This deep dive covers Example: The Haber Process within Equilibrium (HT) for GCSE Chemistry. Revise Equilibrium (HT) in Rates of Reaction for GCSE Chemistry with 20 exam-style questions and 15 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 6 of 14 in this topic. Use this deep dive to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 6 of 14
Practice
20 questions
Recall
15 flashcards
🏭 Example: The Haber Process
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) ΔH = −92 kJ/mol (forward is exothermic)
Analysing conditions using Le Chatelier's Principle:
- Low temperature → favours exothermic forward reaction → more NH₃ BUT too slow (impractical)
- High pressure → favours fewer molecules (4 mol → 2 mol) → more NH₃ BUT very expensive equipment
- Compromise: 450°C, 200 atm, iron catalyst — balances yield, rate, and cost
This is a classic exam example: the industrial conditions are a compromise between equilibrium position (yield) and rate of reaction (economics). Higher temperature gives faster rate but shifts equilibrium left; lower temperature is better for yield but reaction is too slow.