1. Stoichiometry
How does stoichiometry relate to a correctly balanced chemical equation?

2. What information can the coefficients of a correctly balanced chemical equations provide?
Example: 2 H2(g) + O2(g)  2 H2O(g)
The number of atoms / molecules that react with each other
The number of moles of atoms / molecules that react
The relative volume of gases that react (if reactants and products are gases)

3. Stoichiometry
Use the coefficients of a balanced equation to determine the mole ratio among all participants in the reaction.
Example: 2 H2 + O2  2 H2O
There are 2 moles of H2 consumed and 1 mole of 02 consumed for every 2 moles of H2O produced
If 4 moles of oxygen react with excess hydrogen, how many moles of water will be produced?
1 mole O2 = 2 mole H2O
Set up a proportion or use dimensional analysis

4. Think About Units Carefully!
The coefficients indicate the mole ratios and do not indicate mass ratios
If grams are involved, you must convert between grams and moles
Each 1 mol = _____ g from the PT
Example based on: 2 KClO3  2 KCl + 3 O2
How many moles of KClO3 are required to produce 64 grams of O2?
Step 1: Convert given mass of O2 to moles O2
Step 2: Use Coefficients to compare moles O2 to moles KClO3

5. Think About Units Carefully!
Example based on: 2 KClO3  2 KCl + 3 O2
How many grams of O2 are produced if 0.50 mol of KClO3 react completely?
Step 1: Use Coefficients to compare moles KClO3 to moles O2
Step 2: Convert moles of O2 to grams of O2

6. Challenge Question: Based on: 2 KClO3  2 KCl + 3 O2
How many grams of O2 will be produced if 2.38g of KClO3 completely react?
Step 1: Convert given mass of KClO3 to moles KClO3
Step 2: Use Coefficients to compare moles KClO3 to moles O2
Step 3: Convert moles O2 to grams of O2