Cathode:
Al³⁺(l) + 3e⁻ → Al(l)
Anode:
2Cl⁻(l) → Cl₂(g) + 2e⁻
Overall reaction:
2AlCl₃(l) → 2Al(l) + 3Cl₂(g)
Explanation:
* Molten aluminum chloride: The starting material is molten aluminum chloride, which is a liquid at high temperatures.
* Electrolysis: This process involves passing an electric current through the molten salt.
* Cathode: The cathode is the negative electrode where reduction occurs. Aluminum ions (Al³⁺) gain electrons and are reduced to liquid aluminum metal.
* Anode: The anode is the positive electrode where oxidation occurs. Chloride ions (Cl⁻) lose electrons and are oxidized to chlorine gas.
Important notes:
* The electrolysis of molten aluminum chloride is a commercially important process for producing aluminum metal.
* The process requires a high temperature (about 1000 °C) to keep the aluminum chloride molten.
* The chlorine gas produced as a byproduct can be used in other industrial processes.
