The electrochemical equivalent of magnesium is $0.126 \ mg/C$. $A$ current of $5 \ A$ is passed in a suitable solution for $1 \ hour$. The mass of magnesium deposited will be ........... $gm$.

$108 \ g$ of silver (molar mass $108 \ g \ mol^{-1}$) is deposited at the cathode from $AgNO_3(aq)$ solution by a certain quantity of electricity. The volume (in $L$) of oxygen gas produced at $273 \ K$ and $1 \ bar$ pressure from water by the same quantity of electricity is ............. $L$.

When $1 \ C$ of charge is passed through an electrolyte solution,the mass deposited is equal to:

When the same quantity of electricity is passed through aqueous solutions of $AgNO_3$ and $CuSO_4$,if the number of atoms of $Ag$ and $Cu$ deposited are $x$ and $y$ respectively,then determine the correct relationship.

The number of Faradays required to completely deposit magnesium from $1 \ L$ of $0.1 \ M$ $MgCl_2$ aqueous solution is

The electrochemical equivalent of a metal is $x \ g \ C^{-1}$. The equivalent weight of the metal is: