Question

In the electrolysis of aqueous sodium chloride solution which
of the half cell reaction will occur at anode?
(a) Na⁺ (aq) + e⁺ → Na (s) ; E°꜀ₑₗₗ = - 2.71V
(b) 2H₂O(l) → O₂ (g) + 4H⁺ (aq) + 4e⁻ ; E°꜀ₑₗₗ = 1.23V
(c) H⁺ (aq) + e⁻ → 1/2 H₂ (g) ; E°꜀ₑₗₗ = 0.00 V
(d) Cl⁻ (aq) → 1/2 Cl₂ (g) + e⁻ ; E°꜀ₑₗₗ = 1.36 V

Answer 1

Answer:

[d] is the answer

Cl⁻ (aq) → 1/2 Cl₂ (g) + e⁻

Explanation:

Anode is positively charged so it is deficient of electrons and attracts the anions in the aqous medium. So after losing electrons to anode the chloride ions becomes the chlorine

Answer 2

The electrolysis is a way of separation of a compound by passing an electric current through it leading to formation of ions.

The  electrolysis of aqueous sodium chloride solution

At anode we will have (d) Cl⁻ (aq) → 1/2 Cl₂ (g) + e⁻ ; E°꜀ₑₗₗ = 1.36 V

• Electrolysis of aq.NaCl results in Hydrogen and Chlorine gas.
• At cathode (positive electrode) ,reduction of the compound takes place leading to form Hydroxide ion and Hydrogen gas.
• At anode we have negative electrode so, anode hosts oxidation reaction.
• So, oxidation of chloride ion takes place, leading to chlorine gas formation.
• The reaction involved is   Cl⁻ (aq) → 1/2 Cl₂ (g) + e⁻ ; E°꜀ₑₗₗ = 1.36 V