## Core Concepts

In this tutorial, you will learn what is **stoichiometry** and the different types of problems involving it. You will go through several examples to practice and master the content!

## Topics Covered in Other Articles

- Balancing Chemical Equations
- What is a Chemical Reaction?
- Calculating Molar Mass
- Percent Yield Calculation
- How to Calculate Molarity
- What Are Significant Figures

## Stoichiometry Definition

### What is Stoichiometry?

**Stoichiometry **is math having to do with chemical reactions. There are different types of calculations you can perform; stoichiometry with moles is the most common, but you can also do math with masses and even percentages. Read about the origins of stoichiometry here! Learn what is mole in chemistry.

### Stoichiometric Ratio

A stoichiometric ratio comes into play when talking about the relationships of elements or molecules in specific problems. This is the exact ratio between the coefficients of the reactants and products needed for a reaction to proceed normally. Let’s work through some problems you may see when learning about stoichiometry.

## Stoichiometry Problems

### Balancing Chemical Equations

A very common type of stoichiometric problem is balancing equations. This is an important chemistry skill to have because you have to have the correct ratio of reactants and products in order for a reaction to proceed; this is also an important foundation for organic chemistry. Although we have a tutorial on balancing equations, let’s look at one example.

Balance the following reaction:

The main idea when balancing equations is that there should be the same number of each element on both sides of the reaction. You can balance the carbons and the hydrogens first, then move onto the oxygen. The balanced equation should look like this:

### Example – Using Stoichiometric Ratio (Moles)

Use the equation below to solve the problem.

If of C_{6}H_{12}O_{6} reacts, how many moles of carbon dioxide are produced?

Using dimensional analysis, you can use the stoichiometric ratio to find the solution to this problem. By looking at the coefficients, you can see that for every of C_{6}H_{12}O_{6}, of CO_{2} are produced. Using this ratio, you can figure out how many moles of carbon dioxide are made from of glucose.

### Example – Using Stoichiometric Ratio (Mass)

Let’s use the same equation as the problem above.

How many grams of C_{6}H_{12}O_{6} was initially used if of C_{2}H_{5}OH was produced?

Similar to the previous problem, by using the stoichiometric ratio of reactant to product, you can find the answer. Dimensional analysis is used to go from grams of C_{2}H_{5}OH to molar mass to mole (stoichiometric) ratio and back to grams.

## Stoichiometry Practice Problems

**Problem 1**

You mix of CaCl_{2} into a solution with excess AgNO_{3}, hence CaCl_{2} is your limiting reactant. Assuming a 100% yield, how much AgCl would you expect to produce, in grams? (AgCl has a molecular weight of ).

CaCl_{2} and AgNO_{3} react according to the following equation:

**Problem 2**

You burn an unknown amount of hexane (C_{6}H_{14}) and produce of gas. How much hexane did you burn, in grams? (Hexane has a mass of ).

Hexane combusts according to the following reaction:

## Stoichiometry Practice Problem Solutions

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