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

Charge required for reduction of $0.01 \ mol$ of $MnO_4^-$ in neutral medium is ............ $C$.

How much charge in Coulombs is required for the oxidation of $1 \ mol$ of $H_2O$ to $O_2$?

$A$ certain quantity of electricity is passed through an aqueous solution of $AgNO_3$ and a cupric salt solution connected in series. The amount of $Ag$ deposited is $1.08 \ g$. The amount of copper deposited is ............. $g$ (atomic weight of $Cu = 63.5$; $Ag = 108$).

In the electrolysis of $CuCl_2$,a current of $2.0 \ A$ is passed through the solution at $1 \ bar$ pressure and $300 \ K$ temperature for $1 \ hour$. Calculate the amount of product obtained at the anode and cathode. $[Cu = 63.5, \ Cl = 35.5, \ R = 0.08314 \ L \ bar \ K^{-1} \ mol^{-1}]$

The quantity of charge required to obtain $1 \, mole$ of aluminium from $Al_2O_3$ is ............ $F$.