Chemistry
Chapter 9 Practice Test: Stoichiometry
Name ________________________
Free Response
Use the following equation to answer problems 1 - 4 at STP. (Show All Work)
2Al(s)
+
6HCl(aq)

2AlCl3(aq)
+
3H2(g)
1.
How many moles of aluminum chloride (AlCl3) would be produced from 0.12 moles of Hydrochloric acid (HCl)?
2.
If you wanted to completely react 5.0 moles of Aluminum, how many moles of hydrochloric acid (HCl) would
be needed?
3.
How many grams of hydrochloric acid (HCl) would be needed to completely react 35.8 g of Aluminum foil?
4.
How many grams of aluminum would be needed to produce 67.2 dm 3 of hydrogen gas?
Use the following equation to answer problems 5 and 6 at STP.
2CO(g)
+
O2(g)

2CO2(g)
5.
How many molecules of carbon dioxide (CO2) would be produced by completely reacting 8.00 grams of
oxygen gas (O2) with excess Carbon Monoxide (CO)?
6.
What volume in L of oxygen gas (O2) would react with 6.0 L of carbon monoxide gas (CO) ?
Use the following equation to solve problem 7 at STP.
N2(g)
7.
+
3 H2(g)

2 NH3(g)
What volume (in Liters) of ammonia gas (NH3) would be produced from 14.0 grams of nitrogen (N 2) at STP?
Limiting Reagent and % Yield Problem
CH4(g)
8.
+
2O2(g)

CO2(g)
+
2H2O(l)
If 6.0 moles of methane is mixed with 8.0 moles of O2, and the mixture is ignited, determine:
____________________ a. The limiting reactant.
____________________ b. The reactant in excess.
____________________ c. The moles of carbon dioxide (CO2) produced. (Show Work)
____________________ d. How many grams of excess reactant left over. (Show Work)
____________________ e. How many grams of water will theoretically be produced from this reaction?
(Show Work)
____________________ f. Determine the % yield if the actual amount of water produced during this reaction is
130.0 g. (Show Work)