$A$ current of $0.4 \ A$ is passed through excess of molten $MgCl_2$ for $9.65 \times 10^4 \ sec$. The mass of $Mg$ deposited at the cathode is .............. $gm$

How many coulombs of electricity is required to produce $1 \ g$ of $Na$ metal from its ions (in $C$)? (Atomic mass of $Na = 23 \ g/mol$)

$1$ mole of electrons corresponds to how much Faraday,how much Coulomb,and how many electrons?

Two electrolytic cells containing molten solutions of nickel chloride and aluminium chloride are connected in series. If the same amount of electric current is passed through them,what will be the weight of nickel obtained when $18 \ g$ of aluminium is obtained (in $g$)? $[Al = 27 \ g/mol, Ni = 58.5 \ g/mol]$

Calculate the current in ampere required to deposit $4.8 \ g$ of $Cu$ from its salt solution in $30 \ minutes$. $\left[ \text{Molar mass of } Cu = 63.5 \ g \ mol^{-1} \right]$ (in $A$)

How many faradays of electricity is required to produce $4.8 \ g$ of $Mg$ at cathode in the electrolysis of molten $MgCl_2$ (in $F$)? (Molar mass of $Mg = 24 \ g/mol$)