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Kinetics
This topic links reaction rate to particle collisions, activation energy and reaction conditions.
11
Objectives
10
Flashcards
10
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 EnergyArrhenius EquationEffective collisionRate of reactionCollision frequencyReaction rateTemperatureDistribution CurveKinetic EnergyCollision TheoryMaxwell-Boltzmann DistributionCollision Frequency
Exam tips
- Understand the Arrhenius equation: Familiarize yourself with how to manipulate the Arrhenius equation for calculations involving activation energy and temperature.
- Use diagrams to illustrate collision theory: When explaining collision theory, consider drawing diagrams to show how molecules collide and the conditions required for a successful reaction.
Common mistakes
- 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.
- Confusing activation energy with overall energy change: Remember that activation energy is the energy needed to start the reaction, while the overall energy change is the difference between the energy of products and reactants.
Practice preview
- What is the definition of activation energy?
- Explain how temperature affects the activation energy of a reaction.
- A reaction has an activation energy of 75 kJ/mol. Calculate the fraction of molecules that have energy greater than or equal to the activation energy at 298 K using the Arrhenius equation.
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