Chemical Equilibrium: Le Chatelier's Principle?

📌 CONCEPT: Le Chatelier's principle states that when a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the equilibrium will shift in a direction that tends to counteract the effect of the change.

📐 RULE / FORMULA: According to Le Chatelier's principle, the addition of a catalyst to a reversible reaction will not affect the equilibrium constant (Kc), as a catalyst increases the rate of both forward and reverse reactions, leaving the equilibrium position unchanged.

💡 WORKED EXAMPLE: Consider the reversible reaction: N2O4 ⇌ 2NO2. If a catalyst is added to the reaction mixture, the equilibrium will remain the same, and the equilibrium constant (Kc) will not change, as the catalyst increases the rate of both the forward and reverse reactions.

⚠️ COMMON MISTAKE: Students often mistakenly believe that the addition of a catalyst will shift the equilibrium to the product side, but in reality, the equilibrium remains the same, and the catalyst only increases the rate of the reaction.