Effect of a Catalyst

Introduction:

• Adding a catalyst to a reaction at equilibrium does not change the position of equilibrium.
• However, it facilitates the attainment of equilibrium more quickly and at lower temperatures, making reactions more efficient and economically viable.

Catalyst and Equilibrium

• Consider a reversible reaction at equilibrium:
• A + B ⇌ C + D
• When a catalyst is added to this equilibrium system, it increases the rates of both the forward and backward reactions.

Rate Enhancement with Catalyst

• The catalyst lowers the activation energy required for both the forward and reverse reactions.
• This reduction in activation energy leads to a proportional increase in the rates of both reactions.
• Consequently, the equilibrium position remains unaffected by the catalyst.

Benefits of Using Catalysts

• Catalysts enable reactions to reach equilibrium more rapidly, saving time and energy.
• They allow equilibrium to be established at lower temperatures, making reactions more cost-effective and environmentally friendly.
• Catalysts play a crucial role in industrial processes by improving reaction efficiency without altering the final equilibrium composition.

Conclusion

• While catalysts do not change the position of equilibrium, they significantly enhance the rate at which equilibrium is achieved.
• The use of catalysts is a key strategy in chemistry to make reactions more efficient and economically viable.