When $1 \ C$ of electricity is passed through an electrolytic solution,the mass deposited on the electrode is equal to which of the following?

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 ............. $g$.

What is the time (in $sec$) required for depositing all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution by passing a current of $241.25 \ A$? $(1 \ F = 96500 \ C)$

From which solution $2 \ F$ electrical charge will deposit $1 \ g$ atomic weight at cathode?

How much electricity is required in coulomb for the oxidation of
$(i)$ $1 \, mol$ of $H_2O$ to $O_2?$
$(ii)$ $1 \, mol$ of $FeO$ to $Fe_2O_3?$

When $1 \ C$ of charge is passed through an electrolyte solution,the mass deposited is equal to: