How many total Faraday currents will be required to obtain $1 \ mole$ of $Ag$,$Mg$,and $Al$ respectively?

Two electrolytic cells containing $CuSO_4$ and $AgNO_3$ respectively are connected in series and a current is passed through them until $1 \, mg$ of copper is deposited in the first cell. The amount of silver deposited in the second cell during this time is approximately ......... $mg$ [Atomic weights of copper and silver are respectively $63.57$ and $107.88$]

$96.5$ amperes current is passed through the molten $AlCl_3$ for $100$ seconds. The mass of aluminium deposited at the cathode is (atomic weight of $Al = 27$ $u$). (in $g$)

On passing $C$ ampere of electricity through an electrolyte solution for $t$ seconds,$m$ grams of metal are deposited on the cathode. The equivalent weight $E$ of the metal is:

The quantity of charge required to obtain $2$ moles of aluminium from $Al_2O_3$ is: (in $F$)

When a certain amount of electricity is passed through a solution of $Al^{3+}$,$4.5 \ g$ of aluminum (atomic mass $27 \ amu$) is deposited at the cathode. If the same amount of electricity is passed through $H^{+}$ ions,what volume of hydrogen (in $L$) is produced at $STP$?