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

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 $C$)

Two different electrolytic cells filled with molten $Cu(NO_3)_2$ and molten $Al(NO_3)_3$ respectively are connected in series. When electricity is passed,$2.7 \ g$ of $Al$ is deposited on the electrode. Calculate the weight of $Cu$ deposited on the cathode. [Atomic mass: $Cu = 63.5$,$Al = 27.0 \ g \ mol^{-1}$] (in $g$)

An acidic solution of dichromate is electrolyzed for $8 \ min$ using $2 \ A$ current. As per the following equation: $Cr_{2}O_{7}^{2-} + 14H^{+} + 6e^{-} \rightarrow 2Cr^{3+} + 7H_{2}O$. The amount of $Cr^{3+}$ obtained was $0.104 \ g$. The efficiency of the process (in $\%$) is (Take: $F = 96000 \ C$,At. mass of chromium $= 52$)

$108 \ g$ of silver (molar mass $108 \ g \ mol^{-1}$) is deposited at the cathode from $AgNO_3(aq)$ solution by a certain quantity of electricity. The volume (in $L$) of oxygen gas produced at $273 \ K$ and $1 \ bar$ pressure from water by the same quantity of electricity is ............. $L$.

One Faraday of electricity liberates $x \times 10^{-1}$ gram atom of copper from copper sulphate,$x$ is . . . . . . .