Dynamic Equilibrium

Occurs in reversible reactions, when the forward and backward rate are equal
1. It needs a closed system (no reactants or products can escape)
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
Temperature
1. 2NO2 (g) = N2O4 (g) Brown : Colourless
  1. Forward reaction is exothermic (ΔH= -ve) therefore the backward reaction is endothermic ( ΔH= +ve)
  2. 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
Catalysts have no overall effect on equilibrium as they speed up the forward + reverse reaction equally
3H + N2 = 2NH3 ΔH= -ve
1. Temp increased - the equilibrium will move to 3H + N2 because it is the endothermic direction
2. Pressure increased - the equilibrium will move to 2HN3 because there are fewer molecules

Resource summary

	Created by sachakoeppen over 10 years ago

	Copied by Noah Watts about 7 years ago