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8. Reaction kinetics

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  1. 8.1 Rate of reaction

    1. 8.1.1Terms: rate of reaction, frequency of collisions

      • Explain and use the terms: rate of reaction, frequency of collisions, effective collisions and non-effective collisions

    2. 8.1.2—

      • Explain qualitatively, in terms of frequency of effective collisions, the effect of concentration and pressure changes on the rate of a reaction

    3. 8.1.3Experimental data to calculate the rate

      • Use experimental data to calculate the rate of a reaction

  2. 8.2 Temperature, rate and activation energy

    1. 8.2.1Activation energy, EA

      • Define activation energy, EA, as the minimum energy required for a collision to be effective

    2. 8.2.2Sketch and use the Boltzmann distribution

      • Sketch and use the Boltzmann distribution to explain the significance of activation energy

    3. 8.2.3In terms both of the Boltzmann distribution

      • Explain qualitatively, in terms both of the Boltzmann distribution and of frequency of effective collisions, the effect of temperature change on the rate of a reaction

  3. 8.3 Homogeneous and heterogeneous catalysts

    1. 8.3.1

      • Explain and use the terms catalyst and catalysis: - (a) to explain that, with a catalyst, a reaction has a different mechanism, i.e. one of lower activation energy - (b) to explain this catalytic effect in terms of the Boltzmann distribution - (c) to construct and interpret a reaction pathway diagram for a reaction in the presence and absence of an effective catalyst