Learning objective
Define activation energy.
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
Kinetics
Subtopic
Collision theory
Study support
Understand this objective
Quick explanation
Define activation energy
- This point belongs to Kinetics, especially Collision theory.
- You need to be able to define activation energy.
- The key ideas to know are activation energy.
- 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 Collision theory to exam-style questions, flashcards, and revision notes for Kinetics.
Quick student answer
What is the definition of activation energy?
Direct answer
The minimum energy required for a reaction to occur.
Key terms
- Activation Energy: The minimum energy required for a chemical reaction to occur.
- Arrhenius Equation: An equation that expresses the relationship between the rate constant of a reaction and temperature, incorporating activation energy.
Common trap
Confusing activation energy with overall energy change: Activation energy is the energy barrier that must be overcome for a reaction to proceed, while the enthalpy change is the difference in energy between reactants and products.
Related questions
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Flashcard prompts
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Revision tools
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Flashcards0 linked cards
Practice Questions0 linked questions
Revision notestopic notes
Open the full topic revision notes when you are ready to review this objective in context.
Open revision notesRelated learning objectives
- Explain why most collisions do not lead to reaction.
Collision theory
- Use collision frequency and energy to explain reaction rate.
Collision theory
- Draw Maxwell-Boltzmann distribution curves.
Maxwell-Boltzmann distribution
- Interpret distribution curves at different temperatures.
Maxwell-Boltzmann distribution
- Use the area beyond activation energy to explain rate changes.
Maxwell-Boltzmann distribution