Faraday's laws of electrolysis are related to the

In the Hall process,aluminium is produced by the electrolysis of molten $Al_2O_3$. How many seconds would it take to produce enough aluminium by the Hall process to make a case of $24$ cans of aluminium soft-drink,if each can uses $5.0 \ g$ of $Al$,a current of $9650 \ A$ is employed,and the current efficiency of the cell is $90.0 \ \%$?

The number of electrons involved in redox reactions when $1$ Faraday of electricity is passed through an electrolyte in solution is

The time required (in hours) to reduce $3 \ mol$ of $Fe^{3+}$ ions to $Fe^{2+}$ ions with $2.0 \ A$ of current is $\left(1 \ F = 96500 \ C \ mol^{-1}\right)$ (in $.2$)

If $5 \ A$ of current is passed for $193 \ s$ through a solution containing $Cu$ salt,$0.32 \ g$ of copper is deposited. What is the oxidation state of the $Cu$ in the salt?

Match the column :-

Column $I$ (Reduction process)	Column $II$ (Charge required)
$(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$	$(p)$ $193000$ $C$
$(b)$ $1$ mol of $Cr_2O_7^{2-}$ to $Cr^{3+}$	$(q)$ $289500$ $C$
$(c)$ $1$ mol of $Sn^{4+}$ to $Sn^{2+}$	$(r)$ $482500$ $C$
$(d)$ $1$ mol of $Al^{3+}$ to $Al$	$(s)$ $579000$ $C$