Population Standard Deviation
- Precision Review
- Predicting Formulas of Compounds with Polyatomic Ions
- Predicting Formulas of Ionic Compounds
- Prepare a Solution (Molarity)
- Pressure Conversion - Pa to atm
- Pressure Conversion — millibar to atm
- Pressure Conversion — atm to Pa
- Pressure Conversion — bars to atm
- Pressure Conversion — atm to bars
- Pressure Conversion — psi to atm
- Pressure Conversion — atm to psi
- Pressure Conversion — psi to Pa
- Pressure Conversion — psi to millibars
- Protons & Electrons in Ions
- Protons & Electrons in Ions — Example 2
- Protons, Neutrons, and Electrons in Atoms/Ions
R: Radioactive Decay to T: Titration Concentration
- Radioactive Decay — α Decay
- Radioactive Decay — Electron Capture
- Radioactive Decay — β - Decay
- Raoult's Law — Example 1
- Raoult's Law — Example 2
- Raoult's Law — Example 3
- Rate of Radioactive Decay
- Rates of Reaction
- Reactions in Aqueous Solution
- Reaction Quotient
- Redox Reaction
- Relative Error
- Root Mean Square Velocity of Ideal Gas Molecules
- Sample Standard Deviation
- Scientific Notation
- Significant Figures
- Simplest Formula from Percent Composition
- Solubility from Solubility Product
- Solubility Product from Solubility
- Temperature Conversions
- Temperature Conversions—Kelvin to Celsius & Fahrenheit
- Temperature Conversions—Celsius to Fahrenheit
- Temperature Conversions—Celsius to Kelvin
- Temperature Conversions—Kelvin to Celsius
- Temperature Conversions—Fahrenheit to Celsius
- Temperature Conversions—Fahrenheit to Kelvin
- Temperature That Fahrenheit Equals Celsius
- Theoretical Yield
- Theoretical Yield #2
- Titration Concentration
U: Uncertainty to W: Wavelength to Frequency Conversion
- Uncertainty
- Unit Cancelling — English to Metric
- Unit Cancelling — Metric to Metric
- Unit Conversions
- Unit Conversion — What Is The Speed Of Light In Miles Per Hour?
- Vector Scalar Product
- Volume Conversions — Cubic Centimeters to Liters
- Volume Conversions — Cubic Feet to Cubic Inches
- Volume Conversions — Cubic Feet to Liters
- Volume Conversions — Cubic Inches to Cubic Centimeters
- Volume Conversions — Cubic Inches to Cubic Feet
- Volume Conversions — Cubic Meters to Cubic Feet
- Volume Conversions — Cubic Meters to Liters
- Volume Conversions — Gallons to Liters
- Volume Conversions — Cubic Inches to Liters
- Volume Conversions — Fluid Ounces to Milliliters
- Volume Conversions — Liters to Milliliters
- Volume Conversions — Microliters to Milliliters
- Volume Conversions — Milliliters to Liters
- Volume Percent
- Wavelength to Frequency Conversion
Chemistry Worksheets (Pdf to Download or Print)
- Metric to English Conversions Worksheet
- Metric to English Conversions Answers
- Metric to Metric Conversions Worksheet
- Metric to Metric Conversions Answers
- Temperature Conversions Worksheet
- Temperature Conversions Answers
- Temperature Conversions Worksheet #2
- Temperature Conversions Answers #2
- Moles to Grams Conversions Worksheet
- Moles to Grams Conversions Answers
- Formula or Molar Mass Worksheet
- Formula or Molar Mass Worksheet Answers
- Practicing Balancing Chemical Equations — Worksheet
- Balancing Chemical Equations — Answers
- Practicing Balancing Chemical Equations — Worksheet #2
- Balancing Chemical Equations — Answers #2
- Practicing Balancing Chemical Equations — Worksheet #3
- Balancing Chemical Equations — Answers #3
- Common Acid Names & Formulas — Worksheet
- Acid Names and Formulas — Answers
- Practice Calculations with Moles — Worksheet
- Mole Calculations — Answers
- Practice Mole Relations in Balanced Equations — Worksheet
- Mole Relations in Balanced Equations — Answers
- Gas Laws Answers
- Gas Laws Answers — Shown Work
- Limiting Reagent — Worksheet
- Limiting Reagent — Answers
- Calculating Molarity — Worksheet
- Calculating Molarity — Answers
- Acid & Base pH — Worksheet
- Acid & Base pH — Answers
- Electron Configurations — Worksheet
- Electron Configurations — Answers
- Balancing Redox Reactions — Worksheet
- Balancing Redox Reactions — Answers
- Resources for Finding Answers to Chemistry Questions
- How to Pass Chemistry Class
- Calculate Simplest Formula From Percent Composition
- Ideal Gas Law: Worked Chemistry Problems
- How to Convert Grams to Moles and Moles to Grams
- Law of Multiple Proportions Example Problem
- Calorimetry and Heat Flow: Worked Chemistry Problems
- Rate of Radioactive Decay Worked Example Problem
- Molality and Concentration of a Chemical Solution
- Introduction To Stoichiometry
- How to Calculate Experimental Error in Chemistry
- Acids and Bases: Calculating pH of a Strong Acid
- Aqueous Solution Chemical Reaction Problem
- How to Calculate Limiting Reactant and Theoretical Yield
- Polyprotic Acid Example Chemistry Problem
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7.2 / 2.4 = 3 half-lives (1/2) 3 = 0.125 (the amount remaining after 3 half-lives) 100.0 g x 0.125 = 12.5 g remaining
20.0 / 3.6 = 5.56 half-lives (1/2) 5.56 = 0.0213 (the decimal fraction remaining after 5.56 half-lives) (6.02 x 10 23 ) (0.0213) = 1.28 x 10 22 atoms remain
(1/2) 3 = 0.125 (the amount remaining after 3 half-lives) 10.0 g x 0.125 = 1.25 g remain 10.0 g − 1.25 g = 8.75 g have decayed Note that the length of the half-life played no role in this calculation. In addition, note that the question asked for the amount that decayed, not the amount that remaning.
2.00 mg / 128.0 mg = 0.015625
(1/2) n = 0.015625 n log 0.5 = log 0.015625 n = log 0.5 / log 0.015625 n = 6
24 days / 6 half-lives = 4.00 days
17/32 = 0.53125 (this is the decimal amount that remains) (1/2) n = 0.53125 n log 0.5 = log 0.53125 n = 0.91254 (this is how many half-lives have elapsed) 60 min / 0.91254 = 65.75 min n = 66 min (to two sig figs)
(1/2) n = 0.01 n log 0.5 = log 0.01 n = 6.64 6.64 x 8.040 days = 53.4 days
0.334 x 10 = 3.34 seconds
24.0 hr / 23.9 hr/half-life = 1.0042 half-lives One day = one half-life; (1/2) 1.0042 = 0.4985465 remaining = 4.98 g Two days = two half-lives; (1/2) 2.0084 = 0.2485486 remaining = 2.48 g Seven days = 7 half-lives; (1/2) 7.0294 = 0.0076549 remaining = 0.0765 g
5.00 / 100.0 = 0.05 (decimal fraction remaining) (1/2) n = 0.05 n log 0.5 = log 0.05 n = 4.32 half-lives 36.0 hours x 4.32 = 155.6 hours
If you lose 75%, then 25% remains. Use 0.25 rather than 25%. (1/2) n = 0.25 n = 2 (remember (1/2) 2 = 1/4 and 1/4 = 0.25) 12.26 x 2 = 24.52 years
(1/2) n = 0.25 n log 0.5 = log 0.25 n = log 0.25 / log 0.5 n = 2
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Chemistry Problem Solver Online
Every person who desires to study chemistry thoroughly and develop serious and useful knowledge of this subject from time to time requires access to helpful web resources. Resources that will help as a roadmap for their academic career. We will go through the list of them in this post and look through the advantages of these websites.
TOP 3 chemistry homework help sites where you can solve your problems right away:
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If those strange equations a chemistry teacher writes on a chalkboard drive you crazy instead of driving you curious, there’s no need in torturing yourself. Thanks to the digital and technological progress, you can find a chemistry problem solver for any occasion. Here are some alternative sources you can use.
- pH Calculator
- Balancing Chemical Equations
- Mole Calculator
- Half Life Calculator (second order reaction)
- Nomenclature
- Chemical equation calculator
- Philip Harris Molarity Calculator
- Chemical Reaction Calculator
- Reaction balancer
- Frequency Factor Calculator
- Element Finder
- Generador de Estructuras de Lewis ITPA
- Half Life Calculator (zero order reaction)
- VSEPR Widget
- Electron Configuration Calculator
- Phase Diagram
- Chemical formula
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- Flash Point Calculator
- Find and Convert Gram Formula Mass
- NFPA Labels for Chemicals
- Lewis structure
- Half Life Calculator (first order reaction)
- Compound Identifier
- 3-D Chemical Structure Generator
- Ideal Gas Law
- Molecular Structure Creator
- Chemical Compund Drawer
- Solutions Calculator
- JOULES to eV
- Online Problem Solver
- Molar Mass Calculator
- Reagent Table Properties II
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Pls solve this for me and give me the answer immediately Zinc reacts with HCL to form ZNCL balance the equation
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the relative rate of diffusion of a gas as compared with oxygen is 2:1. calculate the relative molecular mass of the gas
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Concentration and Molarity—Finding Concentration of Ions in an Aqueous Solution. Covalent Bond Examples. Dalton's Law of Partial Pressures. de Broglie Wavelength Calculation. Density Calculation. Density of a Solid and a Liquid. Density Example Problem—Finding Mass From Density. Density of an Ideal Gas.
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