The required charge for one equivalent weight of silver deposited on cathode is

The amount of copper metal deposited at the cathode on passing an electric current of $500 \, mA$ for $20 \, minutes$ in a cupric chloride solution is ............ $g$.

To deposit $0.6354 \ g$ of copper by electrolysis of aqueous cupric sulphate solution,the amount of electricity required (in coulombs) is

Copper is to be electrodeposited on a nickel block of $(20 \times 5) \ cm^2$ area by using $CuSO_4$ as electrolyte. How much quantity of electricity is needed to deposit a $3.6 \ \mu m$ layer of copper (in $C$)? [Atomic weight of $Cu = 63.5 \ g \ mol^{-1}$,Density of $Cu = 8.9 \ g/cm^3$]

$A$ solution of $Ni(NO_3)_2$ is electrolysed between platinum electrodes using $0.1 \ F$ electricity. How many moles of $Ni$ will be deposited at the cathode?

One Faraday of electricity liberates $x \times 10^{-1}$ gram atom of copper from copper sulphate,$x$ is . . . . . . .