Charge required to liberate $11.5 \ g$ of sodium is:

$Al_2O_3$ is reduced by electrolysis at low potential and high current. If a current of $4 \times 10^4 \ A$ is passed through molten $Al_2O_3$ for $6 \ h$,how many grams of $Al$ will be produced? (Assume $100\%$ current efficiency and atomic mass of $Al = 27 \ g \ mol^{-1}$)

On passing electric current through molten aluminium chloride,$11.2 \ L$ of $Cl_2$ is liberated at $NTP$ at the anode. The quantity of aluminium deposited at the cathode is .............. $g$ (atomic weight of $Al = 27$).

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

The Faraday constant is $......$

$Assertion (A)$: $A$ current of $96.5 \ A$ is passed into aqueous $AgNO_3$ solution for $100 \ s$. The weight of silver deposited is $10.8 \ g$ (At. wt. of $Ag = 108$).
$Reason (R)$: The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.
The correct answer is :