The relation between Faraday constant $(F)$,chemical equivalent $(E)$,and electrochemical equivalent $(Z)$ is

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 $KClO_{3} = 122 \ g \ mol^{-1}$)

The unit of electrochemical equivalent is

When a current of $0.1 \, A$ is passed through $200 \, mL$ of a $0.1 \, N$ $AgNO_3$ solution,silver is deposited. How much time in $sec$ is required to remove half of the silver from the solution?

$5 \ A$ current is passed through $AgNO_3$ solution for $193 \ s$. If $0.972 \ g$ of $Ag$ is deposited,calculate the current efficiency (cell capacity) of the electrolytic cell. $[Ag = 108 \ u]$ (in $\%$)

Calculate the mass of a divalent metal produced at the cathode by passing $5 \ A$ current through its salt solution for $100 \ minutes$. (Molar mass of metal $= x \ g/mol$)