Calculate the quantity of electricity required to liberate $0.224 \ dm^3$ of chlorine at $STP$ during the electrolysis of fused sodium chloride (in $C$)?

$Assertion (A)$: $A$ 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 :

When $9650 \ C$ of charge is passed through an $AgNO_3$ solution during the electrolysis process in an electroplating bath,what is the weight of silver deposited at the cathode in $g$?

The number of electrons involved in redox reactions when $1$ Faraday of electricity is passed through an electrolyte in solution is

When $9.65 \ C$ of electricity is passed through a solution of silver nitrate (atomic weight of $Ag = 108$),the amount of silver deposited is $............ \ mg$.

When the same quantity of electricity is passed through solutions of $Ag^{+}$,$Cu^{2+}$,and $Fe^{3+}$ ions,what is the ratio of the number of moles of each metal deposited?