Fundamental Equilibrium Concepts (Chemistry)

Recall cards on the fundamentals of chemical equilibrium: reversible reactions and dynamic equilibrium (equal forward and reverse rates, constant concentrations, the double arrow); the reaction quotient Q and the equilibrium constant K (the concentration form Qc and the pressure form Qp, the law of mass action, what large and small K values mean, using Q versus K to predict reaction direction, the relation Kp = Kc(RT)^delta-n, and homogeneous versus heterogeneous equilibria with pure solids and liquids omitted); manipulating equilibrium constants for reversed, multiplied, and combined reactions; Le Chatelier's principle (how concentration, pressure-volume, and temperature changes shift an equilibrium, why a catalyst does not, and the Haber process and carbonated-drink examples); and equilibrium calculations with ICE tables, the quadratic formula, and the small-K approximation.