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Published: 4 June 2021
Last updated: 31 January 2023

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1

Gabriel, Stoltz, and Rousset Mathias, eds. Free energy computations: A mathematical perspective. New Jersey: Imperial College Press, 2010.

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2

Hu, Ningcheng. Collection of papers to restudy the Gibbs free energy. Sichuan, China: [s.n.], 1991.

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3

Ch, Chipot, and Pohorille A, eds. Free energy calculations: Theory and applications in chemistry and biology. New York: Springer, 2007.

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4

Hill, Terrell L. Free energy transduction and biochemical cycle kinetics. New York: Springer-Verlag, 1989.

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5

Reddy, M. Rami, and Mark D. Erion. Free energy calculations in rational drug design. New York: Springer, 2011.

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6

Hemingway, Bruce S. Enthalpy and Gibbs energy of formation of dolomite, CaMg(COb3s)b2s, at 298.15 K from HCl solution calorimetry. [Reston, Va.]: U.S. Dept. of the Interior, U.S. Geological Survey, 1994.

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7

Sophia, Figarova, and SpringerLink (Online service), eds. Thermodynamics, Gibbs Method and Statistical Physics of Electron Gases: Gibbs Method and Statistical Physics of Electron Gases. Berlin, Heidelberg: Springer-Verlag Berlin Heidelberg, 2010.

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8

Flynn, Harry Eugene. Experimental verification of the use of free-energy minimization techniques for modelling complex sulfide smelting. Ann Arbor, MI: University Microfilms International, 1988.

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9

Isham, M. A. Gibbs free energy of reactions involving SiC, Si3N4, H2, and H20 as a function of temperature and pressure. Huntsville, Ala: George C. Marshall Space Flight Center, 1992.

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10

Josephs, Barry D. Gaseous chemical reaction equilibrium: Application of the Gibbs free energy to closed batch or steady state gaseous reaction systems and derivation procedures for the chemical equilibrium constant. 2nd ed. Salem, Mass: Higginson Book Co., 2010.

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11

Josephs, Barry D. Gaseous chemical reaction equilibrium: Application of the Gibbs free energy to closed batch or steady state gaseous reaction systems and derivation procedures for the chemical equilibrium constant. Salem, Massachusetts: Published by Higginson Book Company, 2012.

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12

Josephs, Barry D. Gaseous chemical reaction equilibrium: Application of the Gibbs free energy to closed batch or steady state gaseous reaction systems and derivation procedures for the chemical equilibrium constant. 4th ed. Salem, Mass: Higginson Book Co., 2012.

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13

Josephs, Barry D. Gaseous chemical reaction equilibrium: Application of the Gibbs free energy to closed btch or steady state gaseous reaction systems and derivation procedures for the chemical equilibrium constant. 3rd ed. Salem, Mass: Higginson Book Co., 2011.

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14

The properties of solvents. Chichester: Wiley, 1998.

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15

Sherwood, Dennis, and Paul Dalby. Free energy. Oxford University Press, 2018. http://dx.doi.org/10.1093/oso/9780198782957.003.0013.

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A critical chapter, explaining how the principles of thermodynamics can be applied to real systems. The central concept is the Gibbs free energy, which is explored in depth, with many examples. Specific topics addressed are: Spontaneous changes in closed systems. Definitions and mathematical properties of Gibbs free energy and Helmholtz free energy. Enthalpy- and entropy-driven reactions. Maximum available work. Coupled reactions, and how to make non-spontaneous changes happen, with examples such as tidying a room, life, and global warming. Standard Gibbs free energies. Mixtures, partial molar quantities and the chemical potential.
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16

(Editor), Christophe Chipot, and Andrew Pohorille (Editor), eds. Free Energy Calculations: Theory and Applications in Chemistry and Biology (Springer Series in Chemical Physics). Springer, 2007.

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17

Chipot, Christophe, and Andrew Pohorille. Free Energy Calculations: Theory and Applications in Chemistry and Biology. Springer London, Limited, 2007.

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18

Free Energy Transduction and Biochemical Cycle Kinetics. Springer, 2011.

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19

Hill, Terrell L. Free Energy Transduction and Biochemical Cycle Kinetics. Springer London, Limited, 2012.

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20

Hill, Terrell L. Free Energy Transduction and Biochemical Cycle Kinetics. Dover Publications, 2004.

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21

Hill, Terrell L. Free Energy Transduction and Biochemical Cycle Kinetics. Dover Publications, Incorporated, 2013.

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22

Hill, Terrell L. Free Energy Transduction and Biochemical Cycle Kinetics. Dover Publications, Incorporated, 2013.

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23

(Editor), M. Rami Reddy, and Mark D. Erion (Editor), eds. Free Energy Calculations in Rational Drug Design. Springer, 2001.

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24

M, Rami Reddy, and Erion Mark D, eds. Free energy calculations in rational drug design. New York: Kluwer Academic/Plenum Publishers, 2001.

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25

Figarova, Sophia, and Bahram M. Askerov. Thermodynamics, Gibbs Method and Statistical Physics of Electron Gases. Springer Berlin / Heidelberg, 2012.

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26

Varada, Raj Subramanium, Walker K. P, and United States. National Aeronautics and Space Administration., eds. Stress versus temperature dependent activation energies in creep. [Washington, D.C.]: NASA, 1990.

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27

United States. National Aeronautics and Space Administration., ed. Computation of kinetics for the hydrogen/oxygen system using the thermodynamic method. [Washington, D.C: National Aeronautics and Space Administration, 1996.

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28

Gibbs free energy of reactions involving SiC, SiN, H, and HO as a function of temperature and pressure. [Washington, DC]: National Aeronautics and Space Administration, Office of Management, Scientific and Technical Information Program, 1992.

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29

Composition dependence of the M, temperature in the Ý'NiAl compound. Washington, DC: National Aeronautics and Space Administration, 1988.

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30

Sherwood, Dennis, and Paul Dalby. Chemical equilibrium and chemical kinetics. Oxford University Press, 2018. http://dx.doi.org/10.1093/oso/9780198782957.003.0014.

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Building on the previous chapter, this chapter examines gas phase chemical equilibrium, and the equilibrium constant. This chapter takes a rigorous, yet very clear, ‘first principles’ approach, expressing the total Gibbs free energy of a reaction mixture at any time as the sum of the instantaneous Gibbs free energies of each component, as expressed in terms of the extent-of-reaction. The equilibrium reaction mixture is then defined as the point at which the total system Gibbs free energy is a minimum, from which concepts such as the equilibrium constant emerge. The chapter also explores the temperature dependence of equilibrium, this being one example of Le Chatelier’s principle. Finally, the chapter links thermodynamics to chemical kinetics by showing how the equilibrium constant is the ratio of the forward and backward rate constants. We also introduce the Arrhenius equation, closing with a discussion of the overall effect of temperature on chemical equilibrium.
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31

Sherwood, Dennis, and Paul Dalby. Phase equilibria. Oxford University Press, 2018. http://dx.doi.org/10.1093/oso/9780198782957.003.0015.

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This chapter extends the discussion of gas phase equilibria to phase equilibria. The central concept is the vapour pressure, and the key proof is that the criterion for phase equilibrium is the equality of the molar Gibbs free energies, or chemical potentials, of each phase. This then leads to the Clapeyron and Clausius-Clapeyron equations. A notable feature of this chapter is the discussion of non-ideal gases, answering the question “Given that, by definition, an ideal gas can never liquefy, what is it about a real gas that enables the gas to change phase into a liquid?”. A unique feature of this discussion is the rigorous analysis of the Gibbs free energy of a van der Waals gas under compression, and the proof of the ‘Maxwell construction’.
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32

Sherwood, Dennis, and Paul Dalby. Macromolecular conformations and interactions. Oxford University Press, 2018. http://dx.doi.org/10.1093/oso/9780198782957.003.0025.

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As a polymer of many amino acids, any given protein can, in principle, adopt a huge number of configurations. In reality, however, the biologically stable protein adopts a single configuration that is stable over time. Thermodynamically, this configuration must represent a Gibbs free energy minimum. This chapter therefore explores how the thermodynamics and kinetics of protein folding and unfolding can be investigated experimentally (using, for example, chaotropes, heating or ligand interactions), and how these measurements can be used to enrich our understanding of protein configurations and stability.
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33

Horing, Norman J. Morgenstern. Quantum Mechanical Ensemble Averages and Statistical Thermodynamics. Oxford University Press, 2018. http://dx.doi.org/10.1093/oso/9780198791942.003.0006.

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Chapter 6 introduces quantum-mechanical ensemble theory by proving the asymptotic equivalence of the quantum-mechanical, microcanonical ensemble average with the quantum grand canonical ensemble average for many-particle systems, based on the method of Darwin and Fowler. The procedures involved identify the grand partition function, entropy and other statistical thermodynamic variables, including the grand potential, Helmholtz free energy, thermodynamic potential, Gibbs free energy, Enthalpy and their relations in accordance with the fundamental laws of thermodynamics. Accompanying saddle-point integrations define temperature (inverse thermal energy) and chemical potential (Fermi energy). The concomitant emergence of quantum statistical mechanics and Bose–Einstein and Fermi–Dirac distribution functions are discussed in detail (including Bose condensation). The magnetic moment is derived from the Helmholtz free energy and is expressed in terms of a one-particle retarded Green’s function with an imaginary time argument related to inverse thermal energy. This is employed in a discussion of diamagnetism and the de Haas-van Alphen effect.
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