$A$ 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 $Cu = 63.5$) $(1 \ F = 96500 \ C)$

If a steady current of $4 \, A$ is maintained for $40 \, min$,depositing $4.5 \, g$ of zinc at the cathode,then the electrochemical equivalent $(Z)$ will be:

When $1 \ C$ of charge is passed through an electrolyte solution,the mass deposited is equal to:

Potassium chlorate is prepared by the electrolysis of $KCl$ in basic solution:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
If only $60\%$ of the current is utilized in the reaction,the time (rounded to the nearest hour) required to produce $10 \ g$ of $KClO_{3}$ using a current of $2 \ A$ is:
(Given: $F = 96,500 \ C \ mol^{-1}$,molar mass of $KClO_{3} = 122 \ g \ mol^{-1}$)

One litre solution of $MgCl_2$ is electrolyzed completely by passing a current of $1 \ A$ for $16 \ min \ 5 \ sec$. The original concentration of $MgCl_2$ solution was (Atomic mass of $Mg = 24$)

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 $Cr = 52$)