Topic 9
Kinetics I
Topic 9 explains how fast reactions go and why: collision theory and activation energy, calculating rates from times and from gradients, the Maxwell–Boltzmann distribution and the effect of temperature, and catalysts, their reaction profiles, heterogeneous catalysis at surfaces and their economic benefits. Kinetics II (rate equations) follows in Topic 16.
Revision Notes
4 revision notes, in the order the specification teaches them.
Collision Theory and Rates of Reaction
Collision theory: rate of reaction, activation energy, effective collisions and the effects of concentration, pressure, surface area and temperature.
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Measuring and Calculating Rates
Measuring rates: mass, gas volume and clock methods, rate = 1/time, tangents and initial rate on concentration–time graphs.
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The Maxwell–Boltzmann Distribution
The Maxwell–Boltzmann distribution: shape, activation energy, the effect of temperature and the effect of a catalyst on the proportion of molecules that can react.
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Catalysts and Reaction Profiles
Catalysts: lower activation energy, reaction profiles with the intermediate, homogeneous and heterogeneous catalysis, and the economic and environmental benefits.
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Kinetics Map
Edexcel A Level Chemistry · Topic 9 Kinetics I
The whole section on one A4 page: collision theory, concentration and pressure, surface area, measuring rates, Maxwell–Boltzmann and temperature, and catalysts, with worked examples.
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Specification
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9.1
9.2
- 9.2
understand that reactions only take place when collisions take place with sufficient energy, known as activation energy
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9.3
- ii
be able to calculate the rate of a reaction from: the gradient of a suitable graph, by drawing a tangent, either for initial rate, or at a time, t
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9.4
- 9.4
understand qualitatively, in terms of the Maxwell-Boltzmann distribution of molecular energies, how changes in temperature affect the rate of a reaction
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9.5
- 9.5
understand the role of catalysts in providing alternative reaction routes of lower activation energy
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9.6
9.7
- 9.7
be able to interpret the action of a catalyst in terms of a qualitative understanding of the Maxwell-Boltzmann distribution of molecular energies
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9.8
- 9.8
understand the use of a solid (heterogeneous) catalyst for industrial reactions, in the gas phase, in terms of providing a surface for the reaction
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9.9
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