What is the number of moles of electrons passed when a current of $5 \ A$ is passed through a solution of $FeCl_3$ for $20 \ minutes$?

If a current of $5 \ A$ is passed through a zinc sulfate solution for $40 \ \text{minutes}$,what is the mass of zinc deposited at the cathode (in $g$)?

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

$18.4 \, A$ current is passed for $1$ hour and $42$ minutes through $CuSO_4$ solution using graphite electrodes at $298 \, K$ temperature and $1 \, bar$ pressure. If the cell efficiency is $75 \%$,calculate the mass of $Cu$ deposited and the volume of $O_2$ gas evolved at $STP$. $[Cu = 63.5 \, u, O = 16 \, u, R = 0.08314 \, L \, bar \, K^{-1} \, mol^{-1}]$

On passing $96500 \ C$ of charge through a $CuSO_4$ solution,the amount of copper liberated is:

The same quantity of electricity was passed through solutions of salts of elements $X$,$Y$,and $Z$ with atomic masses $7$,$27$,and $48$ respectively. The masses of $X$,$Y$,and $Z$ deposited were $2.1 \ g$,$2.7 \ g$,and $7.2 \ g$ respectively. The valencies of $X$,$Y$,and $Z$ respectively are: