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 ..... .

Two electrolytic cells containing molten solutions of nickel chloride and aluminium chloride are connected in series. If the same amount of electric current is passed through them,what will be the weight of nickel obtained when $18 \ g$ of aluminium is obtained (in $g$)? $[Al = 27 \ g/mol, Ni = 58.5 \ g/mol]$

One ampere of current is passed for $9650 \ s$ through molten $AlCl_3$. What is the weight in grams of $Al$ deposited at the cathode? (Atomic weight of $Al = 27$)

Two electrolytic cells,one containing acidified ferrous chloride $(FeCl_2)$ and the other containing acidic ferric chloride $(FeCl_3)$,are connected in series. When an electric current is passed through the cells,what is the ratio of iron deposited at the cathodes in the two cells?

How much electricity in terms of Faraday is required to produce:
$(i)$ $20.0 \, g$ of $Ca$ from molten $CaCl_2$?
$(ii)$ $40.0 \, g$ of $Al$ from molten $Al_2O_3$?

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 $C$)