Le Chatelier's Principle
In the Haber process, N₂(g) + 3H₂(g) ⇌ 2NH₃(g); ΔH = −92.4 kJ mol⁻¹, which of the following changes will shift the equilibrium towards the formation of ammonia?
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About This Question
- Subject
- chemistry
- Chapter
- equilibrium
- Topic
- le chatelier's principle
- Difficulty
- Easy
- Year
- 2025
Solution
Correct Answer:
Increasing the pressure of the system
Le Chatelier's principle states that a system at equilibrium will shift to counteract any imposed change. The forward reaction reduces the total number of moles of gas from 4 (1 + 3) to 2. Increasing pressure favours the side with fewer moles of gas, so the equilibrium shifts to the right, producing more NH₃. Increasing temperature would favour the endothermic (reverse) direction since the forward reaction is exothermic. Removing N₂ shifts equilibrium to the left. Adding an inert gas at constant pressure does not change the partial pressures of reactants or products, so it has no effect on the position of equilibrium.
This easy difficulty chemistry question is from the chapter equilibrium, covering the topic of le chatelier's principle. It appeared in the 2025 exam.
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