Reversible reactions and dynamic equilibrium

• What is a reversible reaction?

  A reaction that can proceed in both the forward and reverse directions.
• During a reversible reaction, what happens as the reaction progresses and the reactants react?

  1. The concentration of reactants fall.
  2. The forward reaction slows down
  3. The concentrations of products rise
  4. The backwards reaction speeds up
• When is a system 'at equilibrium'?

  When the rate of the forward reaction is equal to the rate of the backward reaction.
• What is a dynamic equilibrium?

  Both forward and backward reactions are happening but there is no overall affect, because they are at the same rate- products is breaking down as quickly as it is formed.

  No overall change in the concentrations of the reactants or products.
• What conditions is required for a reaction to reach equilibrium?

  Must take place in a closed system where nothing enters or leaves.
• What does it mean is the position of equilibrium lies to the right?

  The concentration of the products is greater than reactants.
• What does it mean if the position of equilibrium lies to the left?

  Concentration of reactants is much greater than concentration of products
• Does equilibrium mean the concentration of products and reactants are equal?


  No, equilibrium mat lie to the left or right and tell us which has the greater concentration.
• What 3 factors alter the position of equilibrium?

  Concentration of reactants and products, temperature, pressure (only for gases.)