0.592 g of copper is deposited in 60 minutes by passing

0.5 A current through a solution of copper (II) sulphate. The electro chemical equivalent of copper (II) (in $\mathrm{gC}^{-1}$ ) is

( $F=96500 \mathrm{C} \mathrm{mol}^{-1}$ )

Two statements are given below.

Statement I : Molten NaCl is electrolysed using Pt electrodes. $\mathrm{Cl}_{2}$ is liberated at anode.

Statement II : Aqueous $\mathrm{CuSO}_{4}$ is electrolysed using Pt electrodes. $\mathrm{O}_{2}$ is liberated at cathode.

The correct answer is