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Collision theory and Boltzmann

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Higher temperatures increase the rate of reaction by providing particles with more kinetic energy, leading to more frequent and more energetic collisions that are more likely to exceed the activation energy needed for the reaction to occur. Specifically, for every 10 degree C rise in temperature, the rate of reaction doubles and the time taken halves, as increased particle energy from heat causes more collisions per unit time and a greater chance of particles reaching the activation energy required to react upon colliding.

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The effect of temperature on rate of reaction Lesson aims: To revise the link between concentration and rate To understand the quantitative affect of temperature on rate To understand the affect of temperature on particle collisions
The relationship between temperature and rate For every 10C rise in temperature the rate of reaction doubles, the time taken for the reaction to occur halves.
Why does this happen? For a reaction to occur two particles must: Collide Collide with enough energy
Why does this happen? Increasing the temperature increases the amount of energy the particles have. If particles are given more energy they will move faster and this will mean: More collisions in a certain time More collisions are likely to result in a reaction
Boltzmann Distribution Every particle in a reaction has a certain amount of energy. Some will have high energy and some will have low energy. Activation energy is the energy they need to react. This can be represented on a graph.
Boltzmann Distribution Energy Number of particles Activation energy The number of particles able to react on collision

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Collision theory and Boltzmann

  • 1. The effect of temperature on rate of reaction Lesson aims: To revise the link between concentration and rate To understand the quantitative affect of temperature on rate To understand the affect of temperature on particle collisions
  • 2. The relationship between temperature and rate For every 10C rise in temperature the rate of reaction doubles, the time taken for the reaction to occur halves.
  • 3. Why does this happen? For a reaction to occur two particles must: Collide Collide with enough energy
  • 4. Why does this happen? Increasing the temperature increases the amount of energy the particles have. If particles are given more energy they will move faster and this will mean: More collisions in a certain time More collisions are likely to result in a reaction
  • 5. Boltzmann Distribution Every particle in a reaction has a certain amount of energy. Some will have high energy and some will have low energy. Activation energy is the energy they need to react. This can be represented on a graph.
  • 6. Boltzmann Distribution Energy Number of particles Activation energy The number of particles able to react on collision