Learning objective
Use Le Chatelier's principle to predict the effect of concentration changes.
Read the explanation, check the common trap, then practise with flashcards and questions.
At a glance
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Flashcards
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Questions
Topic
Chemical equilibria, Le Chatelier's principle and Kc
Subtopic
Equilibrium and Le Chatelier's principle
Study support
Understand this objective
Quick explanation
Use Le Chatelier's principle to predict the effect of concentration changes
- This point belongs to Chemical equilibria, Le Chatelier's principle and Kc, especially Equilibrium and Le Chatelier's principle.
- You need to be able to use Le Chatelier's principle to predict the effect of concentration changes.
- The key ideas to know are Le Chatelier and concentration.
- 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 Equilibrium and Le Chatelier's principle to exam-style questions, flashcards, and revision notes for Chemical equilibria, Le Chatelier's principle and Kc.
Quick student answer
What will happen to the position of equilibrium when the concentration of a reactant is increased in the following reaction? N2(g) + 3H2(g) ⇌ 2NH3(g)
Direct answer
The equilibrium shifts to the right.
Key terms
- Equilibrium: A state in a reversible reaction where the rates of the forward and reverse reactions are equal.
- Concentration: The amount of a substance in a given volume, often expressed in mol/dm³.
Common trap
Confusing the effects of concentration changes: Remember that increasing the concentration of reactants shifts the equilibrium to the right, while increasing products shifts it to the left.
Related questions
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Flashcard prompts
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Revision tools
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Revision notestopic notes
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Open revision notesRelated learning objectives
- Define dynamic equilibrium in a closed system.
Equilibrium and Le Chatelier's principle
- Use Le Chatelier's principle to predict the effect of pressure changes.
Equilibrium and Le Chatelier's principle
- Use Le Chatelier's principle to predict the effect of temperature changes.
Equilibrium and Le Chatelier's principle
- Explain why catalysts do not change the position of equilibrium.
Equilibrium and Le Chatelier's principle
- Construct Kc expressions for homogeneous equilibria.
Equilibrium constant Kc