Equilibrium
Class 11 Chemistry · Chemistry Part I · Chapter 6
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Summary
This unit develops the idea of equilibrium for both physical and chemical systems. Physical equilibria — solid-liquid, liquid-vapour, solid-vapour and the dissolution of solids and gases in liquids (Henry's law) — are dynamic, with opposing processes proceeding at equal rates in a closed system so that measurable properties stay constant. Chemical equilibrium is likewise dynamic, demonstrated by the Haber synthesis of ammonia and by isotope-scrambling experiments. The law of chemical equilibrium (the law of mass action of Guldberg and Waage) gives the equilibrium constant \(K_c\) as the ratio of product to reactant concentrations each raised to its stoichiometric coefficient. For gaseous reactions \(K_p\) is used, with \(K_p=K_c(RT)^{\Delta n}\); pure solids and liquids are omitted from heterogeneous equilibrium constants. The magnitude of \(K\) indicates the extent of a reaction, while the reaction quotient \(Q\) predicts the direction of net change. Equilibrium connects to thermodynamics through \(\Delta G^{\circ}=-RT\ln K\). Le Chatelier's principle explains how concentration, pressure, temperature and catalysts affect equilibrium, a catalyst speeding both directions equally without shifting the position. The unit then turns to ionic equilibrium: strong and weak electrolytes; the Arrhenius, Brønsted-Lowry (conjugate acid-base pairs) and Lewis concepts of acids and bases; ionisation of acids and bases; the ionic product of water \(K_w=1\times10^{-14}\), the pH scale, buffer solutions and solubility product.
Equilibrium in physical processes and Henry's lawDynamic chemical equilibriumLaw of mass action and equilibrium constantKp-Kc relationship and heterogeneous equilibriaReaction quotient and Gibbs energyLe Chatelier's principleAcid-base concepts and conjugate pairsIonic product of water and pH scaleBuffers and solubility product
Key terms
Dynamic equilibrium
A state in which the forward and reverse processes occur at equal rates, so concentrations remain constant though both processes continue.
Equilibrium constant
The constant ratio of product to reactant concentrations, each raised to its stoichiometric coefficient, at a given temperature.
Reaction quotient
The same expression as the equilibrium constant but evaluated for non-equilibrium concentrations; comparing it with \(K\) predicts the reaction direction.
Le Chatelier's principle
When a system at equilibrium is disturbed, it shifts so as to counteract the imposed change.
Conjugate acid-base pair
A Brønsted acid and base related by the gain or loss of a single proton.
Ionic product of water
The constant \(K_w=[H^+][OH^-]=1\times10^{-14}\) at 298 K for the self-ionisation of water.
Extra questions & answers
Try one from this chapter
At dynamic equilibrium, the rates of the forward and reverse reactions are: