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Chemistry 06206.2 Rate of reaction

Rate of reaction lab

Change concentration, temperature and surface area, then compare the gas-volume curves side by side.

  • Collision theory
  • Factors affecting rate
  • Interpreting rate graphs
60cm³time (s)

Initial rate

3cm³/s

Time to 30 cm³

13.9s

Final volume

60cm³

Predict

Raising the temperature by 10 °C roughly doubles the rate. Which effect is the larger reason?

Experiment

  1. 1Keep a curve at 25 °C, then run one at 45 °C and compare the steepness and the plateau height.
  2. 2Switch from lumps to powder with everything else fixed.
  3. 3Add a catalyst and confirm the final volume does not change.

Explain

For a reaction to happen, particles must collide with at least the activation energy and in the right orientation. Anything that increases the frequency of collisions, or the fraction that are successful, increases the rate.

  • Higher concentration or pressure — more particles in the same volume, so more frequent collisions.
  • Larger surface area — more particles exposed, so more frequent collisions.
  • Higher temperature — faster particles and a much larger fraction above the activation energy.
  • Catalyst — an alternative pathway with a lower activation energy, so more collisions succeed.

None of them changes how much product forms. The plateau height depends only on how much reactant you started with.