The mass of ions deposited during a given interval of time in the process of electrolysis depends on

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 ..... .

When the same quantity of electricity is passed through solutions of different electrolytes connected in series,the amounts of substances deposited at the electrodes are in the ratio of their ...?

How much time is required for complete decomposition of $4 \, \text{moles}$ of water using $4 \, \text{A}$ current?

The same quantity of electricity was passed through solutions of salts of elements $X$,$Y$,and $Z$ with atomic masses $7$,$27$,and $48$ respectively. The masses of $X$,$Y$,and $Z$ deposited were $2.1 \ g$,$2.7 \ g$,and $7.2 \ g$ respectively. The valencies of $X$,$Y$,and $Z$ respectively are:

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