Predict the products of the reactions below. Then, write the balanced equation and classify the reaction. If “no
reaction” occurs, write N.R. beside the question (DON’T DO ANY MATH IF THERE IS NO REACTION!!).
Use your activity series, predicting products helper sheet and the solubility rules. Do the stoichiometry on the
problems that have the math after you have a balanced equation.
1. Chromium (III) bromide + chloride 
TYPE _________________
When 3.55 g of chromium (III) bromide with 1.35 g chlorine, is there a reaction? If so, who is the
limiting reactant? How many grams of liquid bromine are made? How much excess is there of the
excess reactant?
2. Aluminum + iron (III) oxide 
TYPE __________________
When aluminum reacts with 10.51 g of iron (III) oxide, 6.92 g of iron is made. What is the percent
yield?
3. Potassium permanganate + silver phosphate 
TYPE____________________
If 6.72 g potassium permanganate reacts with silver phosphate, how many grams of silver phosphate are
needed to react with the potassium permanganate? (assume this reaction occurs)
4. Cobalt (III) carbonate 
TYPE____________________
If I have 4.55 moles of cobalt(III) carbonate, and I heat up this compound, how many moles of each
product are made?
5. Copper + hydrochloric acid 
TYPE ____________________
If I react 5.00 g of copper with 11.2 g of hydrochloric acid, how many grams of each product are made?
6. Sulfurous acid + lithium hydroxide 
TYPE ____________________
If I react 4.00 moles of sulfurous acid with 3.00 moles of lithium hydroxide, how many grams of water
are made?
7. Aluminum + oxygen →
TYPE____________________
If I start with 6.75 g of aluminum and 4.56 g of oxygen, I actually recover 9.8 grams of product. What
is the percent yield?
8. Barium acetate + Lead (II) nitrite→
TYPE_______________________
I have 12.6 g of barium acetate and 32.5 moles of lead (II) nitrite, how many grams of lead (II) acetate
are made?
9. Tungsten (IV) chlorate →
TYPE _____________________
I heat up 8.75 moles of tungsten (IV) chlorate, how many liters of oxygen are made? (density of oxygen
= 1.429 g/L)
10. calcium oxide + water →
TYPE _____________________
If I have 25.4 g of calcium oxide and I mix it with water, how many grams of product will be made?
11. nonane (C9H20) + oxygen gas →
TYPE ___________________
If I start out with 235.0 mL of oxygen gas, how many liters of carbon dioxide will be made? (density of
oxygen = 1.429 g/L and density of carbon dioxide = 1.997 g/L)
12. ammonium bicarbonate (aq) + cadmium sulfite (s) →
TYPE________________
If I mix 9.34 g of ammonium bicarbonate and 8.12 g of cadmium sulfite, how much cadmium
bicarbonate is made? How much excess is left over of the excess reactant?
13. Hexane + oxygen 
TYPE___________________
The empirical formula for hexane is C3H7. The molecular mass of hexane is 86 g/mol. What is the
molecular formula of hexane? Use the molecular formula of hexane in the equation.
If I have 11.2 grams of hexane, how many grams of water are supposed to be made? In lab, 12.8 grams
of water are made, what is the percent yield?
14. Copper (I) chromate + lithium acetate  (this reaction occurs)
TYPE _______________
If I have 3.11 moles of copper (I) chromate and 2.89 moles of lithium acetate, which one is the limiting
reactant?
15. Mercury (II) oxide 
TYPE ________________________
If I start with 9.24 grams of mercury (II) oxide, how many grams of oxygen are made?
16. carbonic acid + barium hydroxide 
TYPE ______________________
If I mix 2.00 grams of carbonic acid and 4.00 grams of barium hydroxide, which one is the limiting
reactant? What is the theoretical yield of water? How much excess do I have of my excess reactant?