Connection Map

EQUILIBRIUM (PC-06)
       │
       ├──► THERMODYNAMICS
       │     • $\Delta G$° = −RT ln K (links Gibbs energy to equilibrium)
       │     • Spontaneity: $\Delta G$ < 0 when Q < K (reaction proceeds forward)
       │     • Van't Hoff equation: d(ln K)/dT = $\Delta H$°/$RT^{2}$
       │
       ├──► ELECTROCHEMISTRY
       │     • Nernst equation: E = E° − (RT/nF)ln Q
       │     • At equilibrium Q = K: E = 0; E° = (RT/nF)ln K
       │     • Ka of weak electrolytes related to conductivity (Kohlrausch)
       │
       ├──► IONIC EQUILIBRIUM ↔ QUALITATIVE ANALYSIS (OC)
       │     • Ksp controls precipitation in Group analysis ($H_{2}S$ groups)
       │     • Buffer principles used in dye chemistry and protein chemistry
       │
       ├──► INDUSTRIAL CHEMISTRY
       │     • Haber process ($N_{2}$ + $3H_{2}$ ⇌ $2NH_{3}$): optimising yield using Le Chatelier
       │     • Contact process ($2SO_{2}$ + $O_{2}$ ⇌ $2SO_{3}$): compromise temperature ~450°C
       │     • Ammonia → $HNO_{3}$ (Ostwald process) — multi-equilibrium cascade
       │
       ├──► CHEMICAL KINETICS
       │     • K_eq = kf/kb (ratio of rate constants at equilibrium)
       │     • Catalyst lowers Ea for both directions equally → same K but faster
       │
       └──► SOLUTIONS & COLLIGATIVE PROPERTIES
             • Degree of dissociation α used in Van't Hoff factor i
             • i = 1 + α(n−1) for electrolytes; links to osmotic pressure