Question Detail

CHM 101 CHM 101 Past Questions Objective Question
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Question

For the equilibrium: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g); ΔH = -198 kJ mol⁻¹. Which of the following changes will decrease the proportion of SO₃ at equilibrium?
Options
A Increasing pressure at constant temperature
B Increasing temperature at constant pressure
Correct Answer
C Adding a catalyst
D Decreasing temperature at constant pressure
Correct Answer

Option B is the correct answer.

Detailed Explanation

The reaction is exothermic (ΔH negative). Increasing temperature favors the endothermic reverse reaction, decreasing SO₃. Pressure favors the side with fewer gas moles (forward, 3→2), so increasing pressure increases SO₃.

Hint

Apply Le Chatelier's principle: treat heat as a product for exothermic reactions.

Question Info

Course: CHM 101
Topic: CHM 101 Past Questions
Type: Objective
Difficulty: Not specified
Question 1410 of 1872
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