A-level Chemistry Reaction rates and equlibrium

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  • Reaction Rates and Equilibrium
    • Collisions
      • Concentration
      • Pressure
      • Untitled
    • Catalysts
      • Homogeneous
        • when catalysts and reactants are the same state
      • Hetrogeneous
        • when catalysts and reactants are different states
    • Boltzmann Distribution
      • Area under graph show the concentration of particles
      • Activation energy- the energy required to start a reaction
        • Catalysts lower activation energy meaning more molecules react and are produced speed up reaction Alternative route
          • Catalysts
            • Homogeneous
              • when catalysts and reactants are the same state
            • Hetrogeneous
              • when catalysts and reactants are different states
    • Dynamic equilibrium
      • Rate of reaction is the same forward as it is reverse Concentration is constant
      • Chandelier Principle
        • Pressure
          • Higher pressure = shift to side with fewer gas molecules
          • Low pressure = shift to side with greater gas molecules
        • temperature
          • Endothermic
            • High temp = shift to right
            • Low temp = shift to left
            • Positive
          • Exothermic
            • High temp = shift to left
            • Low temp = shift to right
            • Negative
        • conentration
          • More product shift left
          • More Reactant shift right
        • when equilibrium changes shifting the system to have minimal effect
    • Equilibrium constant
      • Kc=[E]eX[D]d/[A]aX[B]b
  • Chandelier Principle
    • Pressure
      • Higher pressure = shift to side with fewer gas molecules
      • Low pressure = shift to side with greater gas molecules
    • temperature
      • Endothermic
        • High temp = shift to right
        • Low temp = shift to left
        • Positive
      • Exothermic
        • High temp = shift to left
        • Low temp = shift to right
        • Negative
    • conentration
      • More product shift left
      • More Reactant shift right
    • when equilibrium changes shifting the system to have minimal effect

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