Premium · Question Bank

Physical Chemistry — Practice Set 6

Chemical kinetics: reaction rate and its relation to stoichiometry, rate laws and reaction order determined by experiment (initial-rates and pseudo-order methods), the units of the rate constant, and the integrated rate laws for zero-, first-, and second-order reactions with their characteristic linear plots and half-lives (including the concentration-independent first-order half-life), the temperature dependence of the rate constant through the Arrhenius equation k = Ae^(−Ea/RT), Arrhenius plots and the two-point form, activation energy and the reaction energy profile, reaction mechanisms (molecularity versus order, the rate-determining step, intermediates, the steady-state and pre-equilibrium approximations, and the transition state), theories of reaction rates (collision theory with the energy and steric requirements, transition-state theory, and diffusion control), and catalysis including homogeneous and heterogeneous catalysts, catalyst poisoning, and Michaelis–Menten enzyme kinetics with Vmax and KM. Equations are shown in inline notation.