The Properties of Real Gases

Part of the Handbuch der Physik / Encyclopedia of Physics book series (HDBPHYS, volume 3 / 12)


The following symbols are used for the principal thermodynamic functions: E (energy), H (heat content), S (entropy), A (Helmholtz free-energy), G (Gibbs free-energy).


Pure Substance Virial Coefficient Residual Function Coexistence Curve Critical Constant 
These keywords were added by machine and not by the authors. This process is experimental and the keywords may be updated as the learning algorithm improves.


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General references

  1. [1]
    Beattie, J. A., and W. H. Stockmayer: A Treatise on Physical Chemistry, Vol. 2, Chap. 2, p. 187–290 (ed. H. S. Taylor and S. Glasstone). New York: Van Nostrand 1951. — An account of the thermodynamic properties of gases, principally in terms of the Beattie-Bridgeman equation.Google Scholar
  2. [2]
    Din, F.: The thermodynamic functions of gases, Vol. 1, Ammonia, Carbon monoxide, Carbon dioxide; Vol. 2, Air, Propane, Acetylene, Ethylene, Argon. London: Butterworth 1956. — A critical compilation of all the experimental results presented in the form of smoothed tables and graphs. It covers all three phases for each pure substance.Google Scholar
  3. [3]
    Justi, E.: Spezifische Wärme, Enthalpie, Entropie und Dissoziation technischer Gase. Berlin: Springer 1938. — This book covers the calculation of the thermodynamic properties of perfect gases from quantum theory, and the empirical calculation of the properties of real gases. It includes many tables of results.Google Scholar
  4. [4]
    Keesom, W. H.: Helium, Chap. 2. Amsterdam: Elsevier 1942. This chapter gives experimental details of, for example, the Leiden gas-apparatus, which are relevant to gases other than helium. There is a discussion of the velocity of sound in an imperfect gas and of the use of helium in gas thermometers.Google Scholar
  5. [5]
    Keyes, F. G.: Proc. Amer. Acad. Arts Sci. 68, 505–564 (1933). Methods and Procedures used in the Massachusetts Institute of Technology program of investigation of the pressure and volume of water to 460 C.Google Scholar
  6. J. A. Beattie: Proc. Amer. Acad. Arts Sci. 69, 389–405 (1934). The apparatus and method used for the measurement of the compressibility of several gases in the range 0 to 325 C. — Amongst the apparatus described is a much-copied type of dead-weight gauge.Google Scholar
  7. [6]
    Kobe, K. A., and R. E. Lynn: Chem. Rev. 52, 117–236 (1953). The critical properties of elements and compounds. — A review of all work up to 1953 with recommendations of “best” values, and brief descriptions of apparatus.Google Scholar
  8. [7]
    Michels, A., and C. Michels: Proc. Roy. Soc. A 153, 201–213 (1935). Isotherms of CO2 between 0 and 150° C and pressures from 16 to 250 atm.Google Scholar
  9. A. Michels, C. Michels and H. Wouters: Proc. Roy. Soc. Lond., Ser. A 153, 214–224 (1935). Isotherms of CO2 between 70 and 3000 atm. — These papers describe the apparatus used at Amsterdam for the last twenty years, and also give an account of the Amagat system of units.Google Scholar
  10. [8]
    National Bureau of Standards: Tables of Thermal Properties of Gases, Circular 564 (ed. J. Hilsenrath and others). Washington 1955. — These tables cover air, argon, carbon dioxide, carbon monoxide, hydrogen, nitrogen, oxygen and steam. The maximum pressure is only 100 atm but the temperature range is extended to temperatures up to 3000 K by making theoretical, but reliable, extrapolations.Google Scholar
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    Newitt, D. M.: The design of high pressure plant and the properties of fluids at high pressures. Oxford, England: Clarendon Press 1940. — A full account of experimental methods, and of the thermodynamic and transport properties of compressed gases and liquids.Google Scholar
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    Partington, J. R.: An advanced treatise on Physical Chemistry, Vol. 1, The Properties of Gases, Sect. VIIA—E, p. 546–848. London: Longmans 1949. — This is principally useful for its references to the early history of the subject.Google Scholar
  13. [11]
    Rowlinson, J. S.: Trans. Faraday Soc. 51, 1317–1326 (1955).The reduced equation of state. — A smoothed table of the compressibility factor for the inert gases as a function of reduced temperature and reduced density. The table may also be used for calculating Z for other gases. A similar table with reduced pressure as the second variable is given by K. S. Pitzer, D. Z. Lippman, R. F. Curl, C. M. Huggins and D. E. Peterson: J. Amer. Chem. Soc. 77, 3433 (1955).Google Scholar
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    Thermodynamic and Transport Properties of Fluids. London: Inst. Mech. Engng. (in the press). — The proceedings of an international conference held in London in July 1957 by the Institution of Mechanical Engineers and the International Union of Pure and Applied Chemistry.Google Scholar

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© Springer-Verlag OHG. Berlin · Göttingen · Heidelberg 1958

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