The mass of silver deposited when a charge of $241.25 \ C$ is passed through a solution of $AgNO_3$ is = .......

Three voltameters containing aqueous solutions of $H_2SO_4$,$CuSO_4$,and $AgNO_3$ are connected in series as shown. $A$ current was passed for $10 \ hours$. $10.8 \ g$ of $Ag$ was deposited at the cathode in the $(III)$ electrolytic cell during electrolysis. If the current efficiency is $50\%$,what is the magnitude of the current in amperes?

$A$ solution of copper sulphate is electrolysed for $10 \text{ minutes}$ with a current of $1.5 \text{ amperes}$. The mass of copper deposited at the cathode is:
(Given: Molar mass of $Cu = 63 \text{ g mol}^{-1}$; $1F = 96487 \text{ C mol}^{-1}$)

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

Which of the following represents the first law of Faraday?

From the solution of which of the following will one Faraday of electricity liberate one gram atom of metal?