What is the quantity of electricity required to produce $4.8 \ g$ of $Mg$ (molar mass $= 24 \ g \ mol^{-1}$) from its salt solution (in $F$)?

To deposit $0.6354 \ g$ of copper by electrolysis of aqueous cupric sulphate solution,the amount of electricity required (in coulombs) is

Assertion $(A)$: The charge on one mole of electrons is one Faraday.
Reason $(R)$: The quantity of current required to deposit one mole of $Mg$ from $Mg^{2+}$ electrolyte solution is two Faradays.
The correct answer is

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

$A$ current of $0.5 \ A$ is passed through molten $AlCl_3$ for $96.5 \ s$. The mass of aluminium deposited at cathode is $x \ mg$ and volume of chlorine liberated (at $STP$) at anode is $y \ mL$. $x$ and $y$ are respectively

The amount of substance liberated on electrodes during electrolysis when $1 \ C$ of electricity is passed,is