Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10 \ mA$ current. The time required to liberate $0.01 \ mol$ of $H_2$ gas at the cathode is $(1 \ F = 96500 \ C \ mol^{-1})$

If the electrochemical equivalent of a substance is $0.0006735 \ g/C$,what is its equivalent weight?

What is achieved by Faraday using the principles of electrolysis?

When $96500 \ C$ of electricity is passed through a copper sulphate solution,the amount of copper deposited will be ............... $mol$.

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?

An electrolytic cell contains a solution of $Ag_{2}SO_{4}$ and has platinum electrodes. $A$ current is passed until $1.6 \ g$ of $O_{2}$ is liberated at the anode. The amount of silver deposited at the cathode would be ............ $g$.