Dynamic Equilibrium — GCSE Chemistry Revision
Revise Dynamic Equilibrium 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.
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Go to Le Chatelier's PrincipleWhat is Dynamic Equilibrium?
Dynamic equilibrium occurs in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction. At equilibrium, the concentrations of the reactants and products remain constant, but the reactions have not stopped. The 'dynamic' part means that both reactions are still occurring.
Board notes: Dynamic equilibrium is a higher-tier topic for all boards. It is crucial for understanding Le Chatelier's principle and industrial processes like the Haber process. You must be able to define it in terms of reaction rates and constant concentrations in a closed system.
Step-by-step explanationWorked example
In a sealed bottle of fizzy drink, an equilibrium exists between the dissolved carbon dioxide and the gaseous carbon dioxide: CO₂(aq) ⇌ CO₂(g). The rate at which CO₂ dissolves is equal to the rate at which it escapes from the solution, so the pressure remains constant.
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Common mistakes
- 1Thinking that equilibrium means the reaction has stopped. It is a dynamic process, with both forward and reverse reactions continuing at the same rate.
- 2Believing that the concentrations of reactants and products must be equal at equilibrium. The concentrations are constant, but not necessarily equal.
- 3Forgetting that equilibrium can only be reached in a closed system, where no substances can enter or leave.
Dynamic Equilibrium exam questions
Exam-style questions for Dynamic Equilibrium with mark-scheme style solutions and timing practice. Aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP specifications.
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Dynamic Equilibrium
Core concept
Dynamic equilibrium occurs in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction. At equilibrium, the concentrations of the reactants and products remai…
Frequently asked questions
What is a closed system?
A closed system is one that does not allow any matter to be exchanged with the surroundings. Energy, however, can be transferred in or out.
What happens if you open the fizzy drink bottle?
Opening the bottle means it is no longer a closed system. The CO₂(g) escapes, so the equilibrium is disturbed. The forward reaction (dissolving) is now slower than the reverse reaction (escaping), so the drink goes flat.