The unit of Faraday is

Aluminium oxide may be electrolysed at $1000 \, ^\circ C$ to furnish aluminium metal (At. Mass $= 27 \, amu$; $1 \, F = 96,500 \, C$). The cathode reaction is $Al^{3+} + 3e^- \to Al^0$. To prepare $5.12 \, kg$ of aluminium metal by this method would require:

On passing $0.1 \ F$ of electricity through aluminium chloride,the amount of aluminium metal deposited on the cathode is $(Al = 27)$ ............ $g$.

When an electric current is passed through a solution of $KCl$,$19.5 \ g$ of potassium (atomic mass $= 39$) is deposited. If the same amount of electric current is passed through a solution of $AlCl_3$,how many grams of aluminum will be liberated?

On passing $C$ ampere of current for time $t$ seconds through $1 \ L$ of $2 \ M$ $CuSO_4$ solution (atomic weight of $Cu = 63.5$),the amount $m$ of $Cu$ (in grams) deposited on the cathode will be:

What weight of copper will be deposited by passing $2$ Faradays of electricity through a cupric salt? (Atomic weight of $Cu = 63.5$)