Dynamic Equilibrium

  • Many reactions are reversible
  • Dynamic equilibrium is reached when the concentration of the reactants and products are at a constant, and the forward and backward reactions are at the same rate
  • Dynamic equilibrium can only occur in a closed system at a constant temperature
  • An example of dynamic equilibrium would be more reactants being used up in the reaction would cause the forward reaction to slow down as more products are forming. However as there are now more products than there are reactants the reaction will shift to the left producing more reactants. After a while there will be an equal quantity of both reactants and product forming and therefore the overall concentration of each does not change.

Le Chatelier’s principle

“if a system at equilibrium is disturbed, the equilibrium shifts in the direct that tends to reduce the disturbance”

  • Any factor which changes the effect of the equilibrium mixture will result in the position of equilibrium shifting so to oppose the change
  • Le Chatelier’s Principle does not account for how far the equilibrium changes, and therefore no quantities can be predicted

Change in Concentration

  • If an increase in concentration of one of the reactants then the equilibrium will shift in the direction that will reduce the concentration

A(aq) + B(aq)⇋ C(aq) + D(aq)

  • by increasing the concentration of B this will react with A which will produce more C+D. Thus, more product is formed and equilibrium moves to the right.
  • By removing a product formed, such as C, then the equilibrium will move to the right to produce more C (as well as D) using up the reactants A+B more.

Changing the Pressure

  • Changing the pressure only affects reaction that include gases
  • Changing the pressure only affects gas reactions that have a differing number of molecules on each side

A(g)⇋ 2C(g)

  • Increasing the pressure of a gas means that there are more molecules in it at a given volume, it is equivalent to increasing the concentration of a solution
  • Increasing the pressure of a system will cause the position of equilibrium to shift to the side with the fewer molecules as that will reduce the pressure

Changing the temperature

  • All reversible reactions have an exothermic reactions in one direction and an endothermic reaction in the opposite
  • A negative ΔH = exothermic
  • A positive ΔH = endothermic

A(g) + B(g)⇋ C(g) + D(g) ΔH = -203 Kj mol-1

  • As the ΔH is negative, the forward reaction is exothermic (reactants -> products)
  • The backwards reaction is endothermic (products -> reactants)
  • By increasing the temperature, the equilibrium will move to the endothermic reaction. As endothermic reactions absorb heat
  • By decreasing the temperature, the equilibrium will move to the exothermic reaction. As exothermic reactions give off heat

Catalysts

  • Catalysts do not affect the position of equilibria
  • They allow for equilibrium to be reached more quickly as they effect both side of the reaction equally