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\(^3\)