Predict the products of electrolysis in each of the following :
An aqueous solution of `CuCl_(2)` with platinum electrodes.

Explanation

Electrolysis of `CuCl_(2)` solution using platinum electrodes. `CuCl_(2)(aq)rarr Cu^(2+)(aq)+2Cl^(-)(aq)`,
At cathode : `Cu^(+)` ions will be reduced in preference to `H_(2)O(l)` due to higher standard reduction potential of Cu than that of `H_(2)O(l). Cu^(2+)+2e rarr Cu`
At anode : Though standard reduction potential of the reaction, `H_(2)O(l)rarr 2H^(+)(aq)+(1)/(2)O_(2)(g)+2e` is higher than that of the reaction, `2Cl^(-)(aq)rarr Cl_(2)(g)+2e, Cl^(-)` ions will be oxidised in preference to `H_(2)O(l)` due to overvoltage of `O_(2).Cl^(-)rarr Cl+e, Cl+Cl rarr Cl_(2)(g)`. Thus, Cu will be deposited at teh cathode & `Cl_(2)` will be liberated at anode.