Calculation of Current in Electrolysis of Acidulated Water

Given:
Volume of hydrogen obtained per second = 1.12 cc
Temperature and pressure conditions = S.T.P. (Standard Temperature and Pressure)

To find:
Current to be passed

Solution:
The volume of 1 mole of any gas at S.T.P. conditions = 22.4 L or 22400 cc
So, the volume of 1 mole of hydrogen at S.T.P. conditions = 22400 cc

Now, we can find the number of moles of hydrogen produced per second as follows:
1.12 cc of hydrogen is produced per second
So, the volume of hydrogen produced in 1 mole = 22400 cc
Therefore, the number of moles of hydrogen produced per second = (1.12/22400) moles

According to Faraday's laws of electrolysis,
The amount of substance produced at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.
The quantity of electricity is expressed in coulombs (C).
The amount of substance produced is expressed in moles.

So, we can find the quantity of electricity required to produce (1.12/22400) moles of hydrogen as follows:
1 mole of hydrogen requires 2 Faradays of electricity
Therefore, (1.12/22400) moles of hydrogen requires (2 x 1.12/22400) Faradays of electricity

We know that 1 Faraday of electricity = 96500 C
Therefore, (2 x 1.12/22400) Faradays of electricity = (2 x 1.12/22400 x 96500) C

Finally, we can find the current required to pass this quantity of electricity in 1 second as follows:
Current (I) = Quantity of electricity (Q) / Time (t)
I = [(2 x 1.12/22400 x 96500) C] / 1 s
I = 0.965 A

Therefore, the current to be passed in the electrolysis of acidulated water to obtain 1.12 cc of hydrogen per second under S.T.P. conditions is 0.965 A.

Hence, option (b) is the correct answer.