logo

Learning objective

Distinguish closed systems from open systems for equilibrium.

Read the explanation, check the common trap, then practise with flashcards and questions.

Start flashcardsTry practice questionsTopic hub

At a glance

0

Flashcards

0

Questions

Topic

Reversible reactions and dynamic equilibrium

Subtopic

Equilibrium

Aqa Gcse ChemistryThe rate and extent of chemical change

Study support

Understand this objective

Quick explanation

Distinguish closed systems from open systems for equilibrium

  • This point belongs to Reversible reactions and dynamic equilibrium, especially Equilibrium.
  • You need to be able to distinguish closed systems from open systems for equilibrium.
  • The key ideas to know are closed system and equilibrium.
  • Use the linked flashcards and practice questions to check recall, then practise applying the idea in an exam-style answer.

Key concepts

closed systemequilibrium

Why it matters

This objective helps connect Equilibrium to exam-style questions, flashcards, and revision notes for Reversible reactions and dynamic equilibrium.

Quick student answer

What should you know about distinguish closed systems from open systems for equilibrium?

Direct answer

In Chemistry, this page helps you answer questions about distinguish closed systems from open systems for equilibrium 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 open system.

Key terms

  • closed system: A system where no matter can enter or leave, allowing equilibrium to be established. 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.
  • open system: A system where matter can enter or leave, preventing equilibrium from being established. 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

Closed vs Open System Confusion: Clarify that a closed system cannot exchange matter (only energy) with its surroundings; only in a closed system can a reversible reaction reach dynamic equilibrium because the amounts of reactants and products remain fixed. In an open system, continuous addition or removal of substances prevents the system from stabilising at constant concentrations, so true equilibrium cannot be achieved.

Related questions

Try this as a practice card

4 linked

Question 1 of 4

Choose an answer, get feedback, then move sideways through the set.

0 of 4 attempted

Flashcard prompts

Flip through the key recall cards

4 cards

Flashcard 1 of 4

Press Space to flip, arrows to move

Practise next

AnswersFlashcardsMCQ drillPractice testQuestions

Revision tools

Choose how to practise

Back to topic hub
Flashcards0 linked cards
No objective-specific flashcards are cached for this page. Use the topic hub to revise the surrounding flashcards without triggering a frozen-subject DB fallback.Open topic hub
Practice Questions0 linked questions
No objective-specific practice questions are cached for this page. Use the topic question bank to practise nearby curriculum questions without weakening the egress guard.Open topic questions
Revision notestopic notes

Open the full topic revision notes when you are ready to review this objective in context.

Open revision notes

Related learning objectives