Thermodynamic data for

American Petroleum Institute, Bibliographies on Hydrocarbons, Vols. 1-4, "Vapor-Liquid Equilibrium Data for Hydrocarbon Systems" (1963), "Vapor Pressure Data for Hydrocarbons" (1964), "Volumetric and Thermodynamic Data for Pure Hydrocarbons and Their Mixtures" (1964), "Vapor-Liquid Equilibrium Data for Hydrocarbon-Nonhydrocarbon Gas Systems" (1964), API, Division of Refining, Washington. 

Maczynski, A. "Thermodynamic Data for Technology—Verified Vapor-Liquid Equilibrium Data," Panstwowe Wydawnictwo Naukawa, Warsaw, Volume 1, 1976 Volume 2, 1978. 

Table 3. Thermodynamic Data for Crystalline Aluminum Hydroxides at 298.15K and 0.1 MPa ...

B. D. Smith and R. Srivastava, Thermodynamic Data for Pure Compounds Part A.. Hydrocarbons and Ketones, Elsevier, Amsterdam, the Netherlands, 1986. T. Boubhk, V. Eried, and E. Hala, The Hapour Pressures of Pure Substances, 2nd ed., Elsevier, Amsterdam, the Netherlands, 1984. 

Table 2. Thermodynamic Data for Carbon Monoxide (Ideal Gas) b ...

Each reactant and product appears in the Nemst equation raised to its stoichiometric power. Thermodynamic data for cell potentials have been compiled and graphed (3) as a function of pH. Such graphs are known as Pourbaix diagrams, and are valuable for the study of corrosion, electro deposition, and other phenomena in aqueous solutions.Erom the above thermodynamic analysis, the cell potential can be related to the Gibbs energy change... 

The thermodynamic data for the oxidation (combustion) of the normal and iso-paraffins (alkanes), C2H2 +2, can be represented to within a few kilojoules by the equation... 

The basic thermodynamic data for the design of such reactions can be used to assess the dissociation energies for various degrees of dissociation, and to calculate, approximately, tire relevant equilibrium constants. One important source of dissociation is by heating molecules to elevated temperamres. The data below show the general trend in the thermal dissociation energies of a number of important gaseous molecules. 

The above data are correct to about 20 kJ mole but it will be seen that the general trend among these more covalent bonds does appear to be a decrease in stability from carbon to silicon, i.e. the same way as was found for more ionic bonds in the halides. Thermodynamic data for metallorganic methyl compounds used in the produchon of semiconductor systems are shown in Table 2.3. 

The thermodynamic data for the formation of the IVB diborides together with the coiTespotrditrg hydrogen halides are as follows ... 

Table 4.2 Thermodynamic data for ideal reforming reactions...

Appendix Thermodynamic data for the Gibbs energy of formation of metal oxides... 

It should be remarked that a detailed study of the elimination of mairganese and silicon from the liquid metal shows that silicon together with some of the mairganese is hrst removed, followed by tire rest of the manganese together with some of the carbon, which is hnally removed together widr half of the sulphur contained in the original liquid. This sequence is in accord with what would be expected from thermodynamic data for the stabilities of dre oxides. 

The use of a gas mixture presents a two-part problem. If the state of the mixture is such that it may be considered a mixture of perfect gases, classical thermodynamic methods can be applied to determine the state of each gas constituent. If, however, the state of the mixture is such that the mixture and constituents deviate from the perfect gas laws, other methods must be used that recognize this deviation. In any case, it is important that accurate thermodynamic data for the gases are used. 

If the thermodynamic data for a compound of interest have not been determined and abulated, it may be possible to estimate AHf or AGj from tabulated data pertaining to dividual structural units. Procedures have been developed for estimating thermodynamic characteristics of hydrocarbons and derivatives by summing the contributions of the constituent groups. The group increments are derived from experimental thermochemical iata and therefore depend on the existence of reliable data for the class of compounds of merest. 

It has been possible to obtain thermodynamic data for the ionization of alkyl chlorides by reaction with SbFs, a Lewis acid, in the nonnucleophilic solvent S02C1F. It has been foimd that the solvation energies of the carbocations in this medium are small and do not differ much from one another, making comparison of the nonisomeric systems possible. As long as subsequent reactions of the carbocation can be avoided, the thermodynamic characteristics of this reaction provide a measure of the relative ease of carbocation formation in solution. 

Equation (6.3.15) is not accurate for the calculation of explosion energy of vessels filled with real gases or superheated liquids. A better measure in these cases is the work that can be performed on surrounding air by the expanding fluid, as calculated from thermodynamic data for the fluid. In this section, a method will be described for calculating this energy, which can then be applied to the basic method in order to determine the blast parameters. 

If the fluid is not listed in Table 6.12 or Figure 6.30, thermodynamic data for the fluid at its initial and final (expanded to ambient pressure) states are needed as well. These data include the properties of the fluid ... 

Van Nuys [75] gives excellent thermodynamic data for HCl. Figure 9-87 gives the equilibrium for the 100% HCl gas feed in an adiabatic tower, and Table 9-45 summarizes performance for two concentrations of feed gas. From the data it can be seen that it requires fewer theoretical plates to make 32% acid from 10% feed gas than from 100% gas and at the same time yield a vent containing only 0.01 weight% HCl. 

Some Thermodynamic Data for Idealized Reactions of Importance in Catalytic Cracking... 

Trustworthy thermodynamic data for metal solutions have been very scarce until recently,25 and even now they are accumulating only slowly because of the severe experimental difficulties associated with their measurement. Thermodynamic activities of the component of a metallic solution may be measured by high-temperature galvanic cells,44 by the measurement of the vapor pressure of the individual components, or by equilibration of the metal system with a mixture of gases able to interact with one of the components in the metal.26 Usually, the activity of only one of the components in a binary metallic solution can be directly measured the activity of the other is calculated via the Gibbs-Duhem equation if the activity of the first has been measured over a sufficiently extensive range of composition. 

The thermodynamic data for the substances employed in lead-acid batteries are compiled in Table 4. 

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