Chapter 10. Chemical Equilibrium

At equilibrium, forward and reverse rates are equal and concentrations are constant. For aA + bB ⇌ cC + dD:

K = [C]ᶜ[D]ᵈ / ([A]ᵃ[B]ᵇ)

Pure solids and liquids are omitted. Compare the reaction quotient Q with K: if Q < K the reaction proceeds forward; if Q > K, in reverse.

Le Châtelier’s principle: a system disturbed from equilibrium shifts to counteract the change (concentration, pressure/volume, temperature). Only temperature changes alter K [1][2].

ICE tables (Initial, Change, Equilibrium) organize calculations. K_sp describes sparingly soluble salts; for AgCl, K_sp = [Ag⁺][Cl⁻] [9].

Review: For N₂ + 3H₂ ⇌ 2NH₃ (exothermic), how does raising temperature affect K?