Final answer:
In an electrolytic cell using aqueous copper sulfate, the anode reaction is Cu (s) → Cu2+ (aq) + 2e− and the cathode reaction is Cu2+ (aq) + 2e− → Cu (s). These reactions describe the electroplating process where copper is transferred from the anode to the cathode.
Step-by-step explanation:
The half-reactions at the anode and cathode in an electrolytic cell using aqueous copper sulfate (CuSO4) can be described as follows:
- Anode (oxidation): Cu (s) → Cu2+ (aq) + 2e−
- Cathode (reduction): Cu2+ (aq) + 2e− → Cu (s)
In the electroplating process, copper from the anode is oxidized, allowing copper ions to enter the solution, while at the cathode, copper ions from the solution are reduced and deposited onto the surface of the metal.
For a galvanic cell, such as one involving a zinc electrode and copper(II) ions in aqueous solution, the reactions would be different, with zinc undergoing oxidation at the anode and copper ions being reduced at the cathode.