Learning objective
Use collision frequency and energy to explain reaction rate.
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
Use collision frequency and energy to explain reaction rate
- This point belongs to Kinetics, especially Collision theory.
- You need to be able to use collision frequency and energy to explain reaction rate.
- The key ideas to know are energy, collision, and frequency.
- 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
Which of the following factors does NOT affect the rate of a chemical reaction according to collision theory?
Direct answer
D) Color of reactants
Key terms
- Collision frequency: The number of collisions that occur per unit time in a given volume of reactants.
- Reaction rate: The speed at which reactants are converted into products in a chemical reaction.
Common trap
Confusing activation energy with enthalpy change: Remember that activation energy is the energy barrier that must be overcome for the reaction to proceed, while ΔH 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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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
- Define activation energy.
Collision theory
- Explain why most collisions do not lead to reaction.
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