CHAPTER 9 – STOICHIOMETRY
STOICHIOMETRY - 1
Use the following equation to solve the following problems. Show all work and circle your
answers.
Na3PO4 + 3 AgNO3  Ag3PO4 + 3 NaNO3
1.
How many moles of silver nitrate would be required to react with 1.00 mole of sodium
phosphate?
2.
How many moles of sodium nitrate can be produced from 0.30 mole of sodium
phosphate?
3.
What mass of silver phosphate can be produced from 6.00 grams of silver nitrate?
4.
If you have 12.5 g of sodium phosphate, what weight of silver nitrate is needed for
complete reaction?
5.
What mass of silver phosphate can be produced from the reaction of 20.0 g of silver
nitrate? (*** What is the percent yield if 14.5 g of silver phosphate are actually
produced???)
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STOICHIOMETRY - 2
Use the following equation to solve the following problems. Show all work and circle your
answers.
2 KMnO4 + 16 HCl  5 Cl2 + 2 KCl + 2 MnCl2 + 8 H2O
1.
How many moles of HCl are required to react with 35.0 g of KMnO4?
2.
How many Cl2 molecules will be produced using 3.00 moles of KMnO4?
3.
To produce 65.0 g of MnCl2, what weight of HCl will react?
4.
How many moles of water will be produced when 12.0 moles of KMnO4 are consumed?
5.
What weight of chlorine can be produced by reacting 50.0 g HCl with excess KMnO4?
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STOICHIOMETRY - 3
Use the following equation to solve the following problems. Show all work and circle your
answers.
6 KI + 8 HNO3  6 KNO3 + 2 NO + 3 I2 + 4 H2O
1.
If 27 g of KI are reacted, what weight of potassium nitrate will be formed?
2.
What volume of NO gas, measured at STP, will be formed if 32.0 g of HNO3 are
consumed?
3.
When the reaction produces 4.0 moles of NO, how many molecules of I2 will be
produced?
4.
How many moles of water are produced with the reaction of 80.0 g of potassium iodide?
5.
What mass of KI is needed to completely react with 45.0 g of HNO3?
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STOICHIOMETRY - 4
Use the following equation to solve the following problems. Show all work and circle your
answers.
N2(g) + 3 H2(g)  2 NH3(g)
1.
If 2.0 moles of N2 react, how many moles of ammonia will be formed?
2.
When 4.00 moles of N2 react, what volume of ammonia, measured at STP, will be
formed?
3.
If 9.0 L of hydrogen are reacted, what volume of ammonia will be formed? All volumes
are measured at STP.
4.
How many molecules of NH3 will be formed when 22.4 L of N2 at STP react?
5.
What mass of NH3 will be formed by the reaction of 10.0 g of hydrogen?
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BALANCING EQUATIONS, PREDICTING PRODCUTS
AND STOICHIOMETRY PUTTING IT ALL TOGETHER 
1. Potassium chlorate decomposes into potassium chloride and oxygen gas.
Balanced Equation:
2. How many moles of oxygen are produced when 3.0 moles of potassium chlorate decompose
completely?
3. Butane (C4H10) undergoes combustion.
Balanced Equation:
4. How many grams of CO2 are produced when 88 g of O2 are reacted with an excess of butane?
5. Water decomposes into hydrogen gas and oxygen gas by electrolysis.
Balanced Equation:
6. How many grams of hydrogen will be produced when 6.0 moles of oxygen are produced?
7. How many grams of water are required to produce 9.00 grams of hydrogen?
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8. Cobalt(II) chloride reacts with fluorine in a single replacement reaction.
Balanced Equation:
9. How many grams of fluorine are required to produce 290.8 g of cobalt(II) fluoride?
10. Balance the following equation.
____ SrCl2(aq) + _____ H2SO4(aq)
_____HCl(aq) + ____SrSO4(s)
11. What is the mass of strontium chloride that reacts with 300.0 g of sulfuric acid?
12. Solid iron(III) oxide reacts with hydrogen gas to form iron and water.
Balanced Equation:
13. How many grams of iron are produced when 450 grams of iron(III) oxide are reacted?
14. How many grams of water will be produced when 0.0155 moles of hydrogen gas react completely
with iron(III) oxide?
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LIMITING REACTANT PROBLEMS
Directions: Answer the following problems on another piece of paper. Please show all work and
label all units, both while solving the problem and when stating the answers.
1. A) If 20.0 g of magnesium reacts with 45.0 g of hydrochloric acid, how many grams of
magnesium chloride are produced?
B) Which is the limiting reactant?
C) Which is the excess reactant?
D) How much of the excess reactant is used and how much of the excess reactant is left over?
2. A) How many grams of sodium chloride are produced if 10.0 g of NaI react with 15.0 g of
chlorine?
B) Which is the limiting reactant?
C) Which is the excess reactant?
D) How much of the excess reactant is used and how much of the excess reactant is left over?
3. A) How many grams of silver will be formed if 2.8 g of copper replaces silver from 4.00 g
of silver nitrate? (Hint: Use copper(I) nitrate as one of the products)
B) Which is the limiting reactant?
C) Which is the excess reactant?
D) How much of the excess reactant is used and how much of the excess reactant is left over?
4. A) If 35.0 g of ammonium sulfate reacts with 20.0 g of calcium hydroxide to form ammonia
(NH3), calcium sulfate, and water, how many grams of ammonia will be formed?
B) Which is the limiting reactant?
C) Which is the excess reactant?
D) How much of the excess reactant is used and how much of the excess reactant is left over?
5. A) If 38.0 g of sulfuric acid reacts with 30.0 g of sodium chloride, how many grams of
hydrochloric acid are produced?
B) Which is the limiting reactant?
C) Which is the excess reactant?
D) How much of the excess reactant is used and how much of the excess reactant is left over?
6. A) How much silver phosphate is produced if 10.0 g of silver acetate reacts with 10.0 g of
sodium phosphate?
B) Which is the limiting reactant?
C) Which is the excess reactant?
D) How much of the excess reactant is used and how much of the excess reactant is left over?
7. A) What weight of sodium sulfate is produced if 25.0 g of sodium hydroxide reacts with
23.0 g of sulfuric acid?
B) Which is the limiting reactant?
C) Which is the excess reactant?
D) How much of the excess reactant is used and how much of the excess reactant is left over?
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STOICHIOMETRY REVIEW
1. Write the equation for the combustion of butane, C4H10 (lighter fluid):
________________________________________________________________
A) How many moles of oxygen are needed to burn 10.0 mol of butane?
B) When 10.0 g of butane are burned, what volume of oxygen is needed at STP?
2.
Silicon carbide, SiC, is commonly known as carborundum. This hard substance, which is
commonly used commercially as an abrasive, is made by heating SiO2 and C to high
temperatures:
____SiO2(s) + _____C(s)  ____SiC(s) + ____CO(g)
A) How many grams of SiC are formed by complete reaction of 5.00 g of SiO2?
B) How many grams of C are required to react with 4.1 x 1024 molecules of SiO2?
C) How many grams of SiC can form when 2.50 g of SiO2 are reacted?
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