Le Chatelier's Principle — GCSE Chemistry Revision
Revise Le Chatelier's Principle for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
At a glance
- What StudyVector is
- An exam-practice platform with board-aligned questions, explanations, and adaptive next steps.
- This topic
- Le Chatelier's Principle in GCSE Chemistry: explanation, examples, and practice links on this page.
- Who it’s for
- Students revising GCSE Chemistry for UK exams.
- Exam boards
- Practice is aligned to major specifications (AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP).
- Free plan
- Sign up free to use tutor paths and feedback on your answers. Free access is 3 days uncapped, then 30 min practice/day. Pricing
- What makes it different
- Syllabus-shaped practice and progress tracking—not generic AI answers.
Topic has curated content entry with explanation, mistakes, and worked example. [auto-gate:promote; score=70.6]
Recommended next topic
Next step: Rates of Reaction
Continue in the same course — structured practice and explanations on StudyVector.
Go to Rates of ReactionWhat is Le Chatelier's Principle?
Le Chatelier's principle states that if a change is made to the conditions of a system at equilibrium, the system will respond to counteract the change. This principle is used to predict how changes in temperature, pressure, or concentration will affect the position of equilibrium.
Board notes: Le Chatelier's principle is a higher-tier topic for all exam boards and is essential for explaining industrial process conditions. You must be able to predict the effect of changing temperature, pressure, and concentration on the position of equilibrium for a given reversible reaction.
Step-by-step explanationWorked example
In the Haber process, N₂(g) + 3H₂(g) ⇌ 2NH₃(g), the forward reaction is exothermic. To increase the yield of ammonia, you would use a low temperature (to favour the exothermic direction) and a high pressure (to favour the side with fewer moles of gas).
Practise this topic
Jump into adaptive, exam-style questions for Le Chatelier's Principle. Free to start; sign in to save progress.
Common mistakes
- 1Applying the principle incorrectly. Remember the system tries to *oppose* the change. If you increase temperature, the equilibrium will shift in the endothermic direction to absorb the extra heat.
- 2Forgetting that a catalyst does not change the position of equilibrium. It speeds up both the forward and reverse reactions equally, so equilibrium is reached faster.
- 3Confusing the effect of pressure on reactions with an equal number of moles of gas on both sides. In this case, a change in pressure has no effect on the position of equilibrium.
Le Chatelier's Principle exam questions
Exam-style questions for Le Chatelier's Principle with mark-scheme style solutions and timing practice. Aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP specifications.
Le Chatelier's Principle exam questionsGet help with Le Chatelier's Principle
Get a personalised explanation for Le Chatelier's Principle from the StudyVector tutor. Ask follow-up questions and work through problems with step-by-step support.
Open tutorFree full access to Le Chatelier's Principle
Sign up in 30 seconds to unlock step-by-step explanations, exam-style practice, instant feedback and on-demand coaching — completely free, no card required.
Try a practice question
Unlock Le Chatelier's Principle practice questions
Get instant feedback, step-by-step help and exam-style practice — free, no card needed.
Start Free — No Card NeededAlready have an account? Log in
Step-by-step method
Step-by-step explanation
4 steps · Worked method for Le Chatelier's Principle
Core concept
Le Chatelier's principle states that if a change is made to the conditions of a system at equilibrium, the system will respond to counteract the change. This principle is used to predict how changes i…
Frequently asked questions
What does 'shifting the equilibrium' mean?
Shifting the equilibrium means that the rates of the forward and reverse reactions are temporarily unequal, causing a change in the concentrations of reactants and products until a new equilibrium position is established.
How does changing concentration affect equilibrium?
If you increase the concentration of a reactant, the equilibrium will shift to the right to use up the extra reactant and make more product. If you remove a product, the equilibrium will shift to the right to replace it.