Changing Concentration

Changing Concentration

Introduction:

• In a chemical equilibrium, the rates of the forward and reverse reactions are equal, resulting in a dynamic balance.
• Altering the concentration of reactants or products can shift the position of equilibrium.

Increasing Reactant Concentration

• If you increase the concentration of reactants, the equilibrium position shifts to the right, favouring the formation of products.
• This is because the reaction tries to consume the excess reactants to reestablish equilibrium.

Decreasing Product Concentration

• If you decrease the concentration of products, the equilibrium position shifts to the right as well.
• This happens because the reaction tries to produce more products to make up for the reduced concentration.

Decreasing Reactant Concentration

• Conversely, decreasing the concentration of reactants will shift the equilibrium position to the left, favouring the formation of more reactants.
• The reaction tries to replenish the reduced reactant concentration.

Increasing Product Concentration

• Increasing the concentration of products will also shift the equilibrium position to the left.
• The reaction aims to consume the excess products to restore equilibrium.

Conclusion

• Changing the concentration of reactants or products in a chemical equilibrium can shift the equilibrium position.
• The equilibrium position shifts to counteract the change and reestablish a new equilibrium that maintains dynamic balance in the reaction.