What is the number of faraday required to form $1 \ mol \ H_2$ by reduction of $H^{+}$ ions?

The relation between Faraday constant $F$,electron charge $e$,and Avogadro number $N$ is:

Calculate the amount of electricity required in coulombs to convert $0.08 \ mol$ of $MnO_4^{-}$ to $Mn^{2+}$. (in $C$)

Calculate the current in ampere required to deposit $4.8 \ g$ of $Cu$ from its salt solution in $30 \ minutes$. $\left[ \text{Molar mass of } Cu = 63.5 \ g \ mol^{-1} \right]$ (in $A$)

The amount of metal deposited at the cathode on passing an electric current of $0.75 \ A$ in an aqueous ferric sulphate solution for $30 \ min$ will be - ........... $g$ (atomic weight of $Fe = 56$).

Which of the following represents the first law of Faraday?