Reversible reactions

• Reversible reactions will reach equilibrium:

  • At equilibrium, both reactions are Stilll happening, but there is no overall effect, which means the concentration Of reactants and products have reached a balance and won't change
  • Equilibrium is only reached if the reversible reaction takes place in a Closed system
• The position of equilibrium can be on the right or left

  • when a reactions at equilibrium it doesn't mean the amounts of reactants and products are equal
  • If the equilibrium lies to the right the concentration of products is greater than that of the reactants
  • If the equilibrium lies to the left, the concentration of reactants is greater than that of the products
• Reversible reactions can be endothermic or exothermic
• Le Chatelier's Principle


  If you change the conditions of a reversible reaction at equilibrium, the system will try to counteract that change
• Temperature change


  If you decrease the temperature, the equilibrium will move in the exothermic direction to produce more heat, meaning you'll get more products for that reaction
• Pressure change


  Only effects equilibrium containing gas. If you increase the pressure, equilibrium tries to reduce it by moving in the direction where there are fewer gas molecules
• Concentration change


  If you increase the concentration of the reactants, the system tries to decrease it by making more products