To deposit one $gm$ equivalent of an element at an electrode,the quantity of electricity needed is

The time required to remove electrolytically one fourth of $Ag^+$ from $0.2 \ L$ of $0.1 \ M \ AgCl$ solution by a current of $0.1 \ A$ is approximately $.......... \ min$.

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?

Faraday's laws of electrolysis state that the mass deposited on an electrode is proportional to:

What mass of silver (Atomic mass = $108 \text{ g/mol}$) is deposited by a quantity of electricity that displaces $5600 \text{ mL}$ of $O_2$ gas at $STP$ (in $\text{ g}$)?

When a copper voltameter is connected with a battery of $e.m.f.$ $12 \ V$,$2 \ g$ of copper is deposited in $30 \ minutes$. If the same voltameter is connected across a $6 \ V$ battery,then the mass of copper deposited in $45 \ minutes$ would be ............. $g$.