equilibrium

Cards (18)

  • Chemical equilibrium
    All reversible reactions reach a dynamic equilibrium state
  • Dynamic equilibrium
    1. Forward and backward reactions are occurring at equal rates
    2. Concentrations of reactants and products stays constant
    3. Reaction is continuous
  • Position of equilibrium
    Describes the composition of the equilibrium mixture
  • Position of equilibrium favouring reactants
    Equilibrium mixture will contain mostly reactants
  • Le Chatelier's principle
    If an external condition is changed the equilibrium will shift to oppose the change (and try to reverse it)
  • If temperature is increased
    Equilibrium will shift in the endothermic direction to try to reduce the temperature
  • If temperature is decreased
    Equilibrium will shift in the exothermic direction to try to increase the temperature
  • Low temperatures may give a higher yield of product but will also result in slow rates of reaction
  • If pressure is increased
    Equilibrium will shift towards the side with fewer moles of gas to try to reduce the pressure
  • If pressure is decreased
    Equilibrium will shift towards the side with more moles of gas to try to increase the pressure
  • If the number of moles of gas is the same on both sides of the equation then changing pressure will have no effect on the position of equilibrium
  • Increasing the concentration of OH- ions
    Equilibrium shifts in the forward direction to remove OH- ions
  • Adding H+ ions

    Equilibrium shifts back to the left
  • A catalyst has no effect on the position of equilibrium, but it will speed up the rate at which the equilibrium is achieved
  • Industrial processes using equilibrium
    • Haber process
    • Contact process
    • Hydration of ethene
    • Production of methanol from CO
  • Recycling unreacted reactants back into the reactor can improve the overall yields of these processes
  • High pressure leads to too high energy costs for pumps and too high equipment costs
  • Catalysts speed up the rate, allowing lower temperatures to be used but have no effect on equilibrium