Electrolytic Cells and Faraday's Laws

Electrolytic Cells

In an electrolytic cell, a DC voltage is applied to two electrodes, leading to the oxidation of copper at the anode and the reduction (deposition) of copper at the cathode.
Reactions:
- At the cathode: Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)
- At the anode: Cu(s) \rightarrow Cu^{2+}(s) + 2e^-
Industrial process:
- Impure copper rod serves as the anode and dissolves as current passes through.
- Pure copper rod is used as the cathode, where Cu^{2+} ions deposit.
Electrolytic Cell Ion Movement:
- Cations (positive ions) are attracted to the cathode (negative electrode).
- Cations are discharged at the cathode by accepting electrons; reduction occurs.
- Note: This is opposite to galvanic cells, where the cathode is the positive electrode.
Anode:
- The anode in an electrolytic cell is the positive electrode.
- Oxidation of anions (negative ions) takes place at the anode.

Electrolytic cells are used in the large-scale production of metals like Na, Mg, and Al.
These metals are produced by electrochemical reduction of their respective cations.
This method is used when suitable chemical reducing agents are not available.