Name: _________________________
Name: _________________________
Chapter 12 Study Guide
Chapter 12 Study Guide
**Do your work on another sheet of paper**
**Do your work on another sheet of paper**
1. Given the following equation:
2 KClO3  2 KCl + 3 O2
How many moles of oxygen can be produced by
letting 12.00 moles of potassium chlorate react?
1. Given the following equation:
2 KClO3  2 KCl + 3 O2
How many moles of oxygen can be produced by
letting 12.00 moles of potassium chlorate react?
2. Given the following equation:
2 K + Cl2  2 KCl
How many grams of potassium chloride is
produced from 2.50 grams of potassium and
excess chlorine.
2. Given the following equation:
2 K + Cl2  2 KCl
How many grams of potassium chloride is
produced from 2.50 grams of potassium and
excess chlorine.
3. Given the following equation:
Na2O + H2O  2 NaOH
How many grams of sodium oxide are required to
produce 1.60 x 1021 molecules of sodium
hydroxide?
3. Given the following equation:
Na2O + H2O  2 NaOH
How many grams of sodium oxide are required to
produce 1.60 x 1021 molecules of sodium
hydroxide?
4. Given the following equation:
2 NaClO3  2 NaCl + 3 O2
How many grams of sodium chloride are
produced when 80.0 liters of oxygen are
produced?
4. Given the following equation:
2 NaClO3  2 NaCl + 3 O2
How many grams of sodium chloride are
produced when 80.0 liters of oxygen are
produced?
5. Iron and carbon monoxide are produced in a
blast furnace by the reaction of iron(III) oxide and
carbon. If 25.0 grams of pure Fe2O3 is used, how
many molecules of iron can be produced?
5. Iron and carbon monoxide are produced in a
blast furnace by the reaction of iron(III) oxide and
carbon. If 25.0 grams of pure Fe2O3 is used, how
many molecules of iron can be produced?
6. Glucose (C6H12O6) goes through combustion. If
120 grams of glucose are used, then how many
liters of water are produced?
6. Glucose (C6H12O6) goes through combustion. If
120 grams of glucose are used, then how many
liters of water are produced?
7. Given the following equation:
Cu + 2 AgNO3  Cu(NO3)2 + 2 Ag
If 72 grams of copper and 187 grams of silver (I)
nitrate react, then how many grams of copper (II)
nitrate will be produced? Identify the limiting and
excess reagents.
7. Given the following equation:
Cu + 2 AgNO3  Cu(NO3)2 + 2 Ag
If 72 grams of copper and 187 grams of silver (I)
nitrate react, then how many grams of copper (II)
nitrate will be produced? Identify the limiting and
excess reagents.
8. Given the following equation:
8 Fe + S8  8 FeS
If 150 grams of iron react with 150 grams of sulfur,
then how many grams of iron (II) sulfide are
produced?
8. Given the following equation:
8 Fe + S8  8 FeS
If 150 grams of iron react with 150 grams of sulfur,
then how many grams of iron (II) sulfide are
produced?
9. Given the following equation:
Na2CO3 + 2 HNO3  2 NaNO3 + H2O + CO2
If 30 grams of sodium carbonate react to form
45.5 grams of sodium nitrate, then what is the
percent yield?
9. Given the following equation:
Na2CO3 + 2 HNO3  2 NaNO3 + H2O + CO2
If 30 grams of sodium carbonate react to form
45.5 grams of sodium nitrate, then what is the
percent yield?
10. Given the following equation:
2Fe + 3O2  Fe2O3
If 100 grams of iron react with 90 grams of oxygen
and 130 grams of iron(III)oxide is produced, then
what is the percent yield? Identify the limiting and
excess reagents.
10. Given the following equation:
2Fe + 3O2  Fe2O3
If 100 grams of iron react with 90 grams of oxygen
and 130 grams of iron(III)oxide is produced, then
what is the percent yield? Identify the limiting and
excess reagents.