What amount of electricity can deposit $1 \ mole$ of $Al$ metal at cathode when passed through molten $AlCl_3$?

One litre solution of $MgCl_2$ is electrolyzed completely by passing a current of $1 \ A$ for $16 \ min \ 5 \ sec$. The original concentration of $MgCl_2$ solution was (Atomic mass of $Mg = 24$)

Faraday's laws of electrolysis will fail when

In the electrolysis of acidulated water,it is desired to obtain $1.12 \ cc$ of hydrogen gas per second at $STP$ conditions. The current to be passed is: (in $A$)

The electrolytic cells,one containing acidified ferrous chloride and another acidified ferric chloride,are connected in series. The ratio of iron deposited at the cathodes in the two cells when electricity is passed through the cells will be:

How many Faraday of electricity is required to deposit $0.8 \ g$ of calcium at cathode by the electrolysis of $CaCl_2$ (in $F$)?