Kinetics

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  • Created by: emma
  • Created on: 29-04-14 19:33
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  • Kinetics
    • Activation energy
      • The minimum amount of energy required for a reaction to take place
      • For a reaction to take place
        • Particles must collide with enough energy to overcome activation energy
        • Must collide in the correct orientation
    • Increase rate of reaction
      • Increase temperature
        • average energy of particles increases
          • Particles move faster
            • more particles have a collision energy greater than Ea
              • Number of successful collisions per second increases
      • Decrease particle size
        • Surface area increases
          • Number of successful collisions per second increases
      • Increase pressure
        • Number of particles per unit volume increases
          • Number of successful collisions per seecond increases
      • Increase concentration
        • Number of particles per unit volume increase
          • Number of successful collisions per second increase
      • Add a catalyst
        • What
          • substance which increases rate of chemical reaction with out itself being chemically changed
        • How
          • Substance which provides an alternative rout for the reaction with a lower activation energy
    • Maxwell boltzmann
      • Area under curve is total number of particles
      • Peak represents most probable energy (energy possessed by largest proportion of particles)
      • Area under curve to right of Ea are particles with Ea
      • Increase temp moves curve to the right and lower

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