Le Chatelier's principle is your key to predicting what happens... Show more
Chemistry72 views·Updated Jun 10, 2026·2 pagesMastering AQA GCSE Chemistry Topic 6: Le Chatelier's Principle and Equilibrium
Mighty Blabs@blabsthemighty
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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.
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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 Jun 10, 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
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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
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?
Our AI Companion is a student-focused AI tool that offers more than just answers. Built on millions of Knowunity resources, it provides relevant information, personalised study plans, quizzes, and content directly in the chat, adapting to your individual learning journey.
Where can I download the Knowunity app?
You can download the app from Google Play Store and Apple App Store.
Is Knowunity really free of charge?
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
Most popular content: Shift
2Most popular content in Chemistry
9Most popular content
9Can't find what you're looking for? Explore other subjects.
Students love us — and so will you.
4.6/5App Store
4.7/5Google Play
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan SiOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha KlichAndroid user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
AnnaiOS user