1. 4th Partial: Homework 1
I. Read the following chapters: Stoichiometry and Gases (on the
gases chapter focus on the section that pertains to the Ideal Gas
Law, make sure you look through the rest of the chapter as well).
Take notes to compliment the notes you took in class.
II. Solve the following problems. Show all of your work. Be neat
and orderly otherwise it will cost you deductions. If I can’t find
your answer OR I don’t understand your work the WHOLE
question will be wrong. Make sure you show units (2 points off
for every unit that is not shown). HOMEWORK IS DUE
nd
TUESDAYNOVEMBER 22 , 2011.
1. The reaction between solid sodium and iron (III) oxide is one in
a series of reactions that inflates an automobile airbag: Na (s) +
Fe2O3 (s)  Na2O (s) + Fe (s). If 100 g of Na and 100 g of
Fe2O3are used in this reaction, determinethe following.
a. Limiting reactant
b. Excess reactant
c. Mass of solid iron produced
d. Mass of excess reactant that remains after the reaction is
complete. (HINT: after determining the limiting and
excess reactants. Do a mass to mass conversion of the
amount of product produced to the excess reactant… this
will be the amount of excess reactant you used. Then
subtract that amount from your original reactant).
2. When copper wire is placed into a silver (I) nitrate solution,
silver crystals and copper (II) nitrate solution form.
a. Write the balanced chemical equation for the reaction.
b. If a 20.0-g sample of copper is used, determine the
theoretical yield of silver.
c. If 60.0-g of silver is recovered from the reaction,
determine the percent yield of the reaction.
d. How many particles of silver are present in the product?

2. 4th Partial: Homework 1
3. To produce 15.4 L of nitrogen dioxide at 310 K and 2.0 atm,
how much many liters of nitrogen gas and oxygen gas are
required? (HINT: remember Avogadro’s principle from the
problems in class).
4. The gas acetylene, often used for welding, burns according to
the following equation.
2C2H2 (g) + 5O2 (g)  2H2O + 4CO2 (g)
If you have a 10.0-L tank of acetylene at 25oC and 1.00 atm
pressure, how many moles of CO2 will be produce if you burn
ALL the acetylene in the tank? How many particles of CO2 will
be present?
5. When iron rusts, it undergoes a reaction with oxygen to form
iron (III) oxide.
4Fe (s) + 3O2 (g)  2Fe2O3 (s)
Calculate the volume of oxygen gas at STP that is required to
completely react with 52.0 g of iron. What is the volume of 1
moles of gas at STP? (HINT: look at the problems in class for
specifications on STP).
EXTRA CREDIT CHALLENGE (will only be graded if the rest of the
homework is done):
An excess of acetic acid is added to 28 g of sodium bicarbonate at
25oC and 1 atm pressure. During the reaction, the gas cools to 20oC.
What volume of carbon dioxide will be produced? The balanced
equation for the reaction is shown below.
NaHCO3 (aq) + CH3COOH (aq)  NaCH3COO (aq) + CO2 + H2O