Chem 390. Physical Chemistry II. Spring 2007. Physical Chemistry II. Chem 390.
Review outline for Prelim I. The first Prelim is on Thursday, February 15, ...
Physical Chemistry II
Chem 390
Spring 2007
Physical Chemistry II Chem 390 Review outline for Prelim I The first Prelim is on Thursday, February 15, 7:30-9:00 pm, Ives Hall East 305. This exam will cover material from Chapters 16 & 19 of McQ&S, as described below. You may use a calculator that does not have an alphanumeric keyboard. Devices that store text or that have infrared transmitters are not permitted. 1. Properties of gases Chapter 16 • Basic vocabulary of thermodynamics: thermodynamic state; state functions; intensive and extensive state variables. • Ideal gas equation of state and neglect of intermolecular forces. • Qualitative description of attractive and repulsive intermolecular forces. • Isotherms of an actual gas. Liquid/vapor coexistence. Liquid/vapor critical point. • Significance of compressibility factor Z. • Improving the IGES: van der Waals equation of state. Significance of a and b parameters. Determining a and b from laboratory data. • Improving the IGES: virial equation of state. T -dependence of B2 (T ) and Boyle temperature. 2. First Law of thermodynamics Chapter 19 • Universe = system + surroundings + boundary. • Mechanical definition of work. Thermodynamic definition of work. • Definition of a reversible process. w for isothermal reversible expansion or compression. • δw is an inexact differential. • Definition of heat flow q. • δq is an inexact differential. Mechanical equivalence of heat. • First Law: dU = δq + δw is an exact differential. ∆U = q + w. • Thermodynamic and statistical thermodynamical definitions of U . Molecular interpretation of δw = −pdV and δq. • Processes at constant volume: ∆U = qV . Definition of CV = dqV /dT = (∂U/∂T )V . • Applying the First Law to irreversible and reversible adiabatic processes. • Measurement of ∆U with bomb calorimetry. • Processes at constant pressure. ∆H = qp , H = U + pV . • Determination of ∆H. • Dependence of H on T . Definition of Cp = dqp /dT = (∂H/∂T )p . Relation between Cp and CV : ideal gas; general case. • Thermochemistry. H is a state function. Hess’s law. Known values of ∆H can be used to compute unknown ones.
