Honors Chemistry
Name: ____________________________________ Date: __________________ Mods: __________
Chapter 3 Test Review
1) List the 5 types of chemical reactions:
2) Balance the following equations and identify what type of reactions they are.
a. ______ Fe(NO3)3 (aq) + ______ Na2S (aq)  ______ Fe2S3 (s) + _______ NaNO3 (aq)
Type of Reaction: ______________________________________
b. _____ Mg (s) + _____ HCl (aq)  ______ MgCl2 (aq) + ______ H2 (g)
Type of Reaction: ______________________________________
c. ______ Li (s) + ______ N2 (g)  ______ Li3N (s)
Type of Reaction: ______________________________________
d. ______ C6H14 (l) + ______ O2 (g)  ______ CO2 (g) + ______ H2O (g)
Type of Reaction: ______________________________________
e. ______ AgBr (aq)  ______ Ag (s) + ______ Br2 (g)
Type of Reaction: ______________________________________
3) Write and balance the following word equations.
a. Zinc metal reacts with oxygen gas.
b. Liquid pentanol, C5H12O, undergoes combustion.
c. Solid calcium nitride decomposes.
Directions: Answer the following questions. Show all your work clearly and neatly. Be sure to label
proper units and identify the substances in your answers.
4) What is the percent by mass of chromium in sodium dichromate?
5) What is the percent by mass of titanium in titanium (IV) carbonate?
6) How many moles of carbon dioxide are there in 52.06 g of CO2?
7) How many molecules of methane are in 0.123 mols of methane (CH4)?
8) How many atoms of silver are there in 12.74 g of silver sulfate?
9) A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The molar mass of the
compound is 60.05 g/mol. What is the molecular formula of this compound?
10) A lab experiment is performed in which a hydrate of magnesium chloride is heated in a
crucible until all the water of hydration is removed from the sample. Given the laboratory data
below, determine the empirical formula and name of the hydrate sample used.
Experimental Data:
mass of crucible = 22.130 grams
mass of crucible + hydrate = 25.290 grams
mass of crucible and contents after heating = 23.491 grams
11) Vanillin, the dominant flavoring in vanilla, contains C, H, and O. When 1.05 grams of this
substance is completely combusted, 2.43 g of CO2 and 0.50 g H2O are produced. What is the
empirical formula of vanillin?
12) The reaction of ammonia in the presence of excess oxygen yields NO2 and H2O:
______NH3 (g) + ______O2 (g)  ______NO2 (g) + ______H2O (g)
How many moles of oxygen gas would react with 1.88 moles of ammonia?
13) Gaseous dinitrogen pentoxide reacts with water to form aqueous nitric acid.
a. If 86.3 g of water is used for the reaction, how many grams of nitric acid will be
produced?
b. If 13 moles of dinitrogen pentoxide is used, how many grams of water will be needed
for the reaction?
14) Aqueous solutions of lead (IV) nitrate and lithium sulfate react with each other in a double
replacement reaction to form solid lead (IV) sulfate and aqueous lithium nitrate.
a. What mass, in grams, of the solid product will be formed when 4.22 g of lead (IV)
nitrate react with 5.73 g of lithium sulfate?
b. Which substance is the limiting reactant? _______________________________
c. Which substance is the excess reactant? _______________________________
d. How much of the excess reactant will be left over when the reaction is complete?
e. In lab trial #1 of this double replacement reaction, 3.46 g of the lead (IV) sulfate was
produced. What is the percent yield of this product?
f.
In lab trial #2, a dismal 62.6% yield of lead (IV) sulfate was recovered due to the
breaking of a beaker. What mass of lead (IV) sulfate must have actually been produced
by this trial?