Dynamic Equilibrium

sachakoeppen
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sachakoeppen
Created by sachakoeppen over 6 years ago
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dynamic equilibrium year 10 chemistry igcse

Resource summary

Dynamic Equilibrium
  1. Occurs in reversible reactions, when the forward and backward rate are equal
    1. It needs a closed system (no reactants or products can escape)
    2. Pressure (gas) / concentration (solution)
      1. 2NO2 (g) = N2O4 (g) Brown : Colourless 2 moles: 1 mole
        1. If pressure is increased, the equilibrium moves to where there are fewer molecules.
          1. More N2O4 is produced therefore the container looks more colourless
      2. Temperature
        1. 2NO2 (g) = N2O4 (g) Brown : Colourless
          1. Forward reaction is exothermic (ΔH= -ve) therefore the backward reaction is endothermic ( ΔH= +ve)
            1. If temperature is increased, the equilibrium moves to the endothermic direction
              1. More NO2 (higher yield of NO2) formed therefore the container looks more brown
          2. Catalysts have no overall effect on equilibrium as they speed up the forward + reverse reaction equally
            1. 3H + N2 = 2NH3 ΔH= -ve
              1. Temp increased - the equilibrium will move to 3H + N2 because it is the endothermic direction
                1. Pressure increased - the equilibrium will move to 2HN3 because there are fewer molecules
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