Le Chatelier's principle is your key to predicting what happens...
Chemistry72 views·Updated 1 Jul 2026·2 pagesMastering AQA GCSE Chemistry Topic 6: Le Chatelier's Principle and Equilibrium
Mighty Blabs@blabsthemighty
1
of 2
Le Chatelier's Principle Basics
Think of equilibrium as a perfectly balanced seesaw that doesn't want to be disturbed. When you mess with the conditions, the system fights back to restore balance - that's Le Chatelier's principle in action.
Concentration changes are the easiest to understand. Add more reactants? The reaction shifts right to make more products. Flood the system with products? It shifts left to create more reactants. The system is essentially trying to use up whatever you've added.
Temperature changes depend on whether your reaction gives out heat (exothermic) or takes in heat (endothermic). Crank up the temperature and equilibrium favours the endothermic direction - it's trying to absorb that extra heat you've added.
Quick tip: Remember that increasing temperature always favours the endothermic direction, whilst decreasing temperature favours the exothermic direction.
2
of 2
Pressure Effects on Equilibrium
Pressure changes only matter when you've got gases involved - and it's all about counting molecules. When pressure increases, the equilibrium shifts towards whichever side has fewer gas molecules, trying to reduce the pressure you've applied.
This means you'll get a higher yield of products if the product side has fewer gas molecules. It's like the reaction is trying to squeeze into a smaller space by making fewer, more compact molecules.
When pressure decreases, the opposite happens - equilibrium shifts towards the side with more gas molecules. The reaction spreads out to fill the extra space you've given it.
Exam hack: Always count the number of gas molecules on each side of your equation - this tells you exactly which way pressure changes will push your equilibrium.
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Chemistry72 views·Updated 1 Jul 2026·2 pagesMastering AQA GCSE Chemistry Topic 6: Le Chatelier's Principle and Equilibrium
Mighty Blabs@blabsthemighty
Le Chatelier's principle is your key to predicting what happens when chemical reactions get disrupted. It's like a chemical reaction's way of fighting back against change - understanding this will help you master equilibrium problems in your chemistry exams.
1
of 2
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Le Chatelier's Principle Basics
Think of equilibrium as a perfectly balanced seesaw that doesn't want to be disturbed. When you mess with the conditions, the system fights back to restore balance - that's Le Chatelier's principle in action.
Concentration changes are the easiest to understand. Add more reactants? The reaction shifts right to make more products. Flood the system with products? It shifts left to create more reactants. The system is essentially trying to use up whatever you've added.
Temperature changes depend on whether your reaction gives out heat (exothermic) or takes in heat (endothermic). Crank up the temperature and equilibrium favours the endothermic direction - it's trying to absorb that extra heat you've added.
Quick tip: Remember that increasing temperature always favours the endothermic direction, whilst decreasing temperature favours the exothermic direction.
2
of 2Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Pressure Effects on Equilibrium
Pressure changes only matter when you've got gases involved - and it's all about counting molecules. When pressure increases, the equilibrium shifts towards whichever side has fewer gas molecules, trying to reduce the pressure you've applied.
This means you'll get a higher yield of products if the product side has fewer gas molecules. It's like the reaction is trying to squeeze into a smaller space by making fewer, more compact molecules.
When pressure decreases, the opposite happens - equilibrium shifts towards the side with more gas molecules. The reaction spreads out to fill the extra space you've given it.
Exam hack: Always count the number of gas molecules on each side of your equation - this tells you exactly which way pressure changes will push your equilibrium.
We thought you’d never ask...
What is the Knowunity AI companion?
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