Thermodynamics of Natural Systems Theory and Applications in Geochemistry and Environmental Science

This book is intended as an introduction to thermodynamics. To give instructors the option of including other aspects of particular thermodynamic topics, several chapters and sections from the second edition (Anderson, 2005) are available on the Cambridge University Press website for this book, www.cambridge.org/thermodynamics.

These sections are as follows.

At appropriate places in the text, reference to the additional information available online is noted in a box like this, on page 154:

Equations of State

The ideal gas equation P V = nRT or PV = RT is an equation of state; an equation relating the volume of an ideal gas to its pressure and temperature. For real gases there have been many modifications of this equation, and there are other equations of state which interrelate not only P, V, and T, but also thermodynamic parameters such as enthalpy, Gibbs energy, and entropy. See Chapter 13 Equations of State, in the online material.

Other boxes add worked examples or more details of the material in the text. For example on page 21 there is this:

Scientific vs. Engineering Units

In science, molar properties, such as molar volumes and molar energies, are most commonly used. In engineering, on the other hand, specific properties are more common. Specific properties are mass-related rather than mole-related. Thus the specific volume of water at 25 ◦C is 1.0029 cm3 g-1. Molar and specific properties are related by the molar mass (or so-called gram formula weight, gfw) of the substance. That for water is 18.0153 gmol-1, so 1.0029 cm3 g-1 × 18.0153 gmol-1 = 18.068 cm3 mol-1.

Exercises and Additional Problems

Exercises

At the end of each chapter there is a set of exercises on the material in that chapter under the heading Exercises. These are intended to be done by students as an aid to understanding, and the answers are in Appendix C.