*For each question, balance the equation first, determine and circle the limiting reagent before answering the questions!
1.
A solution with 5.10 g of silver nitrate reacts with another solution that contains
0.06 mol of potassium chloride. a) Determine the mass of silver chloride formed after this reaction. b) Determine the mass of the excess reagent that is left over unreacted.
AgNO
3
+ KCl  KNO
3
+ AgCl
2.
4.0 mol of ammonia reacts with 7.0 mol of oxygen gas to produce nitrogen monoxide gas and water. a) What mass of nitrogen monoxide is produced? b) What mass of the excess reagent remains unchanged at the end of the reaction?
NH
3
+ O
2
 NO + H
2
O
3.
The following reaction is completed using 63.45 g of iodine and 53.96 g of aluminum. a) Determine the mass of product made. b) Determine the number of molecules of aluminum iodide produced.
Al + I
2
 AlI
3
4.
Nitrogen gas and oxygen gas react to produce nitrogen dioxide gas. a) Determine the mass of nitrogen dioxide produced if 0.20 mol of each reactant are used. b) Determine the amount of nitrogen dioxide produced when 2.0 mol of nitrogen gas are reacted with 4.5 mol of oxygen gas.
5.
Hydrogen sulfate is produced from 1.5 mol of sulfur dioxide gas, 32.0 g of oxygen and
2.0 mol of water. a) What mass of hydrogen sulfate is produced?
SO
2
+ O
2
+ H
2
O  H
2
2
SO
4
6.
The balanced equation for the complete combustion of propane is
C
3
H
8
+ 5O
2
 3CO
2
+ 4H
2
O
If 6.02 x 10 24 molecules of propane are burnt with 64.0 g of oxygen, determine: a) The mass of water vapour produced b) The mass of excess reactant remaining.

Answers:
1.
a) 4.30 g AgCl
2.
a) 120 g NO
3.
a) 67.94 g AlI
3
4.
a) 9.2 g NO
2
5.
a) 147.12 g H
2
SO
4
6.
a) 28.83 g H
2
O b) 2.24 g KCl b) 64.0 g O
2 b) 1.0 x 10 23 mlc AlI
3 b) 4.0 mol NO
2 b) 423.46 g C
3
H
8