Equilibria

• Reversible reactions involve reactants forming products and products reforming reactants, represented by a double arrow.
• Dynamic equilibrium is reached when the forward and backward rates of reaction are the same, and concentrations of reactants and products remain constant.
• Le Chatelier's Principle predicts how an equilibrium mixture will change when reaction conditions are altered.
• Increasing temperature favors the endothermic reaction, while decreasing temperature favors the exothermic reaction.
• Increasing the concentration of reactants favors the production of products, while decreasing the concentration of products favors the reforming of reactants.
• The equilibrium constant (Kc) indicates the position of equilibrium for a reaction at a certain temperature.
• Increasing pressure favors the side of the reaction with fewer moles, while decreasing pressure favors the side with more moles.
• Catalysts do not affect the equilibrium position but allow equilibrium to be reached faster.
• Kc is calculated by dividing the concentration of products by the concentration of reactants, with the number of moles raised to a power.
• when we increase the temperature

  • Kc increases if forward reaction is endothermic
  • Kc decreases if forward reaction is exothermic