6.2 - Changing the conditions of equilibrium

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  • 6.2 - Changing the conditions of an equilibrium Reaction
    • Changing Proportion
      • If there are more products in an equilibrium mixture, it means that equilibrium moves to the right. Therefore the reaction goes in the forward direction.
      • If the proportion of reactants is increased, the equilibrium moves to the left, and the reaction occurs in the opposite / reverse direction.
    • Changing Concentration
      • If you increases the concentration of one of the reactants, the equilibrium shifts in the direction that reduces the concentration of the reactant.
    • Changing Pressure
      • Pressure changes only affect gaseous reactions. Increasing a pressure of a gas means more molecules are in a given volume, meaning the concentration essentially changes
    • Increasing Temperature
      • Endothermic Reactions
        • This will go in the opposite direction of an exothermic reaction, but the direction of the reaction is all that changes.. And if the mixture is heated, it will cool down to oppose the change.
      • Exothermic Reactions
        • If you increase the temperature of an exothermic reaction in the forward direction, this means that equilibrium must shift to left in order to cool the system down.
          • Then if there are more reactants, the equilibrium shifts to the right in order to make a higher yield of the products too.
    • Adding Catalysts
      • This has no effect on where the equilibrium goes or shifts as they only produce an alternative route for the reaction. Meaning the products and reactants will still have equal yields.


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