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How to Solve a Chemistry Problem
Last Updated: July 14, 2020
wikiHow is a “wiki,” similar to Wikipedia, which means that many of our articles are co-written by multiple authors. To create this article, volunteer authors worked to edit and improve it over time. This article has been viewed 9,857 times. Learn more...
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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Chemistry: 1001 Practice Problems For Dummies Cheat Sheet
Chemistry: 1001 practice problems for dummies (+ free online practice).
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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.
This article can be found in the category:
- Chemistry ,
- Writing Electron Configurations
- Formulas for Solving Problems Dealing with Acids and Bases
- Keeping Track of Units in Chemistry Calculations
- Balancing Chemical Equations
- Special Limit Formulas in Calculus
- View All Articles From Book
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Chemistry Help - Basic to Advanced Chemistry questions
TutorEye has the best place for chemistry help as we have the right resources for you to learn and grow your chemistry knowledge.
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7. If 24.8 mol of Ar gas occupies 185.6 L, how many mL would occupy 49.3 mol occupy under the same ... erature and pressure? Record your answer in scientific notation using 3 significant figures. View More
8. Mole Conversion practice for chemistry
Core Chemistry Topics:
Acids and bases :.
Acids are defined as the species which have a tendency to donate protons H+ in its aqueous solution or accept electrons.
Bases are the species which accept protons H+ in its aqueous solution or donate electrons.
HCl + NH3 → Cl- + NH4+ Here, HCl donates protons and acts as an acid and NH3 accepts protons and acts as a base.
Alkanes, Cycloalkanes and Functional Groups:
Alkane- The class of hydrocarbons which form a saturated (single bond) carbon system and has a chemical formula of CnH2n+2, where ‘n’ is the number of atoms.
For example – C2H6, n = 2
Cycloalkanes - The class of hydrocarbons which has two hydrogen lesser than alkanes CnH2n , where n and have a ring like structure.
For example - cyclobutane; C4H8
Functional groups - The class of groups of atoms within molecules have their own specific properties and perform characteristic chemical reactions.
By today, there are a total 14 functional groups.
Each of it has arranged in order of their increasing priorities, for IUPAC Nomenclature.
For example - Some of list of functional groups.
Atoms , Compounds and Ions:
Atoms – The smallest particle a chemical element is termed as atom. It was first Introduced by Dalton in 1803 AD.
The atoms are indivisible units of chemical elements that are identical for the same kind.
For example - 2 H atoms in hydrogen molecule H2
Compounds – These are the combinations of atoms of more than one element held together by chemical bonds.
For example - H2O compound Composed of H and O atoms
Ions - These are species like atoms or molecules carrying a net electrical charge (cation or anion).
Here, positively charged ions are called ‘cations’ and negatively charged ions as ‘anions’.
For example - Na+ sodium atom loses an electron to give sodium ‘cation’.
Buffers, Titrations and Solubility Equilibria:
Buffers – A solution of mixture of weak acid and its conjugate base or weak base and its conjugate acid is termed as buffer. The major role of it is to resist the change in pH.
For example- An acidic buffer of Acetic acid – sodium acetate CH3COOH-CH3COONa
Titrations – A quantitative analysis of determination of analyte concentration.
A standard solution of titrant (known concentration ) taken in burette , by using a suitable indicator is added dropwise into the solution of unknown concentration ( analyte )
For example - HCl as an analyte , is titrated against NaOH using an indicator.
Solubility equilibria - It is a dynamic equilibrium between undissolved solids and its ionic species in solution.
The solubility is estimated by the solubility product that is Ksp.
For example - AgCl solid dissolved in aqueous medium
AgCl (s) --> Ag+ (aq) + Cl- (aq)
It is the Intermolecular forces of attraction between atoms, ions or molecules that form the chemical compounds.
For example -
Formation of ionic bonds due to electrostatic forces between oppositely charged ions ( NaCl ) whereas covalent bonds due to sharing of electrons (CH4)
It is a type of dynamic equilibrium that maintains concentration between reactants and products in which the rate of forward reaction equals the rate of backward reactions at certain times.
Chemical Reactions and Compounds:
The type of reaction between one or more reactants to give products during which there is simultaneous breaking and forming of bonds of species or compounds.
Chemical reactions are of many types –
- Decomposition reaction
- Combination reaction
- Displacement reaction
- Double displacement reaction
2Mg + O2 --> 2 MgO
Chemical kinetics is the branch of chemistry, that mainly deals with the rate of chemical reaction. The rate of chemical reaction indicate the change in the concentration of reactant and product with time. Thus, the kinetics of a chemical reaction interpret the speed and rate of change during chemical process.
The branch of chemistry deals with the non spontaneous occurrence of chemical reactions due to electricity.
In this way, there is interconversion of electrical energy into chemical energy.
For example – In electrolysis, chemical reaction takes place due to electrical energy whereas in a battery or cell the reverse process takes place.
Electronic Structure of Atom:
It is the arrangement of electrons on shells of a spherical atomic structure. Also the number of electrons is defined by the atomic number of an element.
For example - lithium with atomic number = 3
Exothermic and Endothermic Reactions:
Exothermic reaction - The type of reaction which releases or produces an amount of energy in the form of heat or light. For example -
Endothermic reaction – The type of energy which absorbs or requires a certain amount of energy in the form of heat or light.
It is the distribution of electrons within atomic orbitals in order of increasing energy of the levels, followed by some rules.
1s, 2s, 2p, 3s,3p,4s,3d, 4p,5s,4d,5p,6s,4f,5d,6p,7s,5f
Kinetic Molecular Theory of Gases:
It is simple theory and it explains thermodynamic behavior of gases. This theory of gases explains the macroscopic properties of gases like Volume , Pressure and temperature and also transport properties. According to this theory gases are made up of a large number of molecules and they are flying in a random direction with particular speed. By knowing the speed of gases molecules easily we can figure out macroscopic properties. According to this theory Kinetic energy is directly proportional to temperature.
Mass Spectrometry :
It is analytical technique and it is used to measure mass to charge ratio of ions and it result as a mass spectrum and this measurement used to calculate exact molecular weight and mass spectrometry also used to identify unknown compounds and also used to determine the structure and chemical properties of molecule.
Mass spectrometry consists of three components such as
1. Ionization source 2. Mass analyser 3. Ion detection system.
It refers to the identity of molecule and relative number of the chemical elements that make any particular molecule.
2- Hydrogen atoms
Nomenclature of Chemical Compounds:
The chemical compounds can be named with the help of IUPAC rules. The IUPAC rules is a set of certain rules that provides a way to name any organic or inorganic chemical compounds. For example; name of CH3-CH2-CH2-CH3 must be butane as there are 4 C atoms so the root word must be but- with -ane as suffix because all the C atoms are bonded single covalent bonds.
Net Ionic Equations:
The net ionic equation is the representation of chemical equation in the form of ions. It represents the ionic form with the physical state of all the ions. The spectator ions are not part of the net ionic equation as they are placed at either side of the chemical equation. For example:
Nuclear Chemistry :
It is a branch of chemistry that deals with the study of nucleus and nuclear reactions in an atom .Nuclear reactions are different chemical reactions . In chemical reactions atoms combine without undergoing any change in nucleus whereas nuclear reaction is one which proceeds with a change in the composition of the nucleus so it will produce atoms of a new element.
Organic Chemistry :
Organic chemistry is the study of the structure , properties , composition , preparation and reactions of carbon containing compounds and along with Carbon it includes Hydrogen , Nitrogen , Oxygen atoms also.
Oxidation Numbers :
It is defined as the charge of an atom that appears to have on forming ionic bonds with other heteroatoms and also atom having high electronegativity even if it forms covalent bond.
Periodic Table and Periodic Properties:
The table of the chemical elements arranged in order of atomic number from lowest atomic number to highest atomic number, electronic configuration and recurring chemical properties usually arranged in rows and columns.
The phenomenon of repetition of similar properties of elements at regular intervals in periodic tables is called periodicity and it is called periodic properties.
Periodic properties includes
1. Atomic radii 2.Ionisation potential 3. Electron affinity 4.Electronegativity 5. Oxidation number 6. Electro positivity 7.Valency
It is a type of chemical reaction that involves a transfer of electrons between two chemical species. One species undergoes oxidation while another undergoes reduction. This oxidation and reduction reactions occur simultaneously. The substance which is getting reduced is known as Oxidizing agent and the substance which is getting oxidized is called reducing agent.
States of Matter and Intermolecular forces:
States of Matter:
It is defined as one of the way to describe the behavior of atoms and molecules in a substance
There are six states of matter
1. Solid state 2. Liquid state 3.Gaseous state 4. Plasma state 5.Bose Einstein condensate state 6. Fermionic condensate state
Intermolecular forces are the attraction forces or repulsion forces which act between neighboring particles such as in between atoms, molecules or ions.
These are the isomeric molecules which have same molecular formula but only differ in spatial arrangement
Cis –but-2-ene Trans -But -2-ene
It is a branch of chemistry that deals with the application of the law of definite proportions and of the conservation of mass and it is the study of quantitative relationship or ratios between two or more substances undergoing physical change or chemical change. Stoicheion means element and metron is a measure and it also deals with the mass or volumes of products and reactants.
Solids and Liquids:
Solid is one of the fundamental states of matter and its molecules are closely packed together and this state of matter is having least kinetic energy. Solids are characterized by structural rigidity and for moving solid objects one definitely needs to apply force to the surface.
Liquids are substances which have an indefinite shape, size and definite volume and are incompressible, loosely packed and free flowing state of matter.
Solution is a homogeneous mixture and it consists of two or more components. Size of particles in solution is smaller than 1 nm. All the solutions contain two common components one is solute and other one is solvent.
Solute quantity in solution is very less and solvent quantity in solution is very high compared to solute.
Examples : Sugar in water, salt in water
Thermodynamics is the branch of physical chemistry and it deals with heat, work and temperature and it interrelates this parameter with chemical reactions or with physical changes of state.
Other Core Chemistry Homework Topics
O2 lewis structure, of2 lewis structure, formal charge formula, n2 lewis structure, density of mercury, c2h2 lewis structure, xef2 lewis structure, rotational symmetry, cs2 lewis structure, density of water, solubility rules, amino acid chart, enthalpy equation, uncompetitive inhibition, c2h4 lewis structure, henderson hasselbalch equation, rate of change, sample chemistry homework help – questions and answers.
1 . In the addition reaction between 1-butyne and hydrogen iodide, two different products can be formed. Identify the name of a major product.
Explanation : 1-butyne is a terminal alkyne in which the triple bonded C atoms are placed at one of the terminal of the molecule. The addition of HI follows the Markovnikov addition (electrophilic addition reaction) that leads to more stable product. Two products are 2-iodo-1-butene and 2,2-diiodobutane.
2 . When 3-methyl-3-chlorohexane is heated to boiling together with NaOH (aq), 3-methyl-3-hexanol is formed as the main organic product. Which type of mechanism is followed by the reaction?
- nucleophilic rearrangement reaction
- nucleophilic addition reaction
- nucleophilic substitution reaction
- electrophilic substitution reaction
Explanation : The reaction follows the nucleophilic substitution reaction. The mechanism proves the reaction of 3-methyl-3-chlorohexane with NaOH (aq) to form 3-methyl-3-hexanol as a nucleophilic substitution reaction. Here nucleophile OH- attacks on more stable tertiary carbocation formed during SN1 mechanism.
3 . What is the rational name of the major product formed when a solution of 2-methyl-1-butene is added hydrogen iodide, HI?
Explanation : The 2-methyl-1-butene can form primary and secondary carbocation as intermediate. Due to hyper conjugation, secondary carbocation is more stable than primary carbocation. Therefor; secondary carbocation forms as major product and primary carbocation forms as minor product.
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Wolfram|alpha as the way to bring computational knowledge superpowers to chatgpt, active learning with wolfram|alpha notebook edition, chemistry step-by-step solutions: chemical reactions.
If you’re studying chemistry or are in a discipline requiring chemistry prerequisite courses, then you know how expensive the required textbooks can be. To combat this, the chemical education community has developed open educational resources to provide free chemistry textbooks. However, although free textbooks keep cash in your wallet, they don’t include solution guides for all the homework problems.
Luckily, the Step-by-Step Solutions feature of Wolfram|Alpha has got your back! Whether you’re studying remotely or collaborating via video conferencing, Wolfram|Alpha helps you learn and apply the problem-solving frameworks for chemical word problems. The step-by-step solutions provide stepwise solution guides that can be viewed one step at a time or all at once. The guides not only hone efficient problem solving, but also facilitate digging deeper into concepts that might still be murky.
Over the next few weeks, we’ll be exploring some of the popular topics that middle-school, high-school and college students encounter in their chemistry courses and final exams: chemical reactions, structure and bonding , chemical solutions , and finally, quantum chemistry . Read on for example problems in chemical reactions and their step-by-step solutions!
Balancing Chemical Equations
A fundamental aspect of chemistry is balancing chemical equations . If chemical equations are the language in which chemical processes are expressed, then balancing chemical equations is the corresponding grammar. The step-by-step solution walks you through a robust algebraic approach to identifying the stoichiometric coefficients.
Write the balanced equation for the reaction of copper with nitric acid to produce copper nitrate, nitrogen oxide and water.
For this class of problem, just enter “ balance copper + nitric acid -> copper nitrate + nitrogen dioxide + water ”.
After balancing the related chemical equations, the next step in planning a laboratory experiment is computing how much of each reactant must be measured out. To do this, one needs the molar mass for each reactant. Step-by-step solutions are available for the molecular mass and relative molecular mass in addition to the molar mass . In all cases, a general framework for solving these types of problems is provided via the Plan step. Details of which formula to use and how to gather the necessary information are provided.
Calculate the molar mass of silver sulfate, Ag 2 SO 4 .
In this case, just enter “ molar mass silver sulfate ”.
One way to analyze individual chemicals is to compute and compare the mass and atom percentages. The step-by-step solution provides a general framework for solving this class of problem in the Plan step. Details of the relevant equations, as well as how to compute the necessary intermediate values, are provided. Ways in which you can check your work during the calculations are also available via the “Show intermediate steps” buttons.
Antihemophilic factor is a coagulant with the formula C 11794 H 18314 N 3220 O 355 S 83 . What is its percent composition?
For the answer, just enter “ antihemophilic factor elemental composition ”.
Chemical conversions crop up in nearly every chemistry homework or research problem. As such, step-by-step solutions are available for converting among moles , mass , volume , molecules and atoms . Unit conversions and dimensional analysis details are provided.
How many atoms are in five milliliters of a 1.5 mM magnesium hydroxide solution?
To solve this, just enter “ convert 5 mL of 1.5 mM magnesium hydroxide to atoms ”.
After running a chemical reaction, one often wants to know how the reaction went by computing the reaction yields . Step-by-step solutions are available for computing the amount of reactants needed and the theoretical yield in addition to the percent yield . The use of stoichiometric factors to generate the desired values is explained in detail.
Upon reaction of 1.274 grams of copper sulfate with excess zinc metal, 0.392 grams of copper metal was obtained according to the following equation: CuSO 4 (aq)+Zn(s)⟶Cu(s)+ZnSO 4 (aq). What is the percent yield?
To find the percent yield, just append the mass values to the corresponding chemical species and ask for the stoichiometry, “ 1.274 g CuSO4 + Zn -> 0.392 g Cu + ZnSO4 stoichiometry ”.
Test your chemical reaction problem-solving skills by using the Wolfram|Alpha tools described to solve these word problems. Answers will be provided in the next blog post in this series.
- Compute the molecular mass of acetaminophen. Is the element with the largest atom count also the element with the largest mass percent?
- What is the limiting reactant and theoretical yield when 24.8 grams of white phosphorus and 0.200 moles of oxygen react to form 10.0 grams of phosphorus pentoxide?
And More Chemistry to Come
Whether you’re studying for upcoming final exams, puzzling out homework or just looking for a refresher, chemical reactions are one of many chemistry topics covered by the Wolfram|Alpha knowledgebase. Next week we’ll cover step-by-step solutions for chemical solutions , followed by structure and bonding , and then quantum chemistry . If you have suggestions for other step-by-step content (in chemistry or other subjects), please let us know! You can reach us by leaving a comment below or sending in feedback at the bottom of any Wolfram|Alpha query page.
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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.
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.
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.
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.
Practice chemistry problems naming ionic compounds, hydrocarbons, and covalent compounds.
- Practice naming covalent compounds.
- Learn hydrocarbon prefixes in organic chemistry.
These chemistry problems involve isotopes, nuclear symbols, half-life, radioactive decay, fission, fusion.
- Review the types of radioactive decay.
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.
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.
There are some many examples of unit conversions that they have their own separate page!
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Free math problem solver answers your chemistry homework questions with step-by-step explanations.
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Helps with molar mass if your lazy like me.
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Use this collection of example worked chemistry problems with answers to learn problem-solving skills and how to use formulas.