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Physical Chemistry — Practice Set 5

Chemical equilibrium and electrochemistry: the equilibrium constant in its Kc, Kp, and Kx forms and their relation Kp = Kc(RT)^Δn, the reaction quotient Q and the direction of net change, heterogeneous equilibria and the exclusion of pure condensed phases, Le Chatelier's principle for changes of concentration, pressure, and temperature, the thermodynamic link ΔG° = −RT ln K and the van 't Hoff temperature dependence of K, acid–base equilibria (Ka, Kb, Kw, buffers and the Henderson–Hasselbalch equation) and solubility equilibria (Ksp and the common-ion effect), and electrochemistry from galvanic and electrolytic cells, standard electrode potentials and the SHE, cell notation and the salt bridge, the Nernst equation, ΔG° = −nFE° and ln K = nFE°/RT, Faraday's laws of electrolysis, and molar conductivity with Kohlrausch's law. Equations are shown in inline notation.