The approximate time duration in hours to electroplate $30 \ g$ of calcium from molten calcium chloride using a current of $5 \ A$ is [At. mass of $Ca=40$]

$Assertion (A)$: $A$ 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 :

The quantity of electricity required to liberate $5600 \ mL$ of $H_2$ at $STP$ is the same as that required to liberate how many grams of silver (equivalent weight = $108$)?

$5 \, A$ current is passed through an electrolytic cell filled with $AgNO_3$ solution for $2.7$ hours. If $1$ spoon requires $0.01 \, g$ of silver to get coated,calculate how many spoons can be coated by the silver obtained at the cathode? $[Ag = 108 \, u]$

When electricity is passed through the solution of $AlCl_3$,$13.5 \ g$ of $Al$ are deposited. The number of Faraday required is:

During electrolysis of fused aluminium chloride,$0.9 \ g$ of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be .............. $litres$ (at $STP$).