Laboratory 4 –
Stoichiometry of
Copper (II) Chloride
and Aluminum
Purpose: Determine the stoichiometry of
CuCl2 (aq) + Al (s)  AlCl3 (aq) + Cu (s)
Materials: Copper (II) chloride solution
Aluminum (2.5 cm x 2.5 cm), 2 500 mL
beakers, ring stand, filter paper, balance,
thermometer
Laboratory 4 –
Stoichiometry of
Copper (II) Chloride
and Aluminum
Procedure:
1. Weigh the Al foil. Place 10 mL of the CuCl2
solution in the one beaker and measure it’s
temperature.
2. Write you group number and period on the filter
paper. Weight it and record the mass.
3. Lightly crumple the foil and place in the beaker.
You can push it under the surface with the
thermometer. Lightly stir with the thermometer.
Laboratory 4 –
Stoichiometry of
Copper (II) Chloride
and Aluminum
Procedure (cont):
4. Measure the temperature every 30 secs.
5. After 5 mins., filter out the solid in the beaker. Rinse
with tap water to get all the solid out of the beaker.
6. Place the filter paper in the oven and the filtrate in the
waste beaker
7. Thoroughly rinse the beakers, graduated cylinder, and
glass funnel with tap water.
8. Weigh the filter paper tomorrow.
Laboratory 4 –
Stoichiometry of
Copper (II) Chloride
and Aluminum
Observations before the chemical reaction:
Mass of Aluminum (g)
Mass of Filter Paper (g)
Temperature after the aluminum is added:
Time (min)
0
0.5
1.0
1.5
2.0
Temperature (°C)
Time (min)
2.5
3.0
3.5
4.0
4.5
Temperature (°C)
Observations after the addition of the aluminum:
Solid in the beaker
Liquid in the beaker
Mass of Filter Paper (g) Day 2
Laboratory 4 –
Stoichiometry of
Copper (II) Chloride
and Aluminum
Analysis:
Balance the equation, then use the mass of
the aluminum to calculate the mass of
copper theoretically produced. Compare
this to the mass of copper determined by
the experiment.