A 2.50 kg impure copper anode contains 96.0% Cu, 1.80% Zn, 0.65% Ni and the rest Ag and Au. It is dissolved completely at the anode and the same charge is passed through the cell, with pure copper deposited at the cathode (only $\mathrm{Cu}{}^{2+}$ is discharged; Zn and Ni dissolve as $\mathrm{Zn}{}^{2+}$ and $\mathrm{Ni}{}^{2+}$). Taking Cu = 63.5, Zn = 65, Ni = 59, the net mass of copper lost from the electrolyte is

1. A17.5 g
2. B44.0 g
3. C2400 g
4. D61.5 g