Question

During electrolysis of H₂SO₄ (aq) with high charge density, H₂S₂O₈ formed as by product. in such electrolysis 22.4 L H2( g) and 8.4 L O₂( g) liberated at 1 atm and 273 K at electrode. The moles of H₂S₂O₈ formed is :

A. 0.25
B. 0.50
C. 0.75
D. 1.00

Answer 1

During electrolysis of H₂SO₄ (aq) with high charge density, H₂S₂O₈ is formed as a byproduct. The moles of H₂S₂O₈ formed is 0.50. The correct answer is option B.

Step-by-step explanation:

The electrolysis of H₂SO₄ (aq) with high charge density can result in the formation of H₂S₂O₈ as a byproduct. In this case, 22.4 L of H2 gas and 8.4 L of O2 gas were liberated at 1 atm and 273 K at the electrode. To find the moles of H₂S₂O₈ formed, we need to use the stoichiometry of the reaction. From the balanced equation:

2H₂O(1) → O2(g) + 2H2(g)

We can see that the ratio of H₂O to H₂S₂O₈ is 2:1. Therefore, the moles of H₂S₂O₈ formed can be calculated as follows:

moles of H₂S₂O₈ = moles of H₂O / 2 = (22.4 L H2 / 22.4 L/mol) / 2 = 0.5 moles

Therefore, the moles of H₂S₂O₈ formed is 0.50 moles (option B).