The mass of a substance liberated when a charge $q$ flows through an electrolyte is proportional to

The time required (in hours) to reduce $3 \ mol$ of $Fe^{3+}$ ions to $Fe^{2+}$ ions with $2.0 \ A$ of current is $\left(1 \ F = 96500 \ C \ mol^{-1}\right)$ (in $.2$)

$A$ certain quantity of electricity is passed through an aqueous solution of $AgNO_3$ and a cupric salt solution connected in series. The amount of $Ag$ deposited is $1.08 \ g$. The amount of copper deposited is ............. $g$ (atomic weight of $Cu = 63.5$; $Ag = 108$).

The amount of charge required to liberate $11.5 \ g$ of sodium is .....

How much electricity is required to deposit $108 \ g$ of silver from a silver nitrate solution?

The atomic weights of silver and copper are $108$ and $64$ respectively. $A$ silver voltameter and a copper voltameter are connected in series,and when current is passed,$10.8 \ g$ of silver is deposited. The mass of copper deposited will be ............. $g$.