Reaction 1
1. Measure out 3.25-3.50 g of copper(II) chloride dihydrate into a 100 mL beaker. Record the actual mass below.
Add ~50 mL of distilled water to the beaker and stir to dissolve the salt.
Actual mass = 3.45g
2. Measure out 0.15-0.20 g of aluminum foil and record the actual mass here.
Actual mass = 0.17g
3. Tear the aluminum foil into small pieces but keep them as sheets. Add the aluminum pieces to the beaker and
stir for five minutes, then let the reaction sit for at least one minute.
Reaction 2
4. Measure out 1.25-1.50 g of copper(II) chloride dihydrate into a 100 mL beaker. Record the actual mass below.
Add ~50 mL of distilled water to the beaker and stir to dissolve the salt.
5. Measure out 0.20-0.25 g of aluminum foil and record the actual mass here.
6. Tear the aluminum foil into small pieces but keep them as sheets. Add the aluminum pieces to the beaker and
stir for five minutes, then let the reaction sit for at least one minute.
ANALYSIS & CALCULATIONS
7. Record your observations of Reaction 1 below.
Brownish-red solid copper formed on the surface of the aluminum. When the reaction was complete there was
no visible solid aluminum remaining- the only visible solid was the copper.
8. Record your observations of Reaction 2 below.
Brownish-red solid copper formed on the surface of the aluminum. When the reaction was complete there was
still solid aluminum remaining in the beaker, in addition to solid copper.
9. Based on these observations, which reactant is limiting, and which reactant is in excess in Reaction 1? Explain
briefly.
10. Based on these observations, which reactant is limiting and which reactant is in excess in Reaction 2? Explain
briefly.
11. Write a balanced chemical equation, including phase labels, for the reaction that you performed today:
Aluminum foil reacts with aqueous copper(II) chloride to produce aqueous aluminum chloride and copper
metal.
12. Which type of reaction is this?
13. Using the given amounts of copper(II) chloride dihydrate and aluminum in Q3-4, calculate the mols of each
reactant and then determine which reactant is the LR. Does this match what you concluded in Q11from the
visual observations? Show your work and use correct digits in your answer
14. Using your LR above, calculate the theoretical yield (in grams) of copper metal that should have been produced
in Reaction 1. Show your work and use correct digits in your answer!
15. If you wanted to isolate the most pure copper product, would it be easier to do from Reaction 1 or Reaction 2?
Explain.