1. (STOY-KEE-AHM-EH-TREE)
Stoichiometry
(STOY-KEE-AHM-EH-TREE)

2. Chemical Equation Review
2 H2 (g) + O2 (g) H2O (l)
coefficient
Product(s)
Reactants
“Reactants with”
“to produce” or “yield”
State of matter

3. Interpreting Chemical Equations
2 H2(g) +
O2(g) →
2 H2O(g)
2 molecules
1 molecule
2 moles
1 mole
2(2.02 g)
1(32.00 g)
2 (18.02 g)
36.04 g reactants
36.04 g product
2(22.4L)
1(22.4L)
Interpretation

4. Mole Ratio

5. Stoichiometry

6. Example 1
How many grams of water can be produced by burning 325 g of octane (C8H18)?

7. Example 2
What volume of carbon dioxide is produced by the complete combustion of L of pentane?

8. Limiting Reactant
Before the rxn has started
After the rxn is complete

9. Steps Use stoichiometry to convert reactant(s) into the product
Identify limiting reactant (LR), excess reactant (ER), and max amount of product
To calculate how much in excess, subtract the max amount of product and use stoichiometry to convert back to grams of excess reactant

10. Example 3
How many grams of silver bromide can be formed when solutions containing 50.0 g of magnesium bromide and g of silver nitrate are mixed together? What is the limiting reactant? What is in excess? How much is in excess?

11. Example 4
How many grams of hydrogen chloride can be produced from 1.00 g of hydrogen and 55.0 g of chlorine? What is the limiting reactant? What is in excess?

12. Example 5
How many grams of barium sulfate will be formed from g of barium nitrate and g of sodium sulfate? What is the limiting reactant? What is in excess?