Learning objective
(HT only) Explain why a closed system is required when applying equilibrium predictions.
Read the explanation, check the common trap, then practise with flashcards and questions.
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Topic
Reversible reactions and dynamic equilibrium
Subtopic
The effect of changing conditions on equilibrium (HT only)
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Quick explanation
(HT only) Explain why a closed system is required when applying equilibrium predictions
- This point belongs to Reversible reactions and dynamic equilibrium, especially The effect of changing conditions on equilibrium (HT only).
- You need to be able to (HT only) Explain why a closed system is required when applying equilibrium predictions.
- The key ideas to know are closed system and HT only.
- Use the linked flashcards and practice questions to check recall, then practise applying the idea in an exam-style answer.
Key concepts
Why it matters
This objective helps connect The effect of changing conditions on equilibrium (HT only) to exam-style questions, flashcards, and revision notes for Reversible reactions and dynamic equilibrium.
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What should you know about (HT only) Explain why a closed system is required when applying equilibrium predictions?
Direct answer
In Chemistry, this page helps you answer questions about (HT only) Explain why a closed system is required when applying equilibrium predictions within Reversible reactions and dynamic equilibrium. Focus on the key process, correct scientific terms, and how the idea links to exam-style questions. Key terms to check are closed system and equilibrium predictions.
Key terms
- closed system: A closed system is one where no matter enters or leaves, allowing for accurate equilibrium predictions. In AQA GCSE Chemistry 8462, use this term specifically when explaining rate of reaction, collision theory, reversible reactions, equilibrium, catalysts, graph gradients, or Le Chatelier's principle.
- equilibrium predictions: Equilibrium predictions are forecasts about the position of equilibrium based on changes in concentration, temperature, or pressure. In AQA GCSE Chemistry 8462, use this term specifically when explaining rate of reaction, collision theory, reversible reactions, equilibrium, catalysts, graph gradients, or Le Chatelier's principle.
Common trap
Understanding Closed Systems: Emphasize that a closed system allows for accurate predictions of equilibrium shifts because it keeps the concentrations of reactants and products constant.
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Revision notestopic notes
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Open revision notesRelated learning objectives
- Define a reversible reaction as a reaction in which products can react to make the original reactants.
Reversible reactions
- Identify the forward reaction and reverse reaction in a reversible reaction.
Reversible reactions
- Use the reversible reaction symbol in equations.
Reversible reactions
- Describe examples of reversible reactions such as hydrated copper sulfate and anhydrous copper sulfate.
Reversible reactions
- Describe thermal decomposition of ammonium chloride as a reversible reaction example.
Reversible reactions