$A$ current of strength $2.5 \ A$ was passed through $CuSO_4$ solution for $6 \ \text{minutes} \ 26 \ \text{seconds}$. The amount of copper deposited is .............. $g$ (Atomic weight of $Cu = 63.5$) $(1 \ F = 96500 \ C)$

Calculate the amount of electricity required in coulombs to convert $0.08 \ mol$ of $MnO_4^{-}$ to $Mn^{2+}$. (in $C$)

In the electrolysis of acidulated water,it is desired to obtain $1.12 \ cc$ of hydrogen gas per second at $STP$ conditions. The current to be passed is: (in $A$)

$CuSO_4$ solution is electrolysed for $15 \ minutes$ to deposit $0.4725 \ g$ of copper at the cathode. The current in amperes required is (Faraday $= 96,500 \ C \ mol^{-1}$,atomic weight of copper $= 63$)

Copper sulphate solution is electrolysed between two platinum electrodes. $A$ current is passed until $1.6 \ g$ of oxygen is liberated at the anode. The amount of copper deposited at the cathode during the same period is .............. $g$ [At. mass of $Cu = 63.6$]

$A$ metal plate of dimension $(1 \times 2 \ cm^2)$ has to be coated on both sides by $Cu$ metal. How long does it take to deposit $Cu$ of $0.01 \ cm$ thickness,if $1.5 \ A$ current is used (in $s$)? [Electrochemical equivalence of $Cu$ is $0.0003 \ g/C$ and the density of $Cu$ is $9 \ g/cm^3$]