When an electric current is passed through acidified water, $112mL$ of hydrogen gas N.T.P was collected at the cathode in $965$ seconds. The current asset, ampere, is:

The amount of energy or charge (Q) transmitted is exactly proportional to the mass of the material (m) deposited or freed at any electrode. In mathematics, it may be expressed as $m=Z\times I\times t$

Where m is the mass of the deposition, I is the current that goes through it, t is the amount of time that the current was passed, and Z is the electrochemical equivalent. Therefore, depositing the same amount of a metal will be the same and will only rely on the electron taking part in the reaction. Alternately, we may claim that the quantity of electrons consumed in the deposition reaction directly relates to the amount of power required.

Moles of hydrogen $=\frac{112}{22400}=\frac{1}{200}=0.005$
As required charge is directly proportional to the moles of the hydrogen gas,
Charge required will be $=0.005\times 96500=482.5$
Hence we can write
$\Rightarrow I\times t=482.5$
$\Rightarrow I\times 96500=482.5$
$\Rightarrow I=\frac{482.5}{96500}$
$\Rightarrow I=0.5\text{ Ampere }$

Hence, option c is correct.