Le Chatelier's Principle (Higher Tier)
Part of Equilibrium (HT) — GCSE Chemistry
This higher tier covers Le Chatelier's Principle (Higher Tier) 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 4 of 13 in this topic. This section is most useful once the core foundation idea is secure, because it adds the detail that pushes answers higher.
Topic position
Section 4 of 13
Practice
20 questions
Recall
15 flashcards
🎓 Le Chatelier's Principle (Higher Tier)
"If a system at equilibrium is disturbed, it will shift in the direction that opposes the change."
Effect of changing CONDITIONS:
🌡️ TEMPERATURE
Increase temperature → equilibrium shifts in the ENDOTHERMIC direction (absorbs the extra heat)
Decrease temperature → equilibrium shifts in the EXOTHERMIC direction (releases heat to compensate)
System tries to "use up" or "release" the extra heat
🧪 CONCENTRATION
Increase concentration of a reactant → shifts to PRODUCTS (right)
Increase concentration of a product → shifts to REACTANTS (left)
System tries to "use up" the added substance
💨 PRESSURE (gases only)
Increase pressure → shifts to side with FEWER gas molecules
Decrease pressure → shifts to side with MORE gas molecules
System tries to reduce the change in pressure
What about catalysts?
Catalysts do NOT change equilibrium position — they just help reach equilibrium faster by speeding up BOTH forward and backward reactions equally.