3.1.5
Kinetics
Section 3.1.5 covers collision theory and activation energy, the Maxwell-Boltzmann distribution and its use to explain the effects of temperature and of a catalyst, the meaning of rate and the qualitative effects of concentration and pressure, and how catalysts work. The measuring page supports required practical 3 (initial rate by a clock method).
Revision Notes
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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
AQA A-level Chemistry · 3.1.5 Kinetics
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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3.1.5.1
- i
understand that reactions can only occur when collisions take place between particles having sufficient energy
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3.1.5.2
3.1.5.3
- iii
use the Maxwell-Boltzmann distribution to explain why a small temperature increase can lead to a large increase in rate
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3.1.5.4
3.1.5.5
- i
know that a catalyst increases the rate of a chemical reaction without being changed in chemical composition or amount
Revise - ii
know that catalysts work by providing an alternative reaction route of lower activation energy
Revise - iii
use a Maxwell-Boltzmann distribution to explain how a catalyst increases the rate of a reaction involving a gas
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