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 amount of substance liberated on electrodes during electrolysis when $1 \ C$ of electricity is passed,is

In the Hall process,aluminium is produced by the electrolysis of molten $Al_2O_3$. How many seconds would it take to produce enough aluminium by the Hall process to make a case of $24$ cans of aluminium soft-drink,if each can uses $5.0 \ g$ of $Al$,a current of $9650 \ A$ is employed,and the current efficiency of the cell is $90.0 \ \%$?

For the given reaction how much quantity of electricity in Coulomb is required? $\frac{2}{3} Al_2O_3 \rightarrow \frac{4}{3} Al + O_2$

$Al_2O_3$ is reduced by electrolysis at low potentials and high currents. If $4.0 \times 10^4$ amperes of current is passed through molten $Al_2O_3$ for $6$ hours,what mass of aluminium is produced? (Assume $100\%$ current efficiency,at. mass of $Al = 27 \ g \ mol^{-1}$).

Three electrolytic cells $A, B, C$ containing solutions of $ZnSO_{4}, AgNO_{3}$ and $CuSO_{4}$ respectively are connected in series. $A$ steady current of $1.5 \ A$ was passed through them until $1.45 \ g$ of silver deposited at the cathode of cell $B$. How long did the current flow? What mass of copper and zinc were deposited?