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

When a current of $2 \ A$ is passed through a molten tin salt for $5 \ hours$,$22.2 \ g$ of tin is deposited. What is the oxidation state of tin in the salt? (Atomic weight of $Sn = 118.69$)

Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10 \ mA$ current. The time required to liberate $0.01 \ mol$ of $H_2$ gas at the cathode is $(1 \ F = 96500 \ C \ mol^{-1})$

What is the time (in $sec$) required for depositing all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution by passing a current of $241.25 \ A$? $(1 \ F = 96500 \ C)$

The quantity of electricity needed to liberate $0.5 \ g$ equivalent of an element is

How much current is required to produce $H_2$ gas at the rate of $1 \ cc / sec$ under $STP$ (in $A$)?