When an aqueous solution of `CuCl_(2)` is electrolysed using Pt inert electrodes, the reaction at cathode and anode respectively are

Options

A. `4H_(2)O(l) overset(+4e)rarr2H_(2)(g) +4OH_(2)(aq), 2H_(2)O(l) overset(-4e^(-))rarrO_(2)(g)+4H^(+)(aq)`
B. `2Cu^(2+) (aq) overset(+4e^(-))rarr2Cu(s), 2H_(2)O(l) overset(-4e^(-))rarrO_(2)(g)+4H^(+)(aq)`
C. `Cu^(2+)(aq) overset(+2e^(-))rarrCu(s), 2Cl^(-) (aq) overset(-2e^(-))rarrCl_(2)(g)`
D. `2H_(2)O(l) overset(+2e^(-))rarrH_(2)(g)+2OH (aq), 2Cl^(-)(aq) overset(-2e^(-))rarrCl_(2)(g)`

Answer

C

Explanation

`CuCl_(2) rarr Cu^(2) (aq) +2Cl^(-) (aq)`
`Cl^(-)` show oxidation at anode and form `Cl_(2)` gas.
`2Cl^(-) overset(-2e^(-))rarrCl_(2)(g)`
Due to less reactivity, `Cu^(2+)` gain electrons and deposited at cathode electrode.
`Cu^(2+) +2e^(-) rarr Cu`