Thermodynamic Properties of Propylene

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

Temperature K Pressure MPa Density mol/dm3 Volume dm3/mol Int. energy kj/mol Enthalpy kj/mol Entropy kJ/(mol-K) Cv kJ/(mol-K) cr kJ/(mol K) Sound speed m/s Joule-Thomson K/MPa 

The values in these tables were generated from the NIST REFPROP software (Lemmon, E. VV, 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 Angus, S., Armstrong, B., and de Reuck, K. M., International Thermodynamic Tables of the Fluid State—7 Propylene, International Union of Pure and Applied Chemistry, Pergamon Press, Oxford, 1980. Validated equations for the viscosity and thermal conductivity are not currently available for this fluid. 

The uncertainties of the equation of state are generally 0.1% in density (except in the critical region), 1% in the heat capacity in the vapor phase, and 2-5% in the heat capacity in the liquid phase. 

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HP he study of the behavior of electrolytes in mixed solvents is currently arousing considerable interest because of its practical and fundamental implications (1). Among the simpler binary solvent mixtures, those where water is one component are obviously of primary importance. We have recently compared the effects of small quantities of water on the thermodynamic properties of selected 1 1 electrolytes in sulfolane, acetonitrile, propylene carbonate, and dimethylsulfoxide (DMSO). These four compounds belong to the dipolar aprotic (DPA) class of solvents that has received a great deal of attention (2) because of their wide use as media for physical separations and chemical and electrochemical reactions. We interpreted our vapor pressure, calorimetry, and NMR results in terms of preferential solvation of small cations and anions by water and obtained... 

ETHYLENE-PROPYLENE COPOLYMER. THERMODYNAMIC PROPERTIES OF POLYMERS - PART 4. 

Silva, L. B. Freitas, L. C. G., Structural and Thermodynamic Properties of Liquid Ethylene Carbonate and Propylene Carbonate by Monte Carlo Simulations. J. Mol. Stmct.-Theochem 2007, 806, 23-34. 

Properties. Propylene is an olefin hydrocarbon that is a gas under ambient conditions bnt is normally stored as a liquid under pressin-e. The physical properties of propylene are given in Table 1. Thermodynamic properties are widely reported in the literature. Vapor-liquid equilibria of mixtures of propylene with other hydrocarbons and hydrogen are accurately represented by correlations for hydrocarbon mixtnres, such as the Chao-Seader correlation. 

Ravdel BA, Pozin MY, Tikhonov KI, Rotinyan AL (1987) Thermodynamic Properties of the Electrochemical Cell Li I L1C104 (Propylene Carbonate) I LixMn02. Sov Electrochem 23 1459-1464... 

Lam, S. Y Benoit, R. L. Some thermodynamic properties of the dimediylsulfoxide-water and propylene carbonate-water systems at 25.deg.C. Can. J. Chem. 1974, 52, 718-722. 

We are interested in the thermodynamic properties of a strip of rubber as it is stretched (see below). Consider n moles ofpure ethylene propylene rubber (EPR) that has an unstretched length Zq-If it is stretched by applying a force F, it will obtain an equilibrium length z, given by ... 

Propylene oxide is a colorless, low hoiling (34.2°C) liquid. Table 1 lists general physical properties Table 2 provides equations for temperature variation on some thermodynamic functions. Vapor—liquid equilibrium data for binary mixtures of propylene oxide and other chemicals of commercial importance ate available. References for binary mixtures include 1,2-propanediol (14), water (7,8,15), 1,2-dichloropropane [78-87-5] (16), 2-propanol [67-63-0] (17), 2-methyl-2-pentene [625-27-4] (18), methyl formate [107-31-3] (19), acetaldehyde [75-07-0] (17), methanol [67-56-1] (20), ptopanal [123-38-6] (16), 1-phenylethanol [60-12-8] (21), and / /f-butanol [75-65-0] (22,23). 

Figure 11-29. Enthalpies of propylene for liquid and vapor. (Used by permission Starling, K. E. Fluid Thermodynamic Properties for Light Petroleum Systems, 1973. Gulf Publishing Co., Houston, Texas. All rights reserved.)...

Propylene conversion over three SAPO molecular sieves (SAPO-5, SAPO-11, and SAPO-34) was conducted at a variety of operating conditions. Catalyst behavior was correlated with the physical and chemical properties of the SAPO molecular sieves. The objective of this work was to determine the relative importance of kinetic and thermodynamic factors on the conversion of propylene and the distribution of products. The rate of olefin cracldng compared to the rate of olefin polymerization will be addressed to account for the observed trends in the product yields. The processes responsible for deactivation will also be addressed. 

Most highly polar and ionic species are not amenable to processing with desirable solvents such as carbon dioxide or any other solvent such as water that has a higher critical temperature well above the decomposition temperature of many solutes. In such instances, the combination of the unique properties of supercritical fluids with those of micro-emulsions can be used to increase the range of applications of supercritical fluids. The resulting thermodynamically stable systems generally contain water, a surfactant and a supercritical fluid (as opposed to a non-polar liquid in liquid micro-emulsions). The possible supercritical fluids that could be used in these systems include carbon dioxide, ethylene, ethane, propane, propylene, n-butane, and n-pentane while many ionic and non-ionic surfactants can be used. The major difference between the liquid based emulsions and the supercritical ones is the effect of pressure. The pressure affects the miscibility gaps as well as the microstracture of the micro-emulsion phase. 

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