Name:_______________________ Date:___________________ Period:_______________
HONORS CHEMISTRY- Stoichiometry Problem Set
For each problem below, write a balanced chemical equation for the described reaction (if it is not given). Show all
work on another piece of paper for credit (no work = no credit). Write your final answer with proper units in the
box provided (pay attention to sig figs!!). Staple all work.
1. One of the main components of pearls is calcium carbonate, CaCO3. If pearls are placed in acidic
solution they dissolve according to the equation:
CaCO3 + 2HCl  CaCl2 + H2O + CO2
How many moles of CaCO3 can be dissolved in 0.0250 moles of HCl?
Answer:
2. Aluminum reacts with oxygen to produce aluminum oxide. How many moles of aluminum oxide would
be formed if you reacted 9.0 moles of oxygen and an excess of aluminum?
Answer:
3. Carbon dioxide is released into the atmosphere through the combustion of octane (C8H18) in gasoline.
Write the balanced equation for the combustion of octane and calculate the mass in grams of octane
needed to release 5.00 moles of carbon dioxide.
Answer:
4. Lithium hydroxide and zinc sulfate react to form lithium sulfate and zinc hydroxide. If 1.32 moles of
lithium hydroxide react with an excess of zinc sulfate, how many grams of zinc hydroxide should be
formed? What type of reaction is this?
Answer:
5. Sodium hydroxide is used to remove carbon dioxide from the cabin of spacecrafts according to the
following balanced reaction: 2NaOH + CO2  Na2CO3 + H2O. If the average human body discharges
925.0g of carbon dioxide per day, how many moles of NaOH are needed each day for each person in the
spacecraft?
Answer:
6. In a fire extinguisher, sulfuric acid reacts with
sodium bicarbonate to produce carbon dioxide, sodium sulfate, and water. How many moles of sodium
bicarbonate would be needed to react with 150.0g of sulfuric acid? H2SO4 + 2NaHCO3  2CO2 +
Na2SO4 + 2H2O
Answer:
7. Aluminum reacts with hydrochloric acid to
produce aluminum chloride and hydrogen gas.
How many grams of hydrochloric acid react with 3.20 moles of aluminum dissolved in excess
hydrochloric acid.
Answer:
8. Sodium oxide reacts with water to produce sodium hydroxide. What mass of sodium oxide must be used
to produce 275 kilograms of sodium hydroxide?
Answer:
9.
When magnesium burns in pure nitrogen gas, magnesium nitride is formed. What mass of magnesium
must be provided in order to produce 1.19 grams of magnesium nitride?
Answer:
10. Rusting of iron occurs in the presence of moisture according to the following equation:
4Fe + 3O2  2Fe2O3
Suppose that 3.19% of a heap of iron scrap with a mass of 1650kg rusts in one year. What mass of
iron (III) oxide will be produced after one year of rusting?
Answer:
11. Aluminum chips are sometimes added to sodium hydroxide based drain cleansers because they react to
generate hydrogen gas, which bubbles and helps loosen material in the drain. The equation follows:
Al + NaOH + H2O  NaAlO2 + H2
a. Balance the equation
b. How many moles of hydrogen gas can be generated from 0.57 mol Al and 0.37 mol NaOH in
excess water?
c. Identify the limiting and excess reactants
Answer:
12. One industrial process for producing nitric acid begins with the following unbalanced reaction:
NH3 + O2  NO + H2O
a. Balance the equation
b. If 2.90 moles of NH3 and 3.75 moles of O2 are available, how many moles of each product are
formed?
c. What mass of NO is formed in the reaction of 869kg of NH3 and 2480kg O2?
Answer: