When a current of $9.65 \ A$ is passed for $10 \ \text{minutes}$,$3.0 \ g$ of metal is deposited. What is the equivalent weight of the metal?

What weight of copper will be deposited by passing $2$ Faradays of electricity through a cupric salt? (Atomic weight of $Cu = 63.5$)

From which solution $2 \ F$ electrical charge will deposit $1 \ g$ atomic weight at cathode?

Three voltameters containing aqueous solutions of $H_{2}SO_{4}$,$CuSO_{4}$,and $AgNO_{3}$ are connected in series as shown in the figure. $A$ current was passed for $10 \ hours$. $10.8 \ g$ of $Ag$ was deposited at the cathode in the $(III)$ electrolytic cell during electrolysis,given that the current efficiency is $50 \%$. If $Z_{1}$,$Z_{2}$,and $Z_{3}$ are the electrochemical equivalents for the formation of $H_{2}$,$Cu$,and $Ag$ respectively,then the ratio $Z_{1} : Z_{2} : Z_{3}$ is:

Salts of $A$ (atomic weight $8$),$B$ (atomic weight $18$) and $C$ (atomic weight $50$) were electrolysed under identical conditions using the same quantity of electricity. It was found that $2.4 \ g$ of $A$ was deposited,the weight of $B$ and $C$ deposited are $1.8 \ g$ and $7.5 \ g$ respectively. The valences of $A$,$B$ and $C$ are,respectively,

The number of Faraday required to generate $1$ $g$ $atom$ of $Mg$ from $MgCl_2$ is :-