Faraday's laws of electrolysis state that the mass deposited on an electrode is proportional to:

For the oxidation of $0.2 \text{ M} \text{ FeSO}_4$ solution,$0.965 \text{ A}$ current is passed through it for $1 \text{ hour}$. The volume of the solution that is oxidised in $\text{mL}$ is:

How much charge is required for the following reductions:
$(i)$ $1 \, mol$ of $Al^{3+}$ to $Al$.
$(ii)$ $1 \, mol$ of $Cu^{2+}$ to $Cu$.
$(iii)$ $1 \, mol$ of $MnO_{4}^{-}$ to $Mn^{2+}$.

How much time (in $sec$) is required to coat a metal surface of $80 \, cm^2$ with a $0.005 \, mm$ thick layer of silver from a silver nitrate solution using a current of $3 \, A$? (Density of silver $= 10.5 \, g \, cm^{-3}$)

One ampere of current is passed for $9650 \ s$ through molten $AlCl_3$. What is the weight in grams of $Al$ deposited at the cathode? (Atomic weight of $Al = 27$)

When electricity is passed through a solution of $AlCl_3$,$13.5 \ g$ of $Al$ is deposited. What is the number of Faradays used?