How many faraday of electricity is required to produce $10 \ g$ of calcium metal (molar mass $= 40 \ g \ mol^{-1}$) from calcium ions (in $F$)?

Match the column :-

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

How many electrons are involved in the reaction when $0.40 \ F$ of electricity is passed through an electrolytic solution?

How many faraday of electricity are required to deposit $10 \ g$ of calcium from molten calcium chloride using inert electrodes (in $F$)? (Molar mass of calcium $= 40 \ g \ mol^{-1}$)

How many seconds of current at $9.65 \ A$ must be passed through a solution of $Al^{3+}$ to obtain $1 \ \text{millimole}$ of $Al$ metal?

Total charge on $1 \, \text{mole}$ of a monovalent metal ion is equal to