The electrochemical equivalent $Z$ of any element can be obtained by multiplying the electrochemical equivalent of hydrogen with

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

How many Faraday of electricity is required to produce $5 \ g$ of magnesium from magnesium chloride (in $F$)? (Molar mass $Mg = 24 \ g \ mol^{-1}$)

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 :-

The ratio of weights of hydrogen gas liberated and magnesium deposited by passing the same amount of electricity from aqueous $H_2SO_4$ and fused $MgSO_4$ are :

$38.6 \ A$ of current is passed for $100 \ s$ through an aqueous $CuSO_4$ solution using platinum electrodes. The mass of copper deposited from the solution and the volume of gas liberated at $STP$ are respectively (molar mass of $Cu = 63.54 \ g \ mol^{-1}$)