Thermodynamic Properties of Fluorine

Temperature Pressure Density Volume Int. energy Enthalpy Entropy C CT Sound speed Joule-Thomson 

The values in these tables were generated from the NIST REFPROP software (Lemmon, E.W., McLinden, M.O., and Huber, M.L., NIST Standard Reference Database 23 Reference Fluid Thermodynamic and Transport Properties—REFPROP, National Institute of Standards and Technology, Standard Reference Data Program, Gaithersburg, Md., 2002, Version 7.1). The primary source for the thermodynamic properties is de Reuck, K. M., International Thermodynamic Tables of the Fluid State—11 Fluorine, International Union of Pure and Applied Chemistry, Pergamon Press, Oxford, 1990. Validated equations for the viscosity and thermal conductivity are not currently available for this fluid. 

The uncertainties of the equation of state are 0.2% in density, 2% in heat capacity, and 1.5% in the speed of sound, except in the critical region. 

Proprietary name for a series of fluorocarbons produced by the Imperial Smelting Corp., Avonmouth, Bristol, UK. Bulletins of thermodynamic properties include PP1 (C6F14), PP2 (C7F14), PP3 (C8F16), PP5 (C10F18), PP9 (CuF ), and PP50, usually for 6.1-100 kg/m2,0-500°C. See also Green, S. W., Chem. ir Ind. (1969) 63-67. 

A series of fire-extinguishing fluids. Halon 1211 is produced by ICI, and Halon 1301, by duPont, the latter issuing a bulletin with thermodynamic properties and a diagram for the range 0.6-600 psia, -160-460°F. 

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J. D. Cox, H. A. Gundry, A. J. Head. Thermodynamic Properties of Fluorine Compounds. Part 1. Heats of Combustion ofp-Fluorobenzoic Acid, Pentafluorobenzoic Acid, Hexafluorobenzene, and Decafluorocyclohexene. Trans. Faraday Soc. 1964, 60, 653-665. 

Ambrose, D., Ellender, J.H., Sprake, C.H.S., Townsend, R. (1975) Thermodynamic properties of fluorine compounds. Part 15.- Vapour pressures of the three tetrafluorobenzenes and l,3,5-trichloro-2,4,6-trifluorobenzene. J. Chem. Soc. Faraday. Tram. 171, 35—41. 

Counsell, J.F., Green, J.H.S., Hales, J.L., Martin, J.F. (1965) Thermodynamic properties of fluorine compounds. Part 2.—Physical and thermodynamic properties of hexafluorobenzene. Trans. Faraday Soc. 61, 212-218. 

Andon RJL, Counsel JF, Hales JL, Lees EB, Martin JF (1968) Thermodynamic properties of fluorine compounds. Part VII. Heat capacity and entropy of penta fluoro chlorobenzene and pentailuorophenol. J. Chem. Soc. A 2357... 

Data published on thermodynamic properties of fluorinated surfactants are scarce. Shinoda and Hutchinson [42] treated the micelle as a separate pseudophase of very small dimensions. The phase-separation model describes the micelle as a separate phase which begins to form at cmc. If micelle formation is analogous to phase separation, the heat and entropy of micellization can be calculated from the temperature dependence of the activities of micelle-forming species. 

Because of the extreme difficulty in handling fluorine, reported physical properties (Table 1) show greater than normal variations among investigators. A detailed summary and correlation of the physical, thermodynamic, transport, and electromagnetic properties of fluorine is given in Reference 20. 

I. Tomaszkiewicz, G. A. Hope, C. M. Beck II, P. A. G. O Hare. Thermodynamic Properties of Silicides. VI. Pentamolybdenum Trisilicide (Mo Sf). Fluorine Combustion Calorimetric Determination of the Standard Molar Enthalpy of Formation at the Temperature of 298.15 K. J. Chem. Thermodynamics 1997, 29, 87-98. 

O Hare, P.A.G. (1993) Calorimetric measurements of the specific energies of reaction of arsenic and of selenium with fluorine. Standard molar enthalpies of formation Af7/°m at the temperature 2.98.15 K of AsFs, SeF6, As2Se3, AS4S4, and As2S3. Thermodynamic properties of AsFs and SeF6 in the ideal-gas state. Critical assessment of AfH°m (AsF3, 1)), and the dissociation enthalpies of As-F bonds. Journal of Chemical Thermodynamics, 25, 391-402. 

Benning, A.F., McHamess, R.C. (1940) Thermodynamic properties of fluorochloromethanes and ethanes. Ind. Eng. Chem. 32,497-499. Beyerlein, A.L., DesMarteau, D.D., Kul, I., Zhao, G. (1998) Properties of novel fluorinated compounds and their mixtures as alternative refrigerants. Fluid Phase Equilibria 150-151, 287-296. 

L. V. Gurvich, I. V. Veyts, and C. B. Alcock, Thermodynamic Properties of Individual Substances, Vol. 1 Elements Oxygen, Hydrogen (Deuterium, Tritium), Fluorine, Chlorine, Bromine, Iodine, Helium, Neon, Argon, Krypton, Xenon, Radon, Sulfur, Nitrogen, Phosphorus, and Their Compounds, Pt. 1 Methods and Computation, Hemisphere, New York, 1989. 

Properties of Fluorine Compounds. Part 2 Physical and Thermodynamic Properties of Hexafluorobenzene, Trans. Faraday Soc. 1965, 61, 212-218. 

THERMODYNAMIC FUNCTIONS OF FLUORINATED BENZOLS IN IDEAL-GAS STATE. FROM TEPLOFIZICHESKIE SOVOISTVA VESHCHESTVI MATERIALOV. /THERMOPHYSICAL PROPERTIES OF SUBSTANCES AND MATERIALS, VOLUME 2/. 

These equations indicate the way in which the thermodynamic properties of the system change with the composition. In a blend of polymers, new interactions can be created which are not present in the homopolymer system. For instance, polar groups can induce dipoles or quadrupoles that will increase the interaction energy between the polymer chains and can change the entropy of the system. Such interactions explain the unusual properties obtained when fluorine atoms are present in a polymer system. 

Determination of the basic thermodynamic properties of the rare earth trifluorides remains incomplete. This is in part due to experimental difficulties, and only one direct calorimetric measurement has been reported. The enthalpy of formation, AH 29s, of YF3 (-410.7 0.8 kcal/mole) has been measured by fluorine bomb calorimetry (Rudzitis et al., 1965). In an expansion of earlier work, Polyachenok (1967) has obtained values for several trifluorides (La, Pr, Nd, Gd, Er) by an equilibrium exchange reaction RCbi -f-A1F3( ->RF3(0 +AICl3(g). Solid state emf data have been reported by Skelton and Patterson (1973) for the trifluorides of Nd, Gd, Dy and Er. Similar measurements have been described by Rezukhina et al. (1974) for the trifluorides of La, Pr and Y. The AHt-m values are 5-10 kcal/mole more negative than values reported earlier. 

Polt, A. Maurer, G. (1992). The Bender equation of state for describing thermodynamic properties of krypton, neon, fluorine, sulfur dioxide and water over a wide range of state. Fluid Phase Equil, 73,27-38. 

This observation was expanded into a thermodynamic argument [42] for the prediction of exfoliation of montmorillonite as a function of the surface treatment and the hydrophilic-hydrophobic balance of the polymer continuous phase. More work needs to be done in matching the hydrophilic-hydrophobic balance of fluorinated polymers with the hydrophilic-hydrophobic balance of the organomontmorillonite in order to achieve full exfoliation of the montmorillonite in the polymer. Full exfoliation of the montmorillonite in the polymer will allow for a valid examination of the mechanical properties of fluorinated polymer-montmorillonite composites in relation to the theory of reinforcement developed in Chapter 5. 

Nevertheless, the system, composed of chain fragments of oxyfluoroniobate complexes, is thermodynamically less stable. Dipole properties of fragments of a certain length are re-orientated so as to be linked into typical infinite chains. There is no doubt that the fragment re-orientation and linking process initiates the partial reduction of niobium to Nb4+ and the oxidation of fluoride to elementary fluorine. The process scheme can be presented as follows ... 

Thermodynamic properties for explosion calculations are presented for major organic chemical compounds. The thermodynamic properties include enthalpy of formation, Gibbs free energy of formation, internal energy of formation and Helmholtz free energy of formation. The major chemicals include hydrocarbon, oxygen, nitrogen, sulfur, fluorine, chlorine, bromine, iodine and other compound types. 

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