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Kinetics
This topic links reaction rate to particle collisions, activation energy and reaction conditions.
11
Objectives
55
Flashcards
55
Questions
90 min
Study time
AQAA LevelChemistryPhysical chemistry
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Syllabus checklist
What you need to know
11 objective pages available
Collision theory3 objectives
- Define activation energy.
- Explain why most collisions do not lead to reaction.
- Use collision frequency and energy to explain reaction rate.
Maxwell-Boltzmann distribution3 objectives
- Draw Maxwell-Boltzmann distribution curves.
- Interpret distribution curves at different temperatures.
- Use the area beyond activation energy to explain rate changes.
Factors affecting reaction rate5 objectives
- Explain how temperature affects rate using Maxwell-Boltzmann distributions.
- Explain how concentration affects collision frequency and rate.
- Explain how pressure affects gas reaction rate.
- Explain how catalysts increase rate by providing an alternative route with lower activation energy.
- Required practical: investigate how reaction rate changes with temperature.
Key terms
activation energycollision theorycollision frequencyMaxwell-Boltzmann distributionreaction ratecatalyst
Exam tips
- Understanding Activation Energy: Explain clearly by remember that activation energy is the minimum energy required for a reaction to occur. This helps in predicting how temperature changes affect reaction rates. Link the point to Collision theory, then state the evidence, calculation, mechanism, observation, or conclusion required by the question.
- Understanding Collision Theory: Explain clearly by focus on how activation energy influences reaction outcomes. Link the point to Collision theory, then state the evidence, calculation, mechanism, observation, or conclusion required by the question.
Common mistakes
- Misunderstanding Activation Energy: Activation energy is the minimum energy required for a reaction to occur, not the energy change. To clarify, remember that activation energy is a barrier that must be overcome for reactants to convert into products.
- Collisions Not Leading to Reaction: To correct this, students should explain that the cause is insufficient energy in most collisions. The mechanism is that only collisions with energy equal to or greater than the activation energy can overcome the energy barrier for reaction. The effect is that these collisions do not result in a reaction, leading to the consequence that reaction rates remain low.
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