Calculate the quantity of electricity required to produce $0.42 \ g$ of $Ag$ at the cathode during the electrolysis of an $AgNO_3$ solution. (Molar mass of $Ag = 108 \ g \ mol^{-1}$) (in $C$)

The negative $Zn$ pole of a Daniel cell,sending a constant current through a circuit,decreases in mass by $0.13 \ g$ in $30$ minutes. If the electrochemical equivalent of $Zn$ and $Cu$ are $32.5$ and $31.5$ respectively,the increase in the mass of the positive $Cu$ pole in this time is .............. $g$.

The number of moles of electrons required to deposit $36 \ g$ of $Al$ from an aqueous solution of $Al(NO_3)_3$ is (At. wt. of $Al = 27$)

Consider the following reaction:
$MnO_4^- + 8H^{+} + 5e^- \rightarrow Mn^{2+} + 4H_2O$,$E^\circ = 1.51 \ V$
The quantity of electricity required in Faraday to reduce five moles of $MnO_4^-$ is ..... .

How much time (in $sec$) is required to coat a metal surface of $80 \, cm^2$ with a $0.005 \, mm$ thick layer of silver from a silver nitrate solution using a current of $3 \, A$? (Density of silver $= 10.5 \, g \, cm^{-3}$)

One ampere of current is passed for $9650 \ s$ through molten $AlCl_3$. What is the weight in grams of $Al$ deposited at the cathode? (Atomic weight of $Al = 27$)