The $E.C.E.$ of $Cu$ and $Ag$ are $7 \times 10^{-6} \ g/C$ and $1.2 \times 10^{-6} \ g/C$ respectively. If a certain current deposits $14 \ g$ of $Cu$,the amount of $Ag$ deposited is .............. $g$.

$A$ solution of $CuSO_4$ is electrolysed for $10 \,min$ with a current of $1.5 \,A$. What is the mass of copper deposited at the cathode (in $,g$)?

When $96500 \ C$ of electricity is passed through a copper sulphate solution,the amount of copper deposited will be ............... $mol$.

What is the number of faraday required to produce $0.18 \ g$ aluminium at cathode during electrolysis of molten $AlCl_3$ (in $F$)? (Molar mass of $Al = 27 \ g \ mol^{-1}$)

Two electrolytic cells are connected in series containing $CuSO_4$ solution and molten $AlCl_3$. If in electrolysis $0.4$ moles of $Cu$ are deposited on the cathode of the first cell,the number of moles of $Al$ deposited on the cathode of the second cell is: (in $moles$)

$1$ mole of electrons corresponds to how much Faraday,how much Coulomb,and how many electrons?