How many faradays of electricity is required to produce $4.8 \ g$ of $Mg$ at cathode in the electrolysis of molten $MgCl_2$ (in $F$)? (Molar mass of $Mg = 24 \ g/mol$)

When a current of $2 \ A$ is passed through a molten tin salt for $5 \ hours$,$22.2 \ g$ of tin is deposited. What is the oxidation state of tin in the salt? (Atomic weight of $Sn = 118.69$)

Three faradays of electricity were passed through an aqueous solution of iron $(II)$ bromide. The weight of iron metal (atomic weight $= 56$) deposited at the cathode (in $g$) is

$96.5$ amperes current is passed through the molten $AlCl_3$ for $100$ seconds. The mass of aluminium deposited at the cathode is (atomic weight of $Al = 27$ $u$). (in $g$)

In the electrolysis of water,one Faraday of electrical energy would evolve

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 $Al$	$(s)$ $579000$ $C$