What mass of $Mg$ is produced during electrolysis of molten $MgCl_2$ by passing $2 \ A$ current for $482.5 \ s$ (in $g$)? $(Molar \ mass \ Mg = 24 \ g \ mol^{-1})$

If $1$ mole of electrons is passed through the solutions of $AlCl_3$,$AgNO_3$,and $MgSO_4$,in what ratio will $Al$,$Ag$,and $Mg$ be deposited at the electrodes?

The atomic weights of silver and copper are $108$ and $64$ respectively. $A$ silver voltameter and a copper voltameter are connected in series,and when current is passed,$10.8 \ g$ of silver is deposited. The mass of copper deposited will be ............. $g$.

Calculate the quantity of electricity required to produce $0.42 \ g$ of $Ag$ at the cathode during the electrolysis of an $AgNO_3$ solution. (Molar mass of $Ag = 108 \ g \ mol^{-1}$) (in $C$)

The chemical equivalent of silver is $108$. If the current in a silver voltameter is $2 \ A$,the time required to deposit $27 \ g$ of silver will be ............ $hrs$.

To complete the precipitation of $Ag$ from $400 \ mL$ of $0.04 \ M$ $AgNO_3$ solution,how long should a $4.8 \ A$ current be passed?