The amount of current in Faraday required for the reduction of $1 \ mol$ of $Cr_{2}O_{7}^{2-}$ ions to $Cr^{3+}$ is, (in $F$)

When the same quantity of electricity is passed through the aqueous solutions of the given electrolytes for the same amount of time,which metal will be deposited in maximum amount on the cathode?

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 $C$)

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

The amount of charge required to liberate $11.5 \ g$ of sodium is .....

If current $(I)$ of an electrolytic cell is doubled and time $(t)$ for electrolysis is halved,then the $\frac{\text{mass}}{\text{eq. wt.}}$ ratio becomes :-