What is the quantity of electricity in Faradays required to produce $8 \text{ g}$ of $Mg$ (molar mass = $24 \text{ g mol}^{-1}$) from $MgCl_2$ solution (in $\text{ F}$)?

When $9650 \ C$ of charge is passed through an $AgNO_3$ solution during the electrolysis process in an electroplating bath,what is the weight of silver deposited at the cathode in $g$?

What is the quantity of electricity (in Coulombs) required to deposit all the silver from $250 \text{ mL}$ of $1 \text{ M AgNO}_3$ solution?

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:

The quantity of electricity required to deposit $1$ gram-equivalent of a substance at an electrode is equal to .......

How many atoms of calcium will be deposited at the cathode when a current of $25 \ mA$ is passed through a $CaCl_2$ solution for $60 \ s$?