What is the number of moles of electrons passed when a current of $2 \text{ A}$ flows through an electrolyte solution for $10 \text{ minutes}$?

The number of Faraday required to generate $1$ $g$ $atom$ of $Mg$ from $MgCl_2$ is :-

When $3 \ F$ of electricity is passed through an aqueous solution of iron $(II)$ bromide,what is the mass of iron metal deposited at the cathode in $g$?

The unit of electrochemical equivalent is

$Assertion (A)$: $A$ current of $96.5 \ A$ is passed into aqueous $AgNO_3$ solution for $100 \ s$. The weight of silver deposited is $10.8 \ g$ (At. wt. of $Ag = 108$).
$Reason (R)$: The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.
The correct answer is :

The amount of metal deposited at the cathode on passing an electric current of $0.75 \ A$ in an aqueous ferric sulphate solution for $30 \ min$ will be - ........... $g$ (atomic weight of $Fe = 56$).