1. For the following equation, 27.0 g of C2H4 is reacted with 63.0 g of O2. C2H4 (g) + 3O2 (g) → 2CO2 (g) + 2H2O (g) a. Calculate the grams of water produced.
b. Identify the limiting reactant.
c. Identify the excess reactant.
d. How much of the excess reactant is used?
e. How much of the excess reactant is left over?
2. When 80.0 a.
b.
c. d. e.
g of copper reacts with 25.0 g of sulfur to form copper (I) sulfide, Write a balanced equation.
How much copper (I) sulfide is formed?
Identify the limiting reactant.
Identify the excess reactant.
How much of the excess reactant is used?
f. How much of the excess reactant is left over?

3. Hydrogen gas can be produced in the laboratory by the reaction of magnesium metal with hydrochloric acid.
Mg(s) + 2HCl (aq) → MgCl2 (aq) + H2 (g)
a. How many grams of hydrogen can be produced when 4.00 g of HCl is added to 3.00 g of Mg?
b. Identify the limiting reactant.
c. Identify the excess reactant.
d. How much of the excess reactant is used?
e. How much of the excess reactant is left over?
4. Hydrogen and oxygen gases react to form water. When 50.0 g of hydrogen react with 15.0 g of oxygen,
a. Write a balanced equation.
b. How much water is formed?
c. Identify the limiting reactant.
d. Identify the excess reactant.
e. How much of the excess reactant is used?
f. How much of the excess reactant is left over?
5. If 65.3 g of diphosphorus pentoxide reacts with 12.6 g of water to form phosphoric acid, 2P2O5 + 6H2O → 4H3PO4

a. How much phosphoric acid is formed?
b. Identify the limiting reactant.
c. Identify the excess reactant.
d. How much of the excess reactant is used?
e. How much of the excess reactant is left over?