In the electrolysis of $AgNO_3$,the mass of $Ag$ deposited is plotted against the charge. Slope of the line gives

$2.644 \ g$ of metal $(M)$ was deposited when $8040 \ C$ of electricity was passed through molten $MF_2$ salt. What is the atomic mass of $M$ $(F = 96500 \ C \ mol^{-1})$ (in $u$)?

Copper is to be electrodeposited on a nickel block of $(20 \times 5) \ cm^2$ area by using $CuSO_4$ as electrolyte. How much quantity of electricity is needed to deposit a $3.6 \ \mu m$ layer of copper (in $C$)? [Atomic weight of $Cu = 63.5 \ g \ mol^{-1}$,Density of $Cu = 8.9 \ g/cm^3$]

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

In the process of electroplating,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ min$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ s$ will be

Three faradays of electricity were passed through an aqueous solution of iron $(II)$ bromide. The weight of iron metal (atomic weight $= 56$) deposited at the cathode (in $g$) is