Given below are two statements. Statement I: During electrolytic...

Impure $Cu$ obtained from ores is converted to pure $Cu$ in an electrolyte cell that the impure copper as the anode an pure copper as the cathode. The electrolyte is an aqueous solution of ${CuSO}_{4}$. At the impure $Cu$ anode, $Cu$ is oxidized along with the more easily oxidized metallic impurities such as $Zn$ and Fe. The less easily oxidized impurities such as $Ag, Au$, and $Pt$ fall to the bottom of the cell as anode mud, which is reprocessed to recover the precious metals. At the pure $Cu$ cathode, ${Cu}^{2 +}$ ions get reduced to pure copper metal

Anode (oxidation) : $M\left(s\right) ⟶ {M}^{2 +}\left(aq\right) + 2{e}^{-}\left(M = Cu, Zn, Fe\right)$

Cathode (reduction) : ${Cu}^{2 +}\left(aq\right) + 2{e}^{-} ⟶ Cu\left(s\right)$

Thus, the net cell reaction simply involves transfer of $Cu$ metal from the impure anode to the pure cathode, $Cu$ obtained by this process is $99 . 95$ pure.