$A$ solution of $CuSO_4$ is electrolysed using a current of $1.5 \ A$ for $10 \ minutes$. What mass of $Cu$ is deposited at the cathode (in $g$)? (Atomic mass of $Cu = 63.7$)

$A$ solution of aluminium chloride is electrolysed for $30$ minutes using a current of $2 \ A$. The amount of the aluminium deposited at the cathode is $.................$
[Given : molar mass of aluminium and chlorine are $27 \ g \ mol^{-1}$ and $35.5 \ g \ mol^{-1}$ respectively,Faraday constant $= 96500 \ C \ mol^{-1}$]. (in $g$)

For the reaction $Al^{3+} + 3e^{-} \rightarrow Al$ (atomic mass of $Al = 27 \ g \ mol^{-1}$),calculate the quantity of electricity in coulombs required to produce $5.12 \ kg$ of $Al$.

Calculate the mass of $Ca$ deposited at the cathode by passing $0.8 \ A$ current through molten $CaCl_2$ for $60 \ minutes$. [Molar mass of $Ca = 40 \ g \ mol^{-1}$] (in $g$)

Two electrolytic cells are connected in series containing $CuSO_4$ solution and molten $AlCl_3$. If in electrolysis $0.4$ moles of $Cu$ are deposited on the cathode of the first cell,the number of moles of $Al$ deposited on the cathode of the second cell is: (in $moles$)

In the electrolysis of an aqueous $Ni(NO_3)_2$ solution using $Ni$ electrodes,upon passing $1$ equivalent of charge,the mass of the cathode $(Ni = 59)$ changes by: