In the electrolysis of aqueous sodium chloride solution which of the half of cell reaction will occur at anode
1
\(N{a^ + }\left( {aq} \right) + {e^ - } \to \) \(Na(s);{E^\theta }_{cell} = - 2.71V\)
2
\(2{H_2}O(I) \to \) \({O_2}(g) + 4{H^ + }(aq) + 4{e^ - }{E^\theta }_{cell} - 1.23V\)
3
\({H^ + }(aq) + {e^ - } \to \) \(\frac{1}{2}{H_2}(g);{E^\theta }_{cell} = 0.00V\)
4
\(C{I^ - }(aq) \to \) \(\frac{1}{2}Cl{}_2(g) + {e^ - };{E^\theta }_{cell} = 1.36V\)
5
Question Not Attempted