Chemistry, Ch. 12
Stoichiometry Worksheets Name_______________
Worksheet # 1 . Theoretical Yield
1. If 2.00 moles of N
2
react in the following equation, how many moles of NH
3
will be produced?
N
2
+ H
2

NH
3
2. If 4.5 moles of H
2
are used in the above equation, how many moles of NH
3
will be produced?
3. If 4.5 moles of H
2
are used, how many grams of NH
3
will be produced?
4. In the following equation, if 2.3 moles of H
2
are used, how many grams of H
2
O will be produced?
H
2
+ O
2

H
2
O
Worksheet # 2 . Theoretical Yield
1. If 35.0 g of N
2
react in the following equation, how many grams of NH
3
will be produced?
N
2
+ H
2

NH
3
2. In the reaction above, if 15.2 g of H
2
are used, how many grams of NH
3
will be produced?
3. If 847.0 g of H
2
are used in the equation below, how many grams of H
2
O will be produced?
H
2
+ O
2

H
2
O
Worksheet # 3 . Theoretical Yield
1. The following reaction takes place: Na + H
2
O

NaOH + H
2
. a) Calculate the number of moles of hydrogen that will be produced if 11.5 g of sodium are used. b) Calculate the number of grams of hydrogen that will be produced in this same reaction.
2. How many grams of iron will be needed to react completely with an excess of oxygen to form
40.0 g of iron (III) oxide? Note: You must write your own equation for this one!!!
3. Aluminum sulfate and calcium hydroxide react to form aluminum hydroxide and calcium sulfate. How many grams of calcium sulfate will be produced if 4.0 moles of aluminum hydroxide are produced?
4. How many grams of magnesium will react with an excess of HNO
3
to produce 1.0 g of hydrogen in a single replacement reaction?

Worksheet # 4 . Limiting Reagents
1. If 28.0 g of nitrogen gas and 4.0 g hydrogen gas are used to make ammonia, what is the limiting reagent?
2. If 8.0 g of hydrogen gas and 8.0 g oxygen gas are used to make water, what is the limiting reagent?
3. If 3.0 g of hydrogen gas and 32.0 g of oxygen gas are used to make water, what is the limiting reagent?
Worksheet # 5 . Limiting Reagents
1. If 42.0 g of sodium and 38.0 g of chlorine are used to produce sodium chloride, what is the limiting reagent?
2. If 80.0 g of magnesium and 80.0 g of water are missed to yield magnesium hydroxide and hydrogen, what is the limiting reagent?
3. If 20.0 g of magnesium and 40.0 g of oxygen are mixed to yield magnesium oxide, what is the limiting reagent?
4. If 15.0 g of aluminum and 30.0 g of copper (II) nitrate are mixed to produce aluminum nitrate and copper, what is the limiting reagent?
Worksheet # 6 . Theoretical Yield
1. If 42.0 g of sodium and 38.0 g of chlorine are used to produce sodium chloride, what is the limiting reagent and who much sodium chloride is produced?
2. If 80.0 g of magnesium and 80.0 g of water are mixed to yield magnesium hydroxide and hydrogen, what is the limiting reagent? How much magnesium hydroxide can be produced?
3. If 20.0 g of magnesium and 40.0 g of oxygen are mixed to yield magnesium oxide, what is the limiting reagent? How much magnesium oxide is produced?
4. If 15.0 g of aluminum and 30.0 g of copper (II) nitrate are mixed to produce aluminum nitrate and copper, how much aluminum nitrate can be produced?
Worksheet # 7 . Percent Yield
1. If 42.0 g of sodium and 38.0 g of chlorine are used to produce sodium chloride and 60.0 g of sodium chloride are actually obtained, what is the percent yield?
2. If 80.0 g of magnesium and 80.0 g of water are mixed to yield magnesium oxide and hydrogen, what is the percent yield if 120.0 g of magnesium hydroxide are obtained?
3. If 20.0 g of magnesium and 40.0 g of oxygen are mixed to yield magnesium oxide and 30.0 g of magnesium oxide are obtained, what is the percent yield?
4. If 15.0 g of aluminum and 30.0 g of copper (II) nitrate are mixed to produce aluminum nitrate and copper, what is the percent yield if 20.0 g of aluminum nitrate are obtained?

Worksheet # 8 . Stoichiometry, Cumulative Problems
1. If 40.0 g of hydrogen phosphate react with 60.0 g of magnesium carbonate, calculate the number of moles of magnesium phosphate produced.
2. If 20.0 g of sodium hydroxide reacts with 30.0 g of sulfuric acid to produce sodium sulfate, which reactant is limiting?
3. If 20.0 g of potassium hydroxide react with 15.0 g of ammonium sulfate, calculate the number of grams of ammonia produced if water is another product?
4. Calculate the mass of silver nitrate required to react with CaCl
2
to produce 64.5 g of silver chloride.
5. Ammonium nitrate, a fertilizer, can be produced by the following reaction:
HNO
3
+ NH
2

NH
4
NO
3
If 189 grams of nitric acid and 104 g of ammonia are used, a) Which reactant is in excess? b) What is the maximum mass of ammonium nitrate obtainable? c) How many grams of excess reactant remains unreacted?
Worksheet # 9 . Stoichiometry, Cumulative Review
1. How much aluminum metal is needed to replace all of the iron from 27.8 g of iron (III) oxide?
2. What weight of iron metal will be required to produce 20.8 g of iron (III) oxide in the reaction with pure oxygen?
3. What weight of aluminum bromide an be produced by the reaction of sufficient aluminum sulfate with 8.75 g of ammonium bromide?
4. What weights of water and diphosphorus pentoxide will be needed in order to produce 95.5 g of phosphoric acid?
5. If 50.0 g of oxygen are available for the combustion of 25.0 g of carbon, is this an adequate amount of oxygen? If so, by how much is the oxygen in excess? If not, by how much is the carbon in excess?
6. How many grams of carbon dioxide can be obtained from the reaction of 100.0 g of sulfuric acid with 100.0 g of calcium carbonate? If 40.0 g are actually obtained, what is the percent yield?
7. In testing for the efficacy of an antacid compound, 5.0 g of hydrochloric acid is mixed with 24.0 g of magnesium hydroxide. Is this enough base to react with all the acid?
Answers to WS # 9.
1. 9.39 g 2. 14.5 g 3. 7.94 g 4. 69.2 g P O; 26.3 g H O
5. C xs by 0.52 moles 6. 44.01 g; 90.89% 7. yes