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

For the reaction $Al^{3+} + 3e^{-} \rightarrow Al$ (atomic mass of $Al = 27 \ g \ mol^{-1}$),calculate the quantity of electricity in coulombs required to produce $5.12 \ kg$ of $Al$.

$A$ solution of $CuSO_4$ is electrolysed for $10$ minutes with a current of $1.5$ amperes. What is the mass of copper deposited at the cathode (in $g$)?

How much electricity is required in Faraday to produce $40.0 \ g$ of $Al$ from molten $Al_2O_3$? (Atomic mass of $Al = 27 \ g \ mol^{-1}$)

When $4.5 \, A$ current is passed through $1 \, L$ of $0.6 \, M$ $CuCl_2$ solution for $1.15 \, hour$,calculate the mass of $Cu$ and the change in concentration of the solution. $[Cu = 63.5 \, u]$

$A$ current of $0.4 \ A$ is passed through excess of molten $MgCl_2$ for $9.65 \times 10^4 \ sec$. The mass of $Mg$ deposited at the cathode is .............. $gm$