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Rates of reaction - Coggle Diagram

- - - - To react, particles must:
      - collide
      - have the correct spatial orientation
      - have energy ≥ activation energy (minimum energy required for a
      - reaction)
- - - - Higher pressures of gas mean more particles per unit volume. Therefore, the frequency of collisions will increase – increasing the rate of reaction.
    - - A catalyst speeds up the rate of reaction but is not consumed in the process.
        Catalysts increase the rate of reaction by: - providing an alternative mechanism for a reaction - with a lower activation energy
    - - For non-porous solids, reactions can only occur on the surface, as this is the only place that reagents can collide. Breaking up the solid into small pieces or a powder increases surface area. Therefore, the frequency of collisions will increase – increasing the rate.
    - - Increasing the temperature leads to particles having a higher kinetic energy: - particles will collide more frequently – only slightly increases rate - particles collide with more energy – more collisions have energy ≥ Ea – much greater proportion of collisions are successful