The time taken for effusion of 32 mL of oxygen will be the same as the time taken for effusion under identical conditions of:

To determine the gas that takes the same time for effusion as 32 mL of Oxygen (O₂), we use Graham's Law of Effusion. According to the law, the time taken for effusion is proportional to the square root of the molar mass of the gas. For the time to remain the same, the volume of effusing gas must adjust based on its molar mass.

Given Data

• Molar mass of O₂: 32 g/mol
• Volume of O₂: 32 mL

Step 2: Formula and Calculations

The equivalent volume for other gases is calculated using the formula:

V₂ = V₁ × √(M₁ / M₂)

• V₁: Volume of O₂ (32 mL)
• M₁: Molar mass of O₂ (32 g/mol)
• M₂: Molar mass of the other gas

Calculations for Each Gas

• Hydrogen (H₂):
  Molar mass = 2 g/mol
  V₂ = 32 × √(32 / 2) = 32 × 4 = 128 mL
• Nitrogen (N₂):
  Molar mass = 28 g/mol
  V₂ = 32 × √(32 / 28) = 32 × 1.07 ≈ 34.24 mL
• Carbon Dioxide (CO₂):
  Molar mass = 44 g/mol
  V₂ = 32 × √(32 / 44) = 32 × 0.85 ≈ 27.3 mL
• Sulfur Dioxide (SO₂):
  Molar mass = 64 g/mol
  V₂ = 32 × √(32 / 64) = 32 × 0.5 = 16 mL

Correct Answer: (C) 27.3 mL of CO₂