Basic Chemical Thermodynamics

Höfundur: E Brian Smith (Útgáfa: 6)
Basic Chemical Thermodynamics

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This widely acclaimed text, now in its sixth edition and translated into many languages, continues to present a clear, simple and concise introduction to chemical thermodynamics. An examination of equilibrium in the everyday world of mechanical objects provides a starting point for an accessible account of the factors that determine equilibrium in chemical systems. This straightforward approach leads students to a thorough understanding of the basic principles of thermodynamics, which are then applied to a wide range of physical chemical systems.

The book also discusses the problems of non-ideal solutions and the concept of activity, and provides an introduction to the molecular basis of thermodynamics. Over six editions, the views of teachers of the subject and their students have been incorporated. Reference to the phase rule has been included in this edition and the notation has been revised to conform to current IUPAC recommendations. Students taking courses in thermodynamics will continue to find this popular book an excellent introductory text.

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Útgefandi
World Scientific Publishing
ISBN
9781783263387
Print ISBN
9781783263356
Format
ePub
Útgáfa
6
Höfundar
E Brian Smith
Tungumál
English
Útgefið
10/04/2013
Prent takmörkun á líftíma
100
Prent takmörkun
2
Afritunar takmörkun
2

Kaflar

  • Cover
  • Halftitle
  • Title
  • Copyright
  • Preface
  • Preface
  • Contents
  • Notation
  • 1 Introduction
  • 1.1 The scope and nature of chemical thermodynamics
  • 1.2 Equilibrium in mechanical systems
  • 1.3 Reversibility and equilibrium
  • 1.4 Why we need thermodynamics
  • 1.5 The mole
  • 1.6 The perfect gas
  • 2 Energy
  • 2.1 Work
  • 2.2 Heat and temperature
  • 2.3 Measurement of temperature
  • 2.4 Heat and molecular motion
  • 2.5 Conservation of energy
  • 2.6 State functions: a digression
  • 2.7 Enthalpy
  • 2.8 Heat capacity
  • Problems
  • 3 Entropy and equilibrium
  • 3.1 Reversibility and equilibrium: a recapitulation
  • 3.2 Condition of equilibrium
  • 3.3 Entropy
  • 3.4 Entropy as a state function
  • 3.5 Entropy of expansion of a gas
  • 3.6 Entropy changes accompanying heat flow
  • 3.7 Entropy and equilibrium
  • 3.8 A cosmological aside
  • 3.9 Entropy as a function of pressure and temperature
  • 3.10   Molecular basis of entropy
  • 3.11   Statistical basis of the Second Law
  • 3.12   Magnitudes of entropy changes
  • 3.13   Heat engines
  • Problems
  • 4 Equilibrium in chemical systems
  • 4.1 Free energy
  • 4.2 Gibbs energy
  • 4.3 Pressure-dependence of Gibbs energy
  • 4.4 Temperature variation of Gibbs energy
  • 4.5 Phase equilibria
  • 4.6 Clapeyron equation
  • 4.7 Clausius–Clapeyron equation
  • 4.8 The vapour pressure of liquids
  • 4.9 Chemical potential
  • 4.10   Chemical potential and Gibbs energy
  • 4.11   Equilibrium between gaseous reactants
  • 4.12   Temperature-dependence of equilibrium constants
  • 4.13   Effect of pressure on equilibrium constants
  • 4.14   Basic results of chemical thermodynamics
  • 4.15   Le Chatelier’s Principle
  • Problems
  • 5 Determination of thermodynamic quantities
  • 5.1 Hess’s Law
  • 5.2 Standard enthalpies of formation
  • 5.3 Average bond energies
  • 5.4 Temperature-dependence of enthalpy changes
  • 5.5 Standard Gibbs energies of formation
  • 5.6 Determination of Gibbs energy changes
  • 5.7 Determination of entropies of substances
  • 5.8 Example of the determination of thermodynamic quantities
  • 5.9 Calculation of thermodynamic quantities at temperatures other than 298 K
  • 5.10   Ellingham diagrams
  • 5.11   Free-energy functions
  • Problems
  • 6 Ideal solutions
  • 6.1 The ideal solution
  • 6.2 Properties of truly ideal solutions
  • 6.3 Mixtures of liquids
  • 6.4 Ideal solutions of solids in liquids
  • 6.5 Ideal dilute solutions
  • 6.6 Colligative properties
  • 6.7 Freezing-point depression
  • 6.8 Elevation of boiling point
  • 6.9 Osmotic pressure
  • 6.10   Properties of the solute in dilute solutions
  • 6.11   Solubility of solids
  • Problems
  • 7 Non-ideal solutions
  • 7.1 The concept of activity
  • 7.2 Activity of solids in liquids
  • 7.3 Activity in aqueous solutions
  • 7.4 Chemical equilibria in solution
  • 7.5 Electrochemical cells
  • 7.6 Standard electrode potentials
  • Problems
  • 8 Thermodynamics of gases
  • 8.1 Expansion of a perfect gas
  • 8.2 Irreversible expansion
  • 8.3 Equation of state of gases
  • 8.4 The Joule–Thomson experiment
  • 8.5 Imperfect gases: fugacity
  • 8.6 Calculation of fugacities
  • Problems
  • 9 The molecular basis of thermodynamics
  • 9.1 Energy levels
  • 9.2 Microstates.160
  • 9.3 The Boltzmann factor
  • 9.4 The behaviour of heat capacity
  • 9.5 Partition functions
  • 9.6 Entropy and the partition function
  • 9.7 Calculation of the translational partition function
  • 9.8 The rotational partition function
  • 9.9 The vibrational partition function
  • 9.10   Evaluation of the thermodynamic properties of gaseous nitrogen
  • 9.11   Chemical equilibrium
  • Problems
  • Answers to problems
  • Further reading
  • Appendix 1: Thermochemical data at 298.15K
  • Appendix 2: Thermodynamic data for ions in aqueous solution at 298.15K
  • Appendix 3: Units and fundamental constants
  • Periodic table of elements
  • Index