The value of one Faraday is .............. $C \ mol^{-1}$.

$A$ current of strength $2.5 \ A$ was passed through $CuSO_4$ solution for $6 \ \text{minutes} \ 26 \ \text{seconds}$. The amount of copper deposited is .............. $g$ (Atomic weight of $Cu = 63.5$) $(1 \ F = 96500 \ C)$

$CuSO_4$ solution is electrolysed for $15 \ minutes$ to deposit $0.4725 \ g$ of copper at the cathode. The current in amperes required is (Faraday $= 96,500 \ C \ mol^{-1}$,atomic weight of copper $= 63$)

How much electricity in terms of Faraday is required for the reduction of $2 \ mol$ of $Cr_2O_7^{2-}$ into $Cr^{3+}$ in an acidic medium (in $F$)?

The density of $Cu$ is $8.94 \, g \, cm^{-3}$. The quantity of electricity needed to plate an area $10 \, cm \times 10 \, cm$ to a thickness of $10^{-2} \, cm$ using $CuSO_4$ solution would be,if atomic mass of $Cu$ is $63.5$ .................. $C$

For the given reaction how much quantity of electricity in Coulomb is required? $\frac{2}{3} Al_2O_3 \rightarrow \frac{4}{3} Al + O_2$