Which of the following statements is true regarding electrolysis of aqueous solution of sodium chloride?

During the electrolysis of aqueous solution of sodium chloride hydrogen gas is produced at the cathode, while chlorine gas is obtained at anode. There are two substances that can be reduced at the cathode: Na⁺ ions and water molecules. At cathode: Na⁺ + e^-  Â® Na       E^o_red = -2.71 V 2 H₂O + 2 e^- Â®H₂ + 2 OH^-                   E^o_red = -0.83 V It is much easier to reduce water than Na⁺ ions. Hence, the only product formed at the cathode is hydrogen gas. There are two substances that can be oxidized at the anode: Cl^- ions and water molecules. At anode:  2 Cl^- Â® Cl₂ + 2 e^-                        E^o_ox = -1.36 V 2 H₂O Â® O₂ + 4 H⁺ + 4 e^-                       E^o_ox = -1.23 V Due to closeness of the standard-state potentials for these half-reactions, we might expect a mixture of Cl₂ and O₂ gas collect at the anode. However, in practice only chlorine gas is obtained at anode.