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

In the electrolysis of an aqueous $NiI_2$ solution using $Ni$ electrodes,what happens to the mass of the cathode upon passing $1$ equivalent of charge? (Given: atomic mass of $Ni = 59$)

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

Calculate the current in ampere required to deposit $4.8 \ g$ of $Cu$ from its salt solution in $30 \ minutes$. $\left[ \text{Molar mass of } Cu = 63.5 \ g \ mol^{-1} \right]$ (in $A$)

The amount of ion discharged during electrolysis is not directly proportional to

When $0.04$ faraday of electricity is passed through a solution of $CaSO_4$,then the weight of $Ca^{2+}$ metal deposited at the cathode is $.............$ $g$.