1. stoichiometry
Chapter 10

2. Stoichiometry Fe + O2 – Fe2O3 Balanced: 4 Fe + 3 O2  2 Fe2O3
This means that 4 atoms of Iron and 3 molecules of O2 combine to make 2 molecules of Fe2O3

4. Mole Ratio
K + Br2  KBr
2KClO3  2KCl + 3O2

5. Mole Ratios
Determine all possible mole ratios for the following balanced chemical equations.
4Al + 3O2  2Al2O3
3Fe + 4H2O  Fe2O4 + 4H2
2HgO +  2Hg + O2

6. Stoichiometric calculations

7. Using Stoichiometry K + H2O  KOH + H2
How many moles of Hydrogen will be produced when 3 moles of K react with excess water?
C3H8 + 5O2  3CO2 + 4H2O
How many molecules of CO2 are produced when 10.0 moles of C3H8 is burned with an excess amount of O2?

8. Mass Calculations Na + H2O  NaOH + H2
How many grams of NaOH can be produced from the reaction of grams of Na?
How many grams of H2 can be produced from the reaction of 24 g of H2O?

9. Why do reactions stop?

10. Limiting and excess reactants

11. When the limiting reactant runs out the reaction will stop

12. Calculations S8 + 4Cl2  4S2Cl2
If g of S8 reacts with g of Cl2 what is the mass of S2Cl2 produced?

13. b.) How many grams of the excess reactant is left over?
16Ag + S8  8Ag2S
a.) If 4.00 g of Ag and 4.00 g of S8 react, which is the limiting reactant?
b.) How many grams of the excess reactant is left over?
c.) How many grams of Ag2S will be produced?
Ag, 3.4 g S8 left, 4.56 g Ag2S

14. b.) How many grams of the excess reactant will be left over?
2Al + 3I2  2AlI3
a.) If 54.0 g of Al reacts with 508 g of I2, which is the limiting reactant?
b.) How many grams of the excess reactant will be left over?
c.) How many grams of product will be produced?
I2, g Al left, g of AlI3 produce.