In the electrolysis of aqueous sodium chloride solution, which of the half cell reactions will occur at anode?

In the electrolysis of aqueous sodium chloride solution, which of the

1.	In the electrolysis of aqueous sodium chloride solution, which of the half cell reactions will occur at anode?
Answer» `CI_(aq) to (1)/(2)CI_(2)+ e^(-), E_("cell")^(0)= 1.36 "VOLTS"` `2H_(2)O_(l) to O_(2)+ 4H^(+)+ 4e^(-), E_("cell")^(0)= 1.23 "volts"` `Na_(aq)^(+) e^(-) to Na_(s), E^(0)= -2.71 "volts"` `H_(aq)^(+)+ e^(-) to (1)/(2)H_(2), E_("cell")^(0)= 0.00"volts"` Solution :During electrolysis of aqueous NaCl FOLLOWING oxidation reaction are possible: `Cl_(aq) to (1)/(2) Cl_(2(g))+e^(-)` , `E_("cell")^(o)=1.36 V` ...(i) `2H_(2)O_(l) to O_(2(g))+4H_(aq)^(+)+4e^(-)`, `E_("cell")^(o)=1.23 V` ...(II) The reaction at anode with lower value of `E^(o)` is preferred and therefore, water should get oxidised in preference to `Cl_(aq)^(-)`. However on account of overpotential of oxygen, reaction (i) is preferred. Thus, Cathode: `H_(2)O_(l)+e^(-) to (1)/(2) H_(2(g))+OH_(aq)^(-)` Anode: `Cl_(aq)^(-) TI (1)/(2)Cl_(2(g))+e^(-)`