The time required (in hours) to reduce $3 \ mol$ of $Fe^{3+}$ ions to $Fe^{2+}$ ions with $2.0 \ A$ of current is $\left(1 \ F = 96500 \ C \ mol^{-1}\right)$ (in $.2$)

From the solution of which of the following will one Faraday of electricity liberate one gram atom of metal?

In the electrolysis of $CuCl_2$,a current of $2.0 \ A$ is passed through the solution at $1 \ bar$ pressure and $300 \ K$ temperature for $1 \ hour$. Calculate the amount of product obtained at the anode and cathode. $[Cu = 63.5, \ Cl = 35.5, \ R = 0.08314 \ L \ bar \ K^{-1} \ mol^{-1}]$

Potassium chlorate is prepared by the electrolysis of $KCl$ in basic solution:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
If only $60\%$ of the current is utilized in the reaction,the time (rounded to the nearest hour) required to produce $10 \ g$ of $KClO_{3}$ using a current of $2 \ A$ is:
(Given: $F = 96,500 \ C \ mol^{-1}$,molar mass of $KClO_{3} = 122 \ g \ mol^{-1}$)

The chemical equivalents of copper and silver are $32$ and $108$ respectively. When copper and silver voltameters are connected in series and electric current is passed through for some time,$1.6 \ g$ of copper is deposited. Then,the mass of silver deposited will be .......... $g$.

How much electricity is required to deposit $108 \ g$ of silver from a silver nitrate solution?