GCSE Chemistry (AQA)

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Reaction Profile for Catalysed Reaction

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The rate and extent of chemical change Rate of reaction

Reaction Profile for Catalysed Reaction

3:05 Effects of Catalysts on the Rate of Reaction
Spec 4.6.1.2 4.6.1.4
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  • Catalysts provide a different pathway for reactions with lower activation energy.
  • Catalysts allow different reactions to occur, creating the same products as the direct reaction without a catalyst.
  • Reaction profiles show how energy changes as a reaction progresses.
  • Without a catalyst, reactants have more energy than products, and a bump represents the activation energy needed.
  • With a catalyst, the energy levels of reactants and products remain unchanged, but the activation energy bump is lower.
  • Lower activation energy means an alternate reaction path is provided by the catalyst.
  • Catalysts are used in industry to lower activation energies, saving costs by reducing the need for high temperatures.
  • Lowering activation energy increases the number of particles with sufficient energy to react.
  • According to collision theory, reactions occur when particles collide with sufficient energy, which is the activation energy.
  • Without a catalyst, many collisions occur, but few have enough energy to react.
  • Adding a catalyst decreases the activation energy, allowing more collisions to lead to reactions.
  • Catalysts increase the proportion of successful collisions, thus increasing the reaction rate.
  • More successful collisions in the same amount of time result in a faster reaction and a higher rate.

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