1. Cu (s) + 2AgNO3(aq) → Cu(NO3)2 (aq) + 2Ag(s)
What mass of silver is produced when g of copper shavings are added to a silver nitrate solution containing 1.95 g of silver nitrate?
Cu (s) + 2AgNO3(aq) → Cu(NO3)2 (aq) + 2Ag(s)
0.500 g Cu x 1 mol Cu x 2 mol Ag x g Ag
63.55 g Cu mol Cu mol Ag
= g Ag
1.95 g AgNO3 x 1 mol AgNO x 2 mol Ag x g Ag
g AgNO mol AgNO mol Ag
= g Ag

2. Cu (s) + 2AgNO3(aq) → Cu(NO3)2 (aq) + 2Ag(s)
How many grams of the excess reactant are left over when this reaction is complete?
Cu (s) + 2AgNO3(aq) → Cu(NO3)2 (aq) + 2Ag(s)
1.24 g Ag x mol Ag x 1 mol Cu x g Cu = g Cu
g Ag mol Ag mol Cu
0.500g Cu g Cu = g Cu

3. If a student really performed this reaction in the lab and only collected 1.17g of silver, what would be her percent yield?
Cu (s) + 2AgNO3(aq) → Cu(NO3)2 (aq) + 2Ag(s)
% Yield = Actual Yield x 100
Theoretical Yield
% Yield = g Ag x 100 = 94.4%
1.24 g Ag

4. % Yield = Actual Yield x 100 Theoretical Yield 0.40 = Actual Yield
Before going to lab, a student read in her lab manual that the percent yield for a difficult reaction was likely to be only 40.% of the theoretical yield. The student's prelab stoichiometric calculations predict that the theoretical yield should be 12.5 g. What's the student's likely actual yield?
% Yield = Actual Yield x 100
Theoretical Yield
0.40 = Actual Yield
12.5 g
Actual Yield = (0.40) (12.5g) = 5.0 g