book reviews Introduction to Chemical Thermodynamics
William G. Douies, St. Mary's College, South Bend, Indiana. W. B. Saunders Ca., Philadelphia, 1972. vi 301 pp. Figs. and tables. 14.3 X 22.6 cm. $4.95.
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Davies has restricted himself to the molecular and thermodynamic concepts necessary t o understanding chemical equilihrium. Within this constraint, or perhaps as a result of it, the concepts are developed exceedingly well. The hook is written far freshmen. It is not meant to develop the concepts rigorously, rather to make them plausible. In the reviewer's opinion it could be used successfully a t the freshman level and also as supplementary reading a t a more advanced level. Presuming only an elementary knowledge of descriptive chemistry and equilihrium constants the subject matter is developed until, a t the end, a reader is ahle not only to use tables of thermodynamic data to predict the equilibrium constants far many chemical reactions but has a sufficient understanding of quantum-statistical-thermodynamic theory that he can understand why the chemical systems behave as they do and make semi-quantitative predictions when thermodynamic data is lacking. For example, using only a table of bond energies and a knowledge of the molecular contributions to entropy, he should he ahle to predict the equilibrium
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constant for the reaction cyclopentane(g) = 1-pentene(g) with reasonable accuracy and predict its temperature dependence. The f m t four chapters are devoted to statistical and quantum concepts and especially how they affect equilibrium. The mathematics of probability is developed as needed. The spacing of translational, rotational, vibrational, and electronic energy levels is analyzed with the aid of the de Broglie wave equation, and minimal mathematics. The presentation is clear and the examples are completely worked. The only criticism I would make of this section is that the Baltzmann distribution law is plucked from the body of "too advanced material for this book" whereas it is a simple matter, using distributions in countable microstates, to show the form which the distribution must have. The thermodynamic state functions relevant to chemical equilibrium a t constant pressure, are developed in succeeding, chapters, first from a molecular point of view and then by showing their relationship to classical thermodynamic heat and work. The effects of energy and entropy on equilibrium are introduced in semiquantitative terms and followed by a very lucid explanation of how and why free energy approaches a minimum as a chemical reaction approaches equilibrium. The discussion of the second law of thermodynamics is very abbreviated. The concept of reversibility and irreversibility is avoided. The usual restriction of reversibility in the relationship between q and A S in an isothermal process is dropped in favor of the
statement "providing a Boltzmann distrihutian is maintained." This reviewer feels the h w k is a very successful attempt t o integrate mlcroscopic concepts, thermodynamic concepts, and equilibrium. For many teachers a major drawback to the book will be that its scope is too limited-essentially, after 300 pages, one arrives a t a very good understanding of gas phase chemical equilibrium but of no other phenomena. As far as this book is concerned ionic equilibria in solution, electrochemistry, and the host of other topics of physleal chemistry which are illuminated by thermodynamics do not exist. Robert C. Plumb Worcester Polytechnic Institute Worcester, Massachusetts 01609
Electron Spin Resonance: Elementary Theory and Practical Applications John E. Wertr, University of Minnesota, and James R. Bolton, University of Western Ontario. McGraw-Hill Book Co., New York, 1972. xiv + 497 pp. Figs. and tables. 23.5 X 17.5 cm. $22.50. Although a number of books on electron spin resonance spectroscopy (esr) exist none has been completely suitable as an introductory text. This new hook seems clearly destined to fill the need. The suhti(Continued onpogeA114)
