lecture recording on 12 March 2025 at 11.12.13 AM

Chemical Equilibrium Overview

• Dynamic Equilibrium: State where forward and reverse reactions occur at equal rates, resulting in constant concentrations of reactants and products, though not necessarily equal amounts.

• Reversible Reactions: Most reactions can proceed in both directions (e.g., N₂O₄ ⇌ 2NO₂). Color changes can indicate progress toward equilibrium.

• Equilibrium Constants (K): For reactions at equilibrium, K is defined as the ratio of the concentration of products to reactants. A high K (>1) indicates a product-favored reaction, while a low K (<1) suggests a reactant-favored reaction.

• Reaction Quotient (Q): Compares current concentrations to K to determine the state of the system (at equilibrium if Q = K).

• Importance of K and Q: Vital for predicting shifts in reactions under changing conditions (Le Chatelier’s Principle).

• Practice: Understanding Q and K expressions is essential for mastering equilibrium concepts and predicting reaction behavior.