Problem Set One provides a series of stoichiometry problems involving balancing chemical equations and calculating amounts of reactants and products using mole ratios. The key reactions covered are: 1) N2H4 + N2O4 → N2 + H2O 2) NO + O2 → NO2 3) NH3 + O2 → N2 + H2O 4) AlF3 + O2 → Al2O3 + F2 5) C3H8 + O2 → CO2 + H2O 6) O2 + Fe → Fe2O3 Problem Set Two involves calculating moles of glucose produced from moles of carbon dioxide reacted in photos

1. Problem Set One:
N2H4 + N2O4N2 + H2O
BE SURE TO BALANCE THE EQUATION FIRST!!
? moles N2O4 = 2.72 moles N2H4

2. Worksheet: Mole/Mole
Answer each of the following questions using the equation provided
. BE SURE TO BALANCE EACH EQUATION BEFORE SOLVING ANY PROBLEMS.
SHOW ALL WORK.
1.___NO + ___O2 ___NO2
a. 2 moles of NO will react with______mole(s) of O2 to produce______ mole(s) of
NO2.
b. How many moles of NO must react to form 4.67 moles of NO2?
2.___NH3 + ___O2 ___N2 + ___H2O
a. 20 moles of NH3 are needed to produce______moles of H2O.
b.How many moles of N2 will be produced if 3.5 moles of O2 react?
3.___AlF3 + ___O2 ___Al2O3 + ___F2
a. 20 moles of AlF3 will produce______moles of F2.
b. ______ moles of AlF3 will react with 0.6 moles of O2.
4.___C3H8 + ___O2 ___CO2 + ___H2O
a. How many moles of oxygen react with 11 moles of C3H8?
b.How many moles of CO2 are produced if 3.5 moles of water are produced?
5.___O2 + ___Fe ___Fe2O3
a. Fill in the following word equation--______moles of oxygen gas react with
______ moles of iron to produce _____ moles of iron (III) oxide.
b.______ moles of O2 are required to produce 3.0 moles of iron (III) oxide.

3. Problem Set #2
In photosynthesis, carbon dioxide and water react to form
glucose, C6H12O6 and oxygen gas.
___CO2 + ___H2O ___C6H12O6 + ___O2
BE SURE TO BALANCE THE EQUATION FIRST!!
If 15.6 grams of carbon dioxide react, how many moles of glu-
cose will be produced?
How many grams of carbon dioxide must react to produce 0.25
moles of glucose?

4. Worksheet Mole/Mass Problems:
Answer each of the following questions using the equation provided.
BE SURE TO BALANCE EACH EQUATION BEFORE SOLVING ANY PROBLEMS.
SHOW ALL WORK.
1.In a reaction between the elements aluminum and chlorine, aluminum chloride is
produced.
___Al + ___Cl2 ___AlCl3
a. 2 moles of Al will react with______mole(s) of Cl2 to produce______
mole(s) of AlCl3.
b. How many grams of AlCl3 will be produced if 2.50 moles of Al react?
c. How many moles of Cl2 must react to produce 12.3g of AlCl3?
d. How many grams of aluminum will react with 3.4 moles of chlorine?
e.If 17 grams of aluminum react, how many moles of aluminum chloride will be pro-
duced?
2. The ammonia (NH3) used to make fertilizers for lawns and gardens is made by
reacting nitrogen and hydrogen according to the following reaction.
___N2 + ___H2 ___NH3
a. Determine the mass in grams of NH3 formed from 1.34moles of nitrogen.
b. What is the mass in grams of hydrogen required to react with 1.34 moles of ni-
trogen?
c. How many moles of nitrogen are required to produce 11.7 moles of NH3?
d. How many moles of nitrogen are required to produce 11.7 grams of NH3?
e. How many grams of hydrogen are required to form 3.5 moles of NH3?

5. Problem Set #3
The first step in the industrial manufacture of nitric acid in-
volves the catalytic oxidation of ammonia according to the fol-
lowing BALANCED equation.
4NH3 (g) + 5O2 (g)4NO(g) + 6H2O(g)
How many moles of NO are formed if 824 g of NH3 react?
How many grams of water are formed if 2.5 moles of ammonia
are oxidized?
How many moles of oxygen are needed to react with 4.6 moles
of ammonia?
Mercury (II) oxide decomposes into mercury and oxygen gas
according to the following UNBALANCED equation.
HgOHg+ O2
How many moles of mercury (II) oxide are needed to produce
125 g of oxygen?
How many moles of mercury are produced if 24.5 moles of
mercury (II) oxide decompose?

6. How many grams of oxygen will be produced if 2.3 moles of
mercury are produced?
Worksheet: Mixed Problems:Mole/Mole and Mole/Mass
Answer each of the following questions using the equation provided.
BE SURE TO BALANCE EACH EQUATION BEFORE SOLVING ANY PROBLEMS. SHOW
ALL WORK.
1.___Cu + ___O2 ___CuO
a. If 101 grams of copper is used, how many moles of copper (II) oxide will be
formed?
b. If 5.25 moles of copper are used, how many moles of oxygen must also be used?
c.If 78.2 grams of oxygen react with copper, how many moles of copper (II) oxide will be
produced?
2.___C4H10 + ___O2 ___CO2 + ___H2O
a. How many moles of butane, C4H10, are needed to react with 5.5 moles of oxygen?
b.How many grams of carbon dioxide will be produced if 3.5 moles of O2 react?
3.___Mg + ___HCl ___MgCl2 + ___H2
a. What mass of HCl is consumed by the reaction of 2.50 moles of magnesium?
b. What mass of MgCl2 is produced if 3.67 moles of HCl react?
c.How many moles of hydrogen gas are produced when 3.0 moles of magnesium react?
4.___NH3 + ___O2 ___N2 + ___H2O
a. How many moles of oxygen react with 0.23 moles of NH3?
b. How many grams of water will be produced if 0.55 moles of oxygen react?
c. How many moles of nitrogen gas will be produced if 12.6 grams of ammonia react?

7. Challenge Problem: Stoichiometry
Use what you have learned about stoichiometry so far to try
to solve the following problem.
When nitrogen and hydrogen react, they form ammonia gas,
which has the formula NH3. If 56.0 g of nitrogen are used up
in the reaction, how many grams of ammonia will be produced?