Correct Answer: Option D

Explanation

For a diatomic divalent element like oxygen, the following reaction takes place:

              2H\(_2\)0  →  O\(_2\)  +  4H\(^+\) +  4e\(^-\)

⇒  4e\(^-\) are transferred to liberate 1 mole of O\(_2\)

So, to calculate the volume of O\(_2\)

4 Faradays (4 x 96,500) of electricity to produce 22.4 dm\(^3\) of O\(_2\) at S.T.P

    4 X 96,500 C = 22.4 dm\(^3\)

      9650 C  =  x dm\(^3\)

    x = \(\frac{9650 X 22.4}{ 4 X  96,500}\)

    x = 0.56dm\(^3\)

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