How much electricity in terms of Faraday is required to reduce $2 \ mol$ of $MnO_4^{-}$ into $Mn^{2+}$?

Which is the weight of $Al$ deposited at cathode when $1 \ A$ current is passed through molten $AlCl_3$ for $9650 \ s$ (in $g$)?
(Atomic mass of $Al = 27$)

When $1 \ F$ (Faraday) of electricity is passed through an aqueous solution of $CuSO_4$,the amount of $Cu$ deposited is:

$5 \ A$ current is passed through a solution of zinc sulphate for $40 \ \text{minutes}$. Find the amount of zinc deposited at the cathode in $gm$.

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 $Al_2O_3$?

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 $g$)