Honors Chemistry
Stoichiometry Review Guide
Chapter 11
Name ______________________
Period ___
Please show all your work and circle your final answers!!
1. In the following chemical reaction, how many moles of oxygen are needed to produce 10 moles of water?
H2 + O2 
H2O
2. How many grams of water can be produced in the following reaction with 10 grams of oxygen?
H2 + O2 
H2O
3. What do the coefficients in a chemical equation represent?
4. The smaller numbers used to write a chemical formula are called ___________ (like the two in MgCl2)
For Questions 5 & 6 below, use the following:
Ammonium nitrate, NH4NO3, is an important fertilizer and is also used in the manufacture of explosives and fireworks.
It is produced by treating nitric acid HNO3, with ammonia gas, NH3. The equation for this reaction is:
HNO3 + NH3  NH4NO3
5. If 6 moles of ammonia gas are used with 4 moles of nitric acid for the reaction, what is the limiting
reactant?
6. How many moles of ammonium nitrate would you make from the reactants in the problem above?
7. Define the following terms:
a. reactant
b. product
c. limiting reactant
d. excess reactant
g. law of conservation of mass
h. stoichiometry
i. mole
j. molar mass
8. The following equation shows the formation of aluminum oxide:
Al + O2  Al2O3
How many grams of aluminum are needed to produce 250 grams of aluminum oxide?
9. In the reaction between calcium hydride and water, the theoretical yield of hydrogen gas from 75.0 grams
of calcium hydride is 7.18 grams. In running this reaction, the actual amount of hydrogen produced was
6.94 grams. What was the percent yield of this reaction?
Balance the equation:
C3H8 +

O2
CO2
+
H2 O
10.____________ In the above reaction, how many grams of carbon dioxide could be produced with 300
grams of propane (tricarbon octahydride) and 800 grams of oxygen?
11. ____________ How many more grams of the limiting reactant would have to be added to finish the
reaction?
Balance the equation:
P4O10 + H2O

H3PO4
12. ____________In the above reaction what is the mole ratio between tetraphosphorus decoxide and water?
13. ____________How many moles of tetraphosphorus decoxide would be required to produce 20 moles of
phosphoric acid?
14. ____________How many grams of water would be required to fully react with 8 moles of
tetraphosphorus decoxide?
15. ____________How many grams of phosphoric acid could be produced with 500 grams of
tetraphosphorus decoxide?
Balance the equation:
N2 +
H2

NH3
16. ____________ The actual yield in the above reaction was 97 grams of ammonia, using 100 grams of
nitrogen and 25 grams of hydrogen, what is the % yield?