How Le Chatelier's Principle Works
Part of Equilibrium (HT) — GCSE Chemistry
This how it works covers How Le Chatelier's Principle Works 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 5 of 13 in this topic. Use this how it works to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 5 of 13
Practice
20 questions
Recall
15 flashcards
⚙️ How Le Chatelier's Principle Works
Le Chatelier's Principle is not magic — it has a chemical explanation. When conditions change, the forward and backward reaction rates become temporarily unequal, causing a net shift until equilibrium is re-established.
Example — adding more reactant:
- Adding reactant increases its concentration
- This increases the forward reaction rate (more collisions)
- The backward rate is momentarily unchanged
- Products accumulate → backward rate increases
- A new equilibrium is reached with more products — the position has shifted right
Example — increasing temperature (for an exothermic forward reaction):
- More heat is supplied to the system
- Both rates increase, but the endothermic (backward) reaction benefits more
- More reactants form — equilibrium position shifts left
- The yield of products decreases (but rate of reaching equilibrium increases)