Rate of Reaction Factors Practical


Part of our learning series on Rate of Reaction Chemistry, this visual chart set out a step by step practical for investigating the effect that catalysts can have on the rate of reaction. A great visual way to understand the steps.
Niamh Ryan
Flowchart by Niamh Ryan, updated more than 1 year ago
Niamh Ryan
Created by Niamh Ryan almost 7 years ago

Resource summary

Flowchart nodes

  • Carbon dioxide collects in the syringe
  • Hydrochloric acid and calcium carbonate react in the beaker
  • Different factors can be varied in order to investigate their effect on the rate of reaction:
  • Surface area to volume ratio: By repeating with marble chips and then calcium carbonate powder
  • Temperature: By repeating with HCl at different temperatures
  • Concentration: By repeating with concentrated and then dilute hydrochloric acid
  • Volume of gas collected is a measure of how much reaction has progressed
  • Measure the volume in syringe at several different times after the beginning of experiment
  • Plot Volume against Time
  • Only change one variable at a time
  • Start the timer as soon as the calcium carbonate is dropeed into the hydrochloric acid
  • The gradient of the volume vs time graph is the rate of reaction
  • If the gradient is steeper, the rate is faster
  • The gradient can be calculated by drawing a tangent to the curve at any point
  • To investigate the effect that catalysts can have on the rate of reaction:
  • Same experimental set-up but replace HCl and marble chips with hydrogen peroxide
  • Hydrogen peroxide decomposes naturally to hydrogen and oxygen but the rate of reaction can be increased using catalysts
  • Repeat the experiment using various catalysts such as manganese oxide, lead oxide, liver
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