Thermodynamics, like classical music, is an acquired taste. The initiation must be sensitively carried out, otherwise the mathematical rigour, like the formal structure of the music, acts to discourage a deeper relationship. It is sad but true that some students, both of thermodynamics and of Bach, never recover from the initial shock. In this, we are all losers. In this book, therefore, I have tried to pre sent thermodynamics in a way which uses little mathematics, but which includes many practical and lively examples. I hope it will provide a basis for an intro ductory course at Honours Degree level, and will also suffice for Higher National Diploma and Certificate students. In general, my aim has been to develop an understanding of Gibbs free energy fairly early on and then to apply this concept in several different fields. I have used many examples from chemical industry, in the firm belief that the basic usefulness of the subject must be demonstrated. I have therefore included a brief discussion of Ellingham diagrams in Chapter 10 and for a similar reason have omitted any mention of the Carnot cycle. I have used symbols consistent with the recommendations of the International Union of Pure and Applied Chemistry and have adopted units of the Systeme International d'Unites (SI).
Auflage
Softcover reprint of the original 1st ed. 1969
Sprache
Verlagsort
Zielgruppe
Für Beruf und Forschung
Research
Illustrationen
Maße
Höhe: 23.5 cm
Breite: 15.5 cm
Dicke: 8 mm
Gewicht
ISBN-13
978-94-010-5054-8 (9789401050548)
DOI
10.1007/978-94-011-2390-7
Schweitzer Klassifikation
1 Energy.- 1.1 The Realm of Thermodynamics.- 1.1.1 Energy Bookkeeping.- 1.1.2 Nature's Driving Forces.- 1.2 Setting the Scene; Basic Ideas.- 1.2.1 System and Surroundings.- 1.2.2 Functions of State.- 1.2.3 Mechanical Work and Expanding Gases.- 1.2.4 The Absolute Temperature Scale.- 1.3 Forms of Energy and Their Interconversion.- 2 The First Law Of Thermodynamics.- 2.1 Statement of the First Law.- 2.1.1 Reversible Expansion of an Ideal Gas.- 2.1.2 Constant Volume Processes.- 2.1.3 Constant Pressure Processes.- 2.2 A New Function-Enthalpy.- 2.2.1 Relationship between ?H and ?U.- 2.3 Uses and Conventions of ?H.- 2.3.1 Enthalpy Change of Reaction.- 2.3.2 Standard Enthalpies of Formation.- 3 Thermochemistry.- 3.1 Calorimetry.- 3.1.1 Bomb Calorimeters.- 3.2 Concepts of Heat Capacity.- 3.2.1 Combustion and Flame Temperatures.- 3.2.2 Variation of Reaction Enthalpies with Temperature.- 3.3 Bond Energies.- 3.3.1 Average Bond Dissociation Energies.- 4 Spontaneous Changes.- 4.1 Everyday Processes.- 4.2 Exothermicity, a Possible Criterion.- 4.2.1 Spontaneous Exothermic Processes.- 4.2.2 Spontaneous Processes Involving no Heat Change.- 4.2.3 Endothermic Processes.- 4.3 The Second Driving Force.- 5 Entropy.- 5.1 Measurement of Entropy.- 5.1.1 The Second Law of Thermodynamics.- 5.1.2 Reversibility and Entropy.- 5.1.3 Changes of Entropy with Temperature.- 5.1.4 An Adiabatic Compression.- 5.2 Absolute Entropies.- 5.2.1 The Third Law of Thermodynamics.- 5.2.2 ?S for Phase Changes.- 5.3 The Direction of Time.- 5.4 A Statistical Approach to Entropy.- 5.4.1 The Boltzmann Entropy Equation.- 5.4.2 Spectroscopic Entropies.- 6 Free Energy, The Arbiter.- 6.1 Processes in Isolated Systems.- 6.2 Gibbs Free Energy, G.- 6.3 Gibbs Free Energy and Maximum Work.- 6.4 Some Processes in Terms of Gibbs Free Energy.- 6.4.1 Adsorption Processes.- 6.4.2 Evaporation Phenomena.- 6.4.3 Endothermic Chemical Processes.- 6.5 Standard Free Energy Changes.- 7 Chemical Equilibrium.- 7.1 Preamble.- 7.2 Variation of G with Gas Pressure.- 7.2.1 Chemical Potential, ?.- 7.2.2 Pressure and Chemical Potential for Ideal Gases.- 7.2.3 Chemical Potential for Real Gases.- 7.2.4 Activity.- 7.3 The Active Mass of Pure Liquids and Solids.- 7.4 Activity of Materials in Solution.- 7.4.1 Solvents.- 7.4.2 Solutes or Minor Components.- 7.5 A Summing Up; Activity as a Unifying Concept.- 7.6 Practical Aspects of Activity.- 7.7 Equilibrium and the Reaction Isotherm.- 8 Equilibrium Experiments and Their Interpretation.- 8.1 The Reaction Isochore Equation.- 8.1.1 Le Chatelier up to Date.- 8.2 Applications of the Isochore Equation.- 8.2.1 Vaporization Processes.- 8.2.2 The Decomposition of the Compound UIn3.- 8.2.3 The High Temperature Dissociation of Water Vapour.- 8.3 The Clapeyron Equation.- 9 Electrochemistry.- 9.1 Electrochemical Cells.- 9.2 Cell Energetics.- 9.3 Standard Electrode Potentials.- 9.4 Variation of Cell e.m.f. with Activity.- 9.4.1 Ionic Activities.- 9.4.2 Analysis of e.m.f. Data to Find E0.- 9.5 Variation of e.m.f. with Temperature.- 10 Free Energy And Industrial Processes.- 10.1 Free Energies as a Function of Temperature.- 10.1.1 The Gibbs-Helmholtz Equation.- 10.1.2 The Integrated Form of the Gibbs-Helmholtz Equation.- 10.1.3 Tabulated Forms of Free Energy.- 10.2 The Synthesis of Ethanol.- 10.2.1 Equilibrium Calculations.- 10.2.2 Use of Activity Coefficients.- 10.3 Ellingham Diagrams.- 10.3.1 Corrosion Prevention.- 10.3.2 Electrolysis of Alumina.- 10.3.3 Thermal Reduction of Magnesia.- 10.3.4 Titanium and the Kroll Process.- Suggested Further Reading.- Appendix I: The Twenty Most Useful Equations.- Appendix II: Fundamental Constants and Conversion Factors.- Answers to Problems.
