Lab #20: Aluminum and Copper (II) Chloride Redox Lab
Chemistry
10 points
**Pre-lab requires title, question, hypothesis, research, and hazards**
Question:
Which chemical is oxidized and which chemical is reduced when aluminum reacts with
aqueous copper (II) chloride?
Hypothesis:
[Use a complete sentence to predict which elements will be oxidized and reduced during this
lab.]
Research:
- Please do not write the questions! Please do not number the questions! Use complete sentences!
1)
2)
3)
4)
5)
6)
7)
8)
What is a limiting reactant?
What is an excess reactant?
What does oxidation mean?
What does reduction mean?
What happens during a single displacement reaction?
Write out and balance the equation for the single displacement reaction between solid
aluminum wire and aqueous copper (II) chloride solution. Include states of matter.
What does the (II) in copper (II) chloride mean?
Read through the procedure and draw a diagram of the set-up.
Materials (don’t write these in your lab book):
1 16 x 125 mm test tube
1 400 mL beaker
1 ringstand
10 mL copper (II) chloride solution
1 large test tube brush
1 permanent marker
1 sparker
1 forceps
1 beaker tongs
1 small test tube brush
1 wire gauze
1 piece of aluminum wire
1 10 mL graduated cylinder
1 test tube clamp
1 Bunsen burner
1 heat resistant pad
1 30 mL beaker
Hazards:
(Use complete sentences to mention the safety contract and the hazards of aluminum and
copper (II) chloride)
Procedure (don’t write this in your lab book):
1. Physically and chemically clean the glassware and forceps (no need to dry).
2. Label the 30 mL beaker with copper (II) chloride and initials.
3. Obtain the copper (II) chloride solution in the 30 mL beaker.
4. Measure out 10 mL of the copper (II) chloride solution with the graduated cylinder
5. Return any extra copper (II) chloride solution.
6. Attach Bunsen burner to jet
7. Attach iron ring to ring stand
8. Place wire gauze on top of iron ring
9. Attach test tube clamp above iron ring
10. Fill 400 mL beaker with approximately 250 mL of tap water
11. Place 400 mL beaker on top of wire gauze
12. Label test tube with copper (II) chloride + aluminum and initials
13. Transfer copper (II) chloride solution to test tube
14. Clamp the test tube inside the 400 mL water bath (so that the test tube does not touch the
bottom of the beaker)
15. Use forceps to add the aluminum wire to the test tube.
16. Heat the 400 mL beaker with the Bunsen burner until the reaction is complete.
17. When the reaction is complete, turn off the burner.
18. Use the clamp to carry the test tube to the solid waste container.
19. Use the forceps to carefully remove the solid products from the solution.
20. Put the solid products into the solid waste container.
21. Use the clamp to carry the test tube to the liquid waste container
22. Decant the solution (pour the solution into the waste container while reserving any
remaining solids) into the waste container
23. Add any remaining solid products to the solid waste container.
24. Clean up
a) Remove labels from glassware
b) Physically clean test tube, beaker, and graduated cylinder
c) Put equipment away
d) Get a clean-up signature
“Calculations”:
1) Give every element in the reaction equation (see research question #6) a charge
(oxidation number)
2) Identify which two elements change charge during the reaction.
3) Write and balance the half-reactions for the reaction that occurred.
(Make sure the same number of electrons were lost and gained!)
4) Label one half-reaction as oxidation
5) Label the other half-reaction as reduction
Claim:
[Use a complete sentence to answer the original question.]
Evidence:
[Use complete sentences to support your claim with data (what you saw happen) and your
calculations. Especially mention how you figured out what was oxidized and what was
reduced.]
Reasoning:
- Please do not write the questions! Please do not number the questions! Use complete sentences!
1) What was the limiting reactant in this lab? How could you tell?
2) What was the excess reactant in this lab? How could you tell?
3) Some students believe that rust was produced in this lab. What was the solid product in
this lab? Explain why it was rust or why it could not be rust.
4) This reaction occurs without being heated. Why did we heat the reaction?
5) Generate two NEW testable questions that could be asked related to this lab.
6) Would we have achieved the same results by adding solid copper wire to an aqueous
aluminum chloride solution? Why or why not?