When $1 \ F$ of electricity is passed through acidulated water,the volume of $O_2$ evolved at $STP$ is ............. $dm^{3}$.

Solutions of $Hg_{2}(ClO_{4})_{2}$,$Hg(ClO_{4})_{2}$,$CuSO_{4}$,and $AgNO_{3}$ are connected in series. If a current of $2.58 \ A$ is passed for $1 \ hour$,calculate the moles of metal liberated from each solution at the cathode.

The quantity of electricity needed to liberate $0.5 \ g$ equivalent of an element is

How many moles of electrons (how many Faradays of electricity) are required to reduce $1 \ mol$ of $MnO_4^-$ to $MnO_2$?

What weight of copper will be deposited by passing $2$ Faradays of electricity through a cupric salt? (Atomic weight of $Cu = 63.5$)

Cells $A$ and $B$ contain aqueous solutions of ferrous chloride $(FeCl_2)$ and ferric chloride $(FeCl_3)$ respectively. If the same quantity of electricity is passed through both cells, what is the ratio of the mass of iron deposited in cell $A$ to that in cell $B$?