One litre solution of $MgCl_2$ is electrolyzed completely by passing a current of $1 \ A$ for $16 \ min \ 5 \ sec$. The original concentration of $MgCl_2$ solution was (Atomic mass of $Mg = 24$)

What will be the weight of $Al$ deposited at the cathode when $0.5 \ F$ of electricity is passed through an aqueous solution of $AlCl_3$ (in $g$)? (Atomic mass of $Al = 27$)

On passing $1 \ F$ of electricity through electrolytic cells containing $Ag^{+}$,$Ni^{2+}$,and $Cr^{3+}$ ions,the mass of $Ag$ $(At. wt. = 108)$,$Ni$ $(At. wt. = 59)$,and $Cr$ $(At. wt. = 52)$ deposited is:

$A$ solution of $Ni(NO_3)_2$ is electrolysed between platinum electrodes using $0.1 \ F$ electricity. How many moles of $Ni$ will be deposited at the cathode?

$A$ current is passed for $2 \, \text{hours}$ through an acidic solution,liberating $11.2 \, L$ of oxygen at $NTP$ at the anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same duration? .......... $g$

Clarify the stoichiometry of the reactions occurring on the electrodes of an electrolytic cell and its relationship with the quantity of electricity.