In the electrolysis of a fused salt,the weight of the deposit on an electrode will not depend on:

How long a current of $3 \, A$ has to be passed through a solution of $AgNO_3$ to coat a metal surface of $80 \, cm^2$ with $0.005 \, mm$ thick layer? Density of $Ag$ is $10.5 \, g/cm^3$. (Answer in $sec$)

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 $Cu = 8.9 \ g/cm^3$]

When a current of $10 \ A$ is passed through molten $AlCl_{3}$ for $1.608 \ minutes$,the mass of $Al$ deposited will be [Atomic mass of $Al = 27 \ g/mol$]:- (in $g$)

$4.5 \ g$ of aluminium (atomic mass $27 \ amu$) is deposited at the cathode from an $Al^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at $STP$ from $H^{+}$ ions in the solution by the same quantity of electric charge will be .............. $L$.

To deposit a silver layer of thickness $5 \times 10^{-3} \ cm$ on a surface area of $80 \ cm^2$ (density $= 10.5 \ g \ cm^{-3}$),a current of $3 \ A$ is passed through a silver nitrate solution for ......... $sec$.