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

Copper is to be electrodeposited on a nickel block of $(20 \times 5) \ cm^2$ area by using $CuSO_4$ as electrolyte. How much quantity of electricity is needed to deposit a $3.6 \ \mu m$ layer of copper (in $C$)? [Atomic weight of $Cu = 63.5 \ g \ mol^{-1}$,Density of $Cu = 8.9 \ g/cm^3$]

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

When an electric current is passed through acidulated water,$112 \ mL$ of hydrogen gas at $N.T.P.$ collects at the cathode in $965 \ seconds$. The current passed,in amperes,is:

The chemical equivalent of silver is $108$. If the current in a silver voltameter is $2 \ A$,the time required to deposit $27 \ g$ of silver will be ............ $hrs$.

How much charge in coulombs is required for the reduction of one mole of $Al^{3+}$ to $Al$?