$A$ solution of $CuSO_4$ is electrolysed for $10 \,min$ with a current of $1.5 \,A$. What is the mass of copper deposited at the cathode (in $,g$)?

Calculate the time required in seconds to deposit $6.35 \ g$ of copper from its salt solution by passing a $5 \ A$ current. [Molar mass of $Cu = 63.5 \ g \ mol^{-1}$]

The mass deposited at an electrode during electrolysis is directly proportional to which of the following?

When $0.1 \ mol$ of $MnO_4^{2-}$ is oxidized,the quantity of electricity required to completely oxidize $MnO_4^{2-}$ to $MnO_4^-$ is $........ \ C$.

Equal amounts of electricity are passed through two separate electrolytic cells containing nickel nitrate $[Ni(NO_3)_2]$ and chromium nitrate $[Cr(NO_3)_3]$. If $0.3 \ g$ of nickel is deposited in the first cell,how much chromium will be deposited in the second cell? (Atomic mass of $Ni = 59$,Atomic mass of $Cr = 52$)

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 $63.5$ .................. $C$