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Introduction to Equilibrium

Chemical equilibrium occurs when a reversible reaction reaches a state where the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant over time.

Key Concepts​

  • Dynamic Equilibrium: Reactions continue, but no net change in concentrations
  • Equilibrium Constant (K): Expresses the ratio of product to reactant concentrations at equilibrium
    • For aA + bB ⇌ cC + dD: K = [C]^c [D]^d / [A]^a [B]^b
  • Reaction Quotient (Q): Used to predict the direction a reaction will shift
    • Q < K → reaction shifts forward
    • Q > K → reaction shifts reverse
    • Q = K → reaction is at equilibrium

Importance​

  • Predicts composition of chemical mixtures at equilibrium
  • Helps in industrial processes like the Haber process
  • Explains effects of concentration, pressure, and temperature on reactions (Le Chatelier’s Principle)

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