Faraday's $2^{nd}$ law of electrolysis states that the mass of a substance deposited at an electrode is directly proportional to its:

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

The amount of metal deposited at the cathode on passing an electric current of $0.75 \ A$ in an aqueous ferric sulphate solution for $30 \ min$ will be - ........... $g$ (atomic weight of $Fe = 56$).

How many electrons flow when a current of $5 \ A$ is passed through a cell for $200 \ s$?

In two separate experiments,the same quantity of electricity was passed through silver and gold solutions. The amounts of $Ag$ and $Au$ deposited are $2.15 \ g$ and $1.31 \ g$,respectively. The valency of gold is [Atomic mass of $Ag = 107.9$; $Au = 197$].

To gain $1 \ mole$ $Mg$ from $Mg^{2+}$ and $1 \ mole$ $Al$ from $Al^{3+}$,how many Coulombs of electricity are required respectively?