The amount of charge required to liberate $9 \ g$ of aluminium (atomic weight = $27$ and valency = $3$) in the process of electrolysis is ......... $coulombs$ (Faraday's constant $= 96500 \ C \ mol^{-1}$)

When $1 \ C$ of charge is passed through an electrolyte solution,the mass deposited is equal to:

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 $Cu = 8.9 \ g/cm^3$]

Faraday's laws of electrolysis are related to

The current flowing in a copper voltameter is $3.2 \ A$. The number of copper ions $(Cu^{2+})$ deposited at the cathode per minute is

Which of the following aqueous solutions will result in the maximum number of moles of metal deposited on passing the same amount of charge?