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Compound thermodynamically

Selected Values of Properties of Chemical Compounds, Thermodynamic Research Center, Texas A M Research Foundation, College Station, Texas (continuing). [Pg.12]

Pure carbon disulfide is a clear, colorless Hquid with a deHcate etherHke odor. A faint yellow color slowly develops upon exposure to sunlight. Low-grade commercial carbon disulfide may display some color and may have a strong, foul odor because of sulfurous impurities. Carbon disulfide is slightly miscible with water, but it is a good solvent for many organic compounds. Thermodynamic constants (1), vapor pressure (1,2), spectral transmission (3,4), and other properties (1,2,5—7) of carbon disulfide have been deterrnined. Principal properties are Hsted in Table 1. [Pg.26]

Compiled from Daubert, T. E., R. R Danner, H. M. Sibul, and C. C. Stebbins, DIPPR Data Compilation of Pure Compound Properties, Project 801 Sponsor Release, July, 1993, Design Institute for Physical Property Data, AlChE, New York, NY and from Thermodynamics Research Center, Selected Values of Properties of Hydrocarbons and Related Compounds, Thermodynamics Research Center Hydrocarbon Project, Texas A M University, College Station, Texas (extant 1994). [Pg.98]

J. B. Pedley, Thermochemical Data and Structures of Organic Compounds, (Thermodynamics Research Center, College Station, TX, 1994). [Pg.211]

Equilibrium vapor pressures were measured in this study by means of a mass spectrometer/target collection apparatus. Analysis of the temperature dependence of the pressure of each intermetallic yielded heats and entropies of sublimation. Combination of these measured values with corresponding parameters for sublimation of elemental Pu enabled calculation of thermodynamic properties of formation of each condensed phase. Previ ly reported results on the subornation of the PuRu phase and the Pu-Pt and Pu-Ru systems are correlated with current research on the PuOs and Pulr compounds. Thermodynamic properties determined for these Pu-intermetallics are compared to analogous parameters of other actinide compounds in order to establish bonding trends and to test theoretical predictions. [Pg.104]

Low-temperature solid-state synthesis is preferred in most cases, where appropriate, for obvious reasons such as energy and cost economy and process safety or for critical concerns regarding the accessibility of compounds that are stable only at low temperatures or non-equilibrium phases, i.e., compounds thermodynamically unstable with respect to the obtained phase (e.g., a ternary instead of binary phase). The use of low-temperature eutectics as solvents for the reactants, hydrothermal growth... [Pg.26]

Amidon, G.L., Anik, S.T. (1980) Hydrophobicity of polycyclic aromatic compounds. Thermodynamic partitioning analysis. J. Phys. Chem. 84, 970-974. [Pg.900]

Zwolinski, B. J. and R. C. Wilhoit, VAPOR PRESSURES AND HEATS OF VAPORIZATION OF HYDROCARBONS AND RELATED COMPOUNDS. Thermodynamic Research Center, TAMU, College Station, TX (1971). [Pg.2]

The internal energy per unit mass e is an intensive (state) function. Enthalpy h, a compound thermodynamic function defined by Equation 1.8, is also an intensive function. [Pg.10]

Dolfing J (1998) Halogenation of Aromatic Compounds Thermodynamic, Mechanistic and Ecological Aspects. FEMS Microbiol Lett 167 271... [Pg.488]

Biochemical Actions of Plant Phenolics Compounds Thermodynamic and Kinetic Aspects... [Pg.91]

Selected Values of Properties of Hydrocarbons and Related Compounds Thermodynamics Research Center Hydrocarbon Project, API 44 Tables. College Station, TX Thermodynamics Research Center. [Pg.427]


See other pages where Compound thermodynamically is mentioned: [Pg.249]    [Pg.462]    [Pg.60]    [Pg.255]    [Pg.251]    [Pg.727]   


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