rate of reactions

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  • rates of reaction
    • reactions
      • slow
        • rusting
      • fast
        • burning
      • faster
        • explosion
    • collision theory
      • particles must collide with enough energy in order to react
      • how often do the particles collide.
      • how much energy is transferred in the collisions.
    • depends on four things
      • temperature
        • when increased, particles move faster
          • faster they move, the faster they collide
          • more energy, so collisions will have enough energy in order to react
      • concentration and pressure
        • more concentrated, more particles collide.
        • more pressure, more particles collide.
      • surface area
        • break into smaller pieces, same volume, more area, more frequent collisions.
      • catalyst
        • catalysts lower activation energy. easier to break bonds and react.
    • rate of reaction = amount of reactant used or amount of product formed / time
    • three ways of measuring the rate of reactions
      • precipitation and colour change
        • clear solution becomes opaque. cross under the conical flask. how long until the cross becomes impossible to see?
        • how long does it take to lose or change colour?
      • change in mass
        • usually produces a gas. the quicker the mass is lost, the quicker the reaction. measure regularly. plot a reaction graph.
      • volume of gas given off.
        • use a gas syringe. more gas given off in an interval of time, the faster the reaction.


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