Chemistry Final Review Spring 2011
Unit 1 (Chapter 10) Equations, Single Displacement, Double Replacement,
Types of reactions
1. Balance the following equations.
a. __Al + __HCl  __AlCl3 + __H2
b. __Ba(ClO3)2  __BaCl2 + __O2
c. __Sn(SO4)2 + __K3PO4  __Sn3(PO4)4 + __K2SO4
d. __C5H12 + __O2  __CO2 + __H2O
2. Write the balanced chemical equation for the following word equations.
a. Solid zinc and aqueous hydrogen sulfate react to produce hydrogen gas and aqueous
zinc sulfate.
b. Nickel (II) hydroxide decomposes to produce nickel (II) oxide and water.
c. Aqueous barium chloride and aqueous potassium carbonate react to produce solid
barium carbonate and aqueous potassium chloride.
3. Single Displacement- Predict the products if a reaction occurs (write NR if no reaction)
a. K + ZnCl2 
b. Fe + Na3PO4 
c. Ca + CuBr2 
d. Mg + AgNO3 
4. Double Replacement – Predict the products of each reaction and determine if a precipitate,
water or gas is made.
a. LiI + AgNO3 
b. BaCl2 + K2CO3 
c. HBr + NaOH 
5. Identify the type of equation given.
a. C6H6 + O2  CO2 + H2O
b. Cr(OH)6  Cr2O6 +H2O
c. Cl2 + 2NO  2NOCl
d. F2 + FeI2  FeF2 + I2
e. Ni(OH)2 +2HCl  NiCl2 + 2H2O
Unit 2 (Chapter 11 and 12) Mole, Percent Comp., Empirical/ Molecular
Formula, Stoichiometry, Percent Yield, Limiting Reactant
1. Solve the following mole conversions.
a. Determine the number of atoms in 2.50 mol Zn.
b. Calculate the mass in grams of 42.6 mol Si.
c. How many liters of Kr are in 5.62 grams of Kr?
d. How many molecules are in 0.124 grams Mg?
2. Calculate the following molar masses.
a. HNO3
b. C6H8O6
c. (C3H5)2S
3. Determine the percent composition of Nitrogen in caffeine (C8H10N4O2).
4. Determine the percent composition of both elements in Fe3O4.
5. Empirical Formula
a. Monosodium glutamate (MSG) is sometimes added to food to enhance flavor. Analysis
determined this compound to be 35.5% C, 4.77% H, 8.29% N, 13.6% Na and 37.9% O.
What is the empirical formula for MSG?
6. Molecular Formula
a. Glycerol is a thick, sweet liquid obtained as a byproduct of the manufacturer of soap. Its
percent composition is 39.12% carbon, 8.75% hydrogen and 52.12% oxygen. The molar
mass is 92.11 g/mol. What is the molecular formula?
b. A substance has an empirical formula of PNCl2. What is its molecular formula if the
molar mass is 695 g/mol?
7. Stoichiometry
a. How many grams CH4 are needed to produce 50.0 grams CHCl3?
CH4 + 3Cl2  CHCl3 + 3HCl
b. What mass of CO2 is produced from the combustion of 100 grams of ethanol (C2H5OH)?
C2H5OH + 3O2  2CO2 + 3H2O
b. If you start with 0.250 mol potassium chromate, determine the mass of lead chromate
that can be obtained.
K2CrO4 + Pb(NO3)2  PbCrO4 + 2KNO3
d. When 5.50 mol calcium carbide (CaC2) reacts with water, how many moles of acetylene
(C2H2) will be produced?
CaC2 + 2H2O  Ca(OH)2 + C2H2
e. How many molecules are needed to produce 45.0 grams of methanol (CH3OH)?
CO + 2H2  CH3OH