The volume of gases evolved when dil H₂SO₄ electrolyzed using 2F at STP is

• (A) 22.4L
• (B) 11.2L
• (C) 33.6L
• (D) 44.8L

To determine the volume of gases evolved when dilute sulfuric acid (H₂SO₄) is electrolyzed using 2 Faradays (F) at standard temperature and pressure (STP), we can use Faraday's laws of electrolysis.

Understanding Electrolysis of H₂SO₄

During the electrolysis of dilute sulfuric acid, water is split into hydrogen and oxygen gases. The overall reaction can be summarized as:

• 2 H₂O(l) → 2 H₂(g) + O₂(g)

Calculating Gas Volume

According to Faraday's laws, 1 Faraday can produce 1 mole of gas at STP. Since we are using 2 Faradays, we can calculate the moles of gases produced:

• 2 F → 1 mole of H₂ + 0.5 mole of O₂

Thus, the total moles of gas produced is:

• 1 mole of H₂ + 0.5 mole of O₂ = 1.5 moles of gas

Volume at STP

At STP, 1 mole of gas occupies 22.4 liters. Therefore, the total volume of gases can be calculated as follows:

• 1.5 moles × 22.4 L/mole = 33.6 L

Final Answer

The volume of gases evolved when dilute H₂SO₄ is electrolyzed using 2F at STP is 33.6 L. Thus, the correct option is (C) 33.6L.