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Top Rated Homework Helpers:

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.

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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

10. Increasing the concentration of a reactant increases

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How to Solve a Chemistry Problem

Last Updated: July 14, 2020

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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.

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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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Chemistry X10 — problem solver 4+

Chemical reactions & formulas, designed for ipad.

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Chemistry X10 solves homework and tests. • Is suitable for 7, 8, 9, 10 and 11 classes • Works without Internet connection • 800 000 downloads TASKS SOLUTIONS Enter: "Given" and "Find" Result: a solved task with explanation and its answer Types of solvable tasks: • by formulas • solutions • mixtures • reaction equation • lack and excess The app does not solve tasks of derivation of the substance formula CHEMICAL REACTIONS Finds reaction equations by entered part 8000 reactions are available without internet connection TRANSFORMATION CHAINS Solves open chains Enter: Cu = CuO = CuCl2 = Cu(OH) 2 Result: 1) Cu + H2SO4 = CuO + SO2 + H2O 2) 4CuO + 2NH4Cl = 3Cu + CuCl2 + N2 + 4H2O 3) 2NaOH + CuCl2 = 2NaCl + Cu(OH)2 COEFFICIENT ARRANGEMENT Arranges the coefficients by fitting or by method of electronic balance Enter: H2 + O2 = H2O Result: 2H2 + O2 = 2H2O MOLAR MASSES Counts molar masses of complex substances. Enter: Cu(OH)2 Result: 98 g / mol. Find in the periodic table all the elements that make up Cu (OH) 2. These are: Cu, O and H ... FORMULAS FOR TASKS Formulas are divided into values parts: mass, molar mass, etc. There are prepared formulas for each of them: mass: m = nM, m = ρV and other. THE PERIODIC TABLE You can find: period, group, atom mass, class, valence, type of crystal lattice, color, temperature of melting and boiling, electronic configuration, energetic levels, electronegativity. PROTECTION FROM TEACHER: Call From Mom and Clock John is cheating on his grand test. The Teacher notices that and tries to take his phone. “Excuse me, my mom is calling”, says John and shows the screen to the Teacher. There is a phone call from John’s mom. “Go to the hall and pick up the phone”, she suggests. In the hall John taps on the lest top corner of the screen – and there is a solved task as before! He remembers the solution and comes back to the classroom. His mom didn’t call him. John has turned on protection from the teacher. There are 2 types of protection in “Chemistry X10” – Call From Mom and Clock. Clock works by default, Call From Mom is available in Pro-version. ----- “Pro-version” is a service upon monthly subscription. It gives you infinite gems and access to features which are available only in “Pro-version”: protection from teacher “Call From Mom” and detailed solution of tasks. “Pro-version” costs 1.99 USD (equivalent in local currency) per week. Subscription will be updated automatically if you don't turn off auto-extension of subscription 24 hours before current subscription expiration. Payment will be proceeded from your iTunes account during 24 hours before current subscription expiration. User can manage the subscriptions. You can turn off auto-extension after purchase in account settings. Privacy Policy: appcrab.net/privacy-policy Terms of Use: appcrab.net/terms-of-use

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d. Hydrogen is produced industrially from methane through the reaction CH4(g) + H20(g) + heat =Co(g) + 3H2(g). The following diagram represents this reaction. Use this information to answer the following questions. (14 points)

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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.

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.

For example,

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)

Chemical Bonds:

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)

Chemical Equilibrium:

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 –

2Mg + O2 --> 2 MgO

Chemical-kinetics :

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.

Electro-Chemistry:

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.

Electronic Configuration:

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

For example-

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.

Molecular Composition:

It refers to the identity of molecule and relative number of the chemical elements that make any particular molecule.

2- Hydrogen atoms

4-Oxygen 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.

Periodic properties:

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

Redox Reactions:

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:

Intermolecular forces are the attraction forces or repulsion forces which act between neighboring particles such as in between atoms, molecules or ions.

Stereoisomers:

These are the isomeric molecules which have same molecular formula but only differ in spatial arrangement

Cis –but-2-ene Trans -But -2-ene

Stoichiometry:

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.

Solutions:

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:

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.

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To study high school chemistry, you must first and foremost analyze whether you know the fundamentals of the subject. You can easily study and revise the basics by studying from our highly qualified Chemistry experts. Nonetheless, make sure you practice the equations and study the properties of the substances regularly. With the help of diagrams and study notes provided by our professionals, you can invest time in understanding the step-by-step processes involved in a reaction. The key to doing well in high school is practice and regular revision of key principles. Here at TutorEye we can make this journey easier for you and help you get good grades in the subject.

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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.

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.

Example Problem

Write the balanced equation for the reaction of copper with nitric acid to produce copper nitrate, nitrogen oxide and water.

Step-by-Step Solution

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 ”.

Mass Composition

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

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 ”.

Stoichiometry

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 ”.

"1.274 g CuSO4 + Zn -> 0.392 g Cu + ZnSO4 stoichiometry"

Challenge Problems

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.

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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Chemistry Problems With Answers

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 .

Atomic Structure Problems

Learn about atomic mass, the Bohr model, and the part of the atom.

Chemical Bonds

Learn how to use electronegativity to determine whether atoms form ionic or covalent bonds. See chemistry problems drawing Lewis structures.

Chemical Equations

Practice writing and balancing chemical equations.

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.

Error Calculations

Learn about the types of error and see worked chemistry example problems.

Equilibrium Chemistry Problems

Learn about Le Chatelier’s principle, reaction rates, and equilibrium.

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.

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.

Molecular Structure Chemistry Problems

See chemistry problems writing chemical formulas. See examples of monatomic and diatomic elements.

Nomenclature

Practice chemistry problems naming ionic compounds, hydrocarbons, and covalent compounds.

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.

Physical Chemistry

Explore thermochemistry and physical chemistry, including enthalpy, entropy, heat of fusion, and heat of vaporization.

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.

Unit Conversions

There are some many examples of unit conversions that they have their own separate page!

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Chemistry Step-by-Step Solutions: Chemical Reactions
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