For depositing $1 \ g$ of $Cu$ in a copper voltameter by passing $2 \ A$ of current,the time required will be (For copper $Z = 0.00033 \ g/C$)

The density of $Cu$ is $8.94 \, g \, cm^{-3}$. The quantity of electricity needed to plate an area $10 \, cm \times 10 \, cm$ to a thickness of $10^{-2} \, cm$ using $CuSO_4$ solution would be,if atomic mass of $Cu$ is $63.5$ .................. $C$

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

What is the number of faraday required to produce $0.18 \ g$ aluminium at cathode during electrolysis of molten $AlCl_3$ (in $F$)? (Molar mass of $Al = 27 \ g \ mol^{-1}$)

How many coulombs of electricity is required to produce $1 \ g$ of $Na$ metal from its ions (in $C$)? (Atomic mass of $Na = 23 \ g/mol$)

Solutions of $Hg_{2}(ClO_{4})_{2}$,$Hg(ClO_{4})_{2}$,$CuSO_{4}$,and $AgNO_{3}$ are connected in series. If a current of $2.58 \ A$ is passed for $1 \ hour$,calculate the moles of metal liberated from each solution at the cathode.