The amount of charge in $F$ (Faraday) required to obtain one mole of iron from $Fe_{3}O_{4}$ is (Nearest Integer).

Which of the following aqueous solutions will result in the maximum number of moles of metal deposited on passing the same amount of charge?

When $0.1 \ mol$ of $MnO_4^{2-}$ is oxidized,the quantity of electricity required to completely oxidize $MnO_4^{2-}$ to $MnO_4^-$ is $........ \ C$.

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 $.2$)

When $10 \,A$ current is passed for $80 \,min$, the volume of hydrogen gas liberated at $STP$ is: (in $\,L$)

$A$ certain current liberated $0.504 \ g$ of hydrogen in $2 \ hours$. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution?