S HORT C ONTENTS
Preface to the Second Edition
From the Preface to the First Edition
2 Systems and Their Properties
3 The First Law
4 The Second Law
5 Thermodynamic Potentials
6 The Third Law and Cryogenics
7 Pure Substances in Single Phases
8 Phase Transitions and Equilibria of Pure Substances
10 Electrolyte Solutions
11 Reactions and Other Chemical Processes
12 Equilibrium Conditions in Multicomponent Systems
13 The Phase Rule and Phase Diagrams
14 Galvanic Cells
Appendix A Deﬁnitions of the SI Base Units
P REFACE TO THE S ECOND E DITION
This second edition of Thermodynamics and Chemistry is a revised and enlarged version
of the ﬁrst edition published by Prentice Hall in 2001. The book is designed primarily as a
textbook for a one-semester course for graduate or undergraduate students who have already
been introduced to thermodynamics in a physical chemistry course.
The PDF ﬁle of this book contains hyperlinks to pages, sections, equations, tables,
ﬁgures, bibliography items, and problems. If you are viewing the PDF on a computer
screen, tablet, or color e-reader, the links are colored in blue.
Scattered through the text are sixteen one-page biographical sketches of some of the
historical giants of thermodynamics. A list is given on the preceding page. The sketches
are not intended to be comprehensive biographies, but rather to illustrate the human side of
thermodynamics—the struggles and controversies by which the concepts and experimental
methodology of the subject were developed.
The epigraphs on page 18 are intended to suggest the nature and importance of classical thermodynamics. You may wonder about the conversation between Alice and Humpty
Dumpty. Its point, particularly important in the study of thermodynamics, is the need to pay
attention to deﬁnitions—the intended meanings of words.
I welcome comments and suggestions for improving this book. My e-mail address appears below.
F ROM THE P REFACE TO THE F IRST
Classical thermodynamics, the subject of this book, is concerned with macroscopic aspects of the
interaction of matter with energy in its various forms. This book is designed as a text for a onesemester course for senior undergraduate or graduate students who have already been introduced to
thermodynamics in an undergraduate physical chemistry course.
Anyone who studies and uses thermodynamics knows that a deep understanding of this subject
does not come easily. There are subtleties and interconnections that are difﬁcult to grasp at ﬁrst. The
more times one goes through a thermodynamics course (as a student or a teacher), the more insight
one gains. Thus, this text will reinforce and extend the knowledge gained from an earlier exposure
to thermodynamics. To this end, there is fairly intense discussion of some basic topics, such as the
nature of spontaneous and reversible processes, and inclusion of a number of advanced topics, such
as the reduction of bomb calorimetry measurements to standard-state conditions.
This book makes no claim to be an exhaustive treatment of thermodynamics. It concentrates
on derivations of fundamental relations starting with the thermodynamic laws and on applications
of these relations in various areas of interest to chemists. Although classical thermodynamics treats
matter from a purely macroscopic viewpoint, the book discusses connections with molecular properties when appropriate.
In deriving equations, I have strived for rigor, clarity, and a minimum of mathematical complexity. I have attempted to clearly state the conditions under which each theoretical relation is valid
because only by understanding the assumptions and limitations of a derivation can one know when
to use the relation and how to adapt it for special purposes. I have taken care to be consistent in the
use of symbols for physical properties. The choice of symbols follows the current recommendations
of the International Union of Pure and Applied Chemistry (IUPAC) with a few exceptions made to
I owe much to J. Arthur Campbell, Luke E. Steiner, and William Mofﬁtt, gifted teachers who
introduced me to the elegant logic and practical utility of thermodynamics. I am immensely grateful
to my wife Stephanie for her continued encouragement and patience during the period this book
went from concept to reality.
I would also like to acknowledge the help of the following reviewers: James L. Copeland,
Kansas State University; Lee Hansen, Brigham Young University; Reed Howald, Montana State
University–Bozeman; David W. Larsen, University of Missouri–St. Louis; Mark Ondrias, University
of New Mexico; Philip H. Rieger, Brown University; Leslie Schwartz, St. John Fisher College; Allan
L. Smith, Drexel University; and Paul E. Smith, Kansas State University.
A theory is the more impressive the greater the simplicity of its
premises is, the more different kinds of things it relates, and the more
extended is its area of applicability. Therefore the deep impression
which classical thermodynamics made upon me. It is the only physical
theory of universal content concerning which I am convinced that,
within the framework of the applicability of its basic concepts, it will
never be overthrown.
Thermodynamics is a discipline that involves a formalization of a large
number of intuitive concepts derived from common experience.
J. G. Kirkwood and I. Oppenheim, Chemical Thermodynamics, 1961
The ﬁrst law of thermodynamics is nothing more than the principle of
the conservation of energy applied to phenomena involving the
production or absorption of heat.
Max Planck, Treatise on Thermodynamics, 1922
The law that entropy always increases—the second law of
thermodynamics—holds, I think, the supreme position among the laws
of Nature. If someone points out to you that your pet theory of the
universe is in disagreement with Maxwell’s equations—then so much
the worse for Maxwell’s equations. If it is found to be contradicted by
observation—well, these experimentalists do bungle things sometimes.
But if your theory is found to be against the second law of
thermodynamics I can give you no hope; there is nothing for it but to
collapse in deepest humiliation.
Sir Arthur Eddington, The Nature of the Physical World, 1928
Thermodynamics is a collection of useful relations between quantities,
every one of which is independently measurable. What do such
relations “tell one” about one’s system, or in other words what do we
learn from thermodynamics about the microscopic explanations of
macroscopic changes? Nothing whatever. What then is the use of
thermodynamics? Thermodynamics is useful precisely because some
quantities are easier to measure than others, and that is all.
M. L. McGlashan, J. Chem. Educ., 43, 226–232 (1966)
“When I use a word,” Humpty Dumpty said, in rather a scornful tone,
“it means just what I choose it to mean—neither more nor less.”
“The question is,” said Alice,“whether you can make words mean
so many different things.”
“The question is,” said Humpty Dumpty, “which is to be master—
Lewis Carroll, Through the Looking-Glass
C HAPTER 1
Thermodynamics is a quantitative subject. It allows us to derive relations between the
values of numerous physical quantities. Some physical quantities, such as a mole fraction,
are dimensionless; the value of one of these quantities is a pure number. Most quantities,
however, are not dimensionless and their values must include one or more units. This
chapter reviews the SI system of units, which are the preferred units in science applications.
The chapter then discusses some useful mathematical manipulations of physical quantities
using quantity calculus, and certain general aspects of dimensional analysis.
There is international agreement that the units used for physical quantities in science and
technology should be those of the International System of Units, or SI (standing for the
French Syst` me International d’Unit´ s). The Physical Chemistry Division of the Intere
national Union of Pure and Applied Chemistry, or IUPAC, produces a manual of recommended symbols and terminology for physical quantities and units based on the SI. The
manual has become known as the Green Book (from the color of its cover) and is referred
to here as the IUPAC Green Book. This book will, with a few exceptions, use symbols recommended in the third edition (2007) of the IUPAC Green Book;1 these symbols are listed
for convenient reference in Appendices C and D.
The SI is built on the seven base units listed in Table 1.1 on the next page. These base
units are independent physical quantities that are sufﬁcient to describe all other physical
quantities. One of the seven quantities, luminous intensity, is not used in this book and is
usually not needed in thermodynamics. The ofﬁcial deﬁnitions of the base units are given
in Appendix A.
Table 1.2 lists derived units for some additional physical quantities used in thermodynamics. The derived units have exact deﬁnitions in terms of SI base units, as given in the
last column of the table.
The units listed in Table 1.3 are sometimes used in thermodynamics but are not part
of the SI. They do, however, have exact deﬁnitions in terms of SI units and so offer no
problems of numerical conversion to or from SI units.
. The references are listed in the Bibliography at the back of the book.
C HAPTER 2
S YSTEMS AND T HEIR P ROPERTIES
This chapter begins by explaining some basic terminology of thermodynamics. It discusses
macroscopic properties of matter in general and properties distinguishing different physical
states of matter in particular. Virial equations of state of a pure gas are introduced. The
chapter goes on to discuss some basic macroscopic properties and their measurement. Finally, several important concepts needed in later chapters are described: thermodynamic
states and state functions, independent and dependent variables, processes, and internal energy.
2.1 THE SYSTEM, SURROUNDINGS, AND BOUNDARY
Chemists are interested in systems containing matter—that which has mass and occupies
physical space. Classical thermodynamics looks at macroscopic aspects of matter. It deals
with the properties of aggregates of vast numbers of microscopic particles (molecules,
atoms, and ions). The macroscopic viewpoint, in fact, treats matter as a continuous material medium rather than as the collection of discrete microscopic particles we know are
actually present. Although this book is an exposition of classical thermodynamics, at times
it will point out connections between macroscopic properties and molecular structure and
A thermodynamic system is any three-dimensional region of physical space on which
we wish to focus our attention. Usually we consider only one system at a time and call it
simply “the system.” The rest of the physical universe constitutes the surroundings of the
The boundary is the closed three-dimensional surface that encloses the system and
separates it from the surroundings. The boundary may (and usually does) coincide with
real physical surfaces: the interface between two phases, the inner or outer surface of the
wall of a ﬂask or other vessel, and so on. Alternatively, part or all of the boundary may be
an imagined intangible surface in space, unrelated to any physical structure. The size and
shape of the system, as deﬁned by its boundary, may change in time. In short, our choice of
the three-dimensional region that constitutes the system is arbitrary—but it is essential that
we know exactly what this choice is.
We usually think of the system as a part of the physical universe that we are able to
inﬂuence only indirectly through its interaction with the surroundings, and the surroundings