The quantity of electricity required to deposit $1$ gram-equivalent of a substance at an electrode is equal to .......

Two different electrolytic cells filled with molten $Cu(NO_3)_2$ and molten $Al(NO_3)_3$ respectively are connected in series. When electricity is passed,$2.7 \ g$ of $Al$ is deposited on the electrode. Calculate the weight of $Cu$ deposited on the cathode. [Atomic mass: $Cu = 63.5$,$Al = 27.0 \ g \ mol^{-1}$] (in $g$)

The atomic weights of silver and copper are $108$ and $64$ respectively. $A$ silver voltameter and a copper voltameter are connected in series,and when current is passed,$10.8 \ g$ of silver is deposited. The mass of copper deposited will be ............. $g$.

Salts of $A$ (atomic weight $8$),$B$ (atomic weight $18$) and $C$ (atomic weight $50$) were electrolysed under identical conditions using the same quantity of electricity. It was found that $2.4 \ g$ of $A$ was deposited,the weight of $B$ and $C$ deposited are $1.8 \ g$ and $7.5 \ g$ respectively. The valences of $A$,$B$ and $C$ are,respectively,

$A$ steady current of $5 \, A$ is maintained for $45 \, min$. During this time,it deposits $4.572 \, g$ of zinc at the cathode of a voltameter. The $E.C.E.$ of zinc is:

The amount of substance deposited when a current of $1 \ A$ is passed for $1 \ s$ is equal to: