Theoretical Yield Vs. Actual Yield: Sample Lab Data
Name:_____________________ Hr:___
Rhee Action was in the chemistry lab when some aluminum metal fell into a container of bluecolored copper(II) nitrate Cu(NO3)2 solution. An immediate reaction occurred producing much heat,
the blue color faded, and a shiny, brown product, Cu, was formed.
1. Write the balanced equation for this reaction.
2. What type of reaction is this?_____________________________________
Rhee decided to do this reaction under more controlled conditions. At the end of the experiment
there was aluminum remaining, copper product, and a clear, colorless solution. She decanted the
solution, removed the aluminum, and dried the copper product. She recorded:
Mass of aluminum before reaction
Mass of aluminum after reaction
Mass of copper and beaker
Mass of empty beaker
2.59g
1.35g
52.73g
48.52g
SHOW WORK AND UNITS FOR THE FOLLOWING CALCULATIONS:
3. Determine the mass of aluminum that reacted.
4. Use the mass of aluminum and stoichiometry to calculate the expected mass of copper produced
from this reaction, also known as "theoretical yield".
5. Determine the experimental mass of copper produced, or "actual yield".
6. Calculate the percent yield using the following formula:
7. Calculate the percent error using the following:
% yield =
8. What do you notice about these percentages?
9. Identify the reactant in excess:_________________________
10. Identify the limiting reactant:_________________________
theoretical yield
x 100
theoretical yield−actual yield
% error = |
[Note the absolute value signs]
actual yield
theoretical yield
|x 100