If in a voltaic cell $5 \ g$ of zinc is consumed,then how many ampere-hours are produced? (Given that the $E.C.E.$ of $Zn$ is $3.387 \times 10^{-7} \ kg/C$)

Potassium chlorate is prepared by electrolysis of $KCl$ in basic solution as shown by the following equation:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
$A$ current of $x \ A$ has to be passed for $10 \ h$ to produce $10.0 \ g$ of potassium chlorate. The value of $x$ is $.......$ (Nearest integer).
(Molar mass of $KClO_{3} = 122.6 \ g \ mol^{-1}, F = 96500 \ C \ mol^{-1}$)

On passing $3 \ A$ of electricity for $50 \ minutes$,$1.8 \ g$ of metal deposits. The equivalent mass of the metal is:

For electroplating,$1.5 \ A$ current is passed for $250 \ s$ through $250 \ mL$ of $0.15 \ M$ solution of $MSO_4$. Only $85 \ \%$ of the current was utilised for electrolysis. The molarity of $MSO_4$ solution after electrolysis is closest to $.......$ [Assume that the volume of the solution remained constant] (in $M$)

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

Find the number of faradays of electricity required to produce $45 \ g$ of $Al$ from molten $Al_2O_3$. (in $F$)