Give reasons-On the basis of E-o values- O-2 gas should be liberated anode but it is Cl-2 gas which is liberated in the electrolysis of aqueous NaCl-

Question

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It is due to the phenomenon of over-voltage- Experimentally- it is observed that the actual voltage required for electrolysis is greater than that calculated from standard potentials- This addition voltage required is called over-voltage- It is required because the rate of transfer of electrons at the interface of electrode and solutions for both half reactions is slow- The over-voltage required for formation of oxygen is much larger than that required for the formation of chlorine- Hence- chlorine-xA0- gas which is liberated in the electrolysis of aqueous NaCl-

Give reasons:On the basis of Eo values, O2 gas should be liberated at anode but it is Cl2 gas which is liberated in the electrolysis of aqueous NaCl.

Give reasons:
On the basis of $E^{o}$ values, $O_{2}$ gas should be liberated at anode but it is $C l_{2}$ gas which is liberated in the electrolysis of aqueous NaCl.