An impure copper anode of mass 800 g contains 95.0% Cu, 2.60% Zn, 1.40% Fe and 1.00% of Ag and Au (by mass). It is dissolved completely in acidified $\mathrm{CuSO}{}_4$ electrolysis at a constant current of 40.0 A. Assume 100% current efficiency, that Cu, Zn and Fe dissolve as $\mathrm{Cu}{}^{2+}$, $\mathrm{Zn}{}^{2+}$ and $\mathrm{Fe}{}^{2+}$, and that Ag and Au fall as anode mud. Using Cu = 63.5, Zn = 65, Fe = 56 and F = 96500 C/mol, find the time required in hours (answer to two decimals).

Numerical answer type, answer in h, tolerance 0.01.