Rates of Reactions

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  • Created by: Lena Fray
  • Created on: 17-09-15 12:28
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  • Rate Of Reactions
    • Calculation
      • Rate of Reaction = Amount of reactant used or amount of product formed
        • divided by time
    • Activation Energy
      • The minimum amount of energy need for a reaction to happen
        • If there is not enough energy then....
          • There is no reaction
        • They the particles collide with enough energy then...
          • They react and form a product
    • Factors that effect it
      • Catalysts
        • lower the activation need
          • So more particles are able to react
        • They are NOT used up
      • Concentration/Pressure
        • means there are more reacting particles in the solution
          • A higher ratio
          • this means more reactions happen
      • Temprature
        • Increasing  makes the reaction faster
          • because it gives the particles more energy
            • So they are more likely to collide
              • as they will hold at least the activation energy.
      • Surface Area
        • The larger the surface are the faster the reaction.
          • the more reacting particles exposed
            • so more collisions happen
    • Measuring
      • Whats produced
        • Make sure you state the length of time
        • Volume produced
        • Mass
    • Collision Theory
      • Parties must collide with sufficient energy in order to react
        • This is known as ACTIVATION ENERGY


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