How many electrons would be required to deposit $6.35 \ g$ of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate? (Atomic mass of copper $= 63.5 \ u$,$N_A =$ Avogadro's constant)

What is the number of faraday required to produce $0.18 \ g$ aluminium at cathode during electrolysis of molten $AlCl_3$ (in $F$)? (Molar mass of $Al = 27 \ g \ mol^{-1}$)

$A$ current of $16\, A$ flows through molten $NaCl$ for $10\, min$. The amount of metallic sodium that appears at the negative electrode would be ............ $g$.

Calculate the amount of electricity required in coulombs to convert $0.08 \ mol$ of $MnO_4^{-}$ to $Mn^{2+}$. (in $C$)

From the solution of which of the following will one Faraday of electricity liberate one gram atom of metal?

$A$ constant current was passed through a solution of $AuCl_4^-$ ion between gold electrodes. After a period of $10.0 \ \text{minutes}$,the increase in mass of cathode was $1.314 \ \text{g}$. The total charge passed through the solution is . . . . . . $\times 10^{-2} \ \text{F}$. (Given atomic mass of $Au = 197$)