Chemistry – Electrochemistry - Electrolysis | e-Consult

Explanation: Electrolysis of aqueous potassium chloride results in the formation of both hydrogen gas and chlorine gas. This occurs because the ions in the aqueous solution are mobile and can be reduced or oxidised.

Cathode: Hydrogen gas (H₂) is formed at the cathode. The reduction half-reaction is: 2H⁺(aq) + 2e^- → H₂(g)

Anode: Chlorine gas (Cl₂) is formed at the anode. The oxidation half-reaction is: 2Cl^-(aq) → Cl₂(g) + 2e^-

Reasoning: Potassium (K⁺) is a metal and is readily reduced to form potassium metal. However, the concentration of K⁺ is relatively low in the aqueous solution, and the reduction of H⁺ to H₂ is favoured over the reduction of K⁺. Similarly, chloride ions (Cl^-) are readily oxidised to form chlorine gas.