Two statements, one Assertion and the other Reason, are given. Choose the correct option. Assertion: During the electrolysis of aqueous NaCl , Cl ₂ is liberated at the anode in preference to O ₂ and water gets reduced to H ₂ at cathode. Reason: The reaction at Anode with lower oxidation potential is not preferred due to over potential of Oxygen.

Step-by-step solution

In the electrolysis of aqueous NaCl , the competing reactions at the anode are: 1. 2 Cl ⁻(aq) Cl ₂(g) + 2e⁻ , E^ = 1.36 V 2. 2 H ₂ O (l) O ₂(g) + 4 H ⁺(aq) + 4e⁻ , E^ = 1.23 V Although the standard oxidation potential for water is lower, the evolution of oxygen gas at the anode requires an additional overpotential. Due to this overpotential, the oxidation of Cl ⁻ occurs preferentially, leading to the liberation of Cl ₂ gas. At the cathode, the reduction of water ( 2 H ₂ O + 2e⁻ H ₂ + 2 OH ⁻ ) is preferred over the