Thermodynamic Properties of Heptane

Temperature Pressure Density Volume Int. energy Enthalpy Entropy C, CF Sound speed Joule-Thomson Therm, cond. Viscosity 

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 Span, R., and Wagner, W., Equations of State for Technical Applications. II. Results for Nonpolar Fluids, Int.J. Thermophys., 24(1) 41-109,2003. The source for viscosity is NIST14, Version 9.08. The source for thermal conductivity is NIST14, Version 9.08. 

The uncertainties of the equation of state are approximately 0.2% (to 0.5% at high pressures) in density, 1% (in the vapor phase) to 2% in heat capacity, 1% (in the vapor phase) to 2% in the speed of sound, and 0.2% in vapor pressure, except in the critical region. For viscosity, estimated uncertainty is 2%. For thermal conductivity, estimated uncertainty, except near the critical region, is 4-6%. 

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Segovia, J. J. Martin, M. C. Chamorro, C. R. Villamanan, M. A. Excess thermodynamic properties of binary and ternary mixtures containing methyl 1,1-diinethylethyl ether (MTBE), n-heptane, and methanol at T = 313.15 K7. Chem. Thermodyn. 1999,31, 1231-1246... 

Thermodynamic properties of (n-alkoxyethanols + organic solvents). Xll. Tofed vapour pressure measurements for (n-hexane, n-heptane or cyclohexane -1- 2-methoxyethanol) at different temperatures J. Chem. Thermodyn. 2001,33,47-59... 

Thermodynamic properties of n-alkoxyethanols + organic solvent mixtures. XI. Toted vapor pressure measurements for n-hexane, cyclohexane or n-heptane + 2-ethoxyethanol at 303.15 emd 323.15 K7. Chem. Eng. Data 2000,45,699-703... 

R.K. Mitra, B.K. Pal, and S.P. Moulik 2006 Phase behavior, interfacial composition and thermodynamic properties of mixed surfactant (CTAB and Brij-58) derived w/o microemulsions with 1-butanol and 1-pentanol as cosurfactants and n-heptane and -decane as oils, J. Colloid Interf. Sci. 300, 755-764. 

Urdaneta, O. Handa, Y. P. Benson, G. C. Thermodynamic properties of binary mixtures containing ketones. V. Excess enthalpies of an isomeric heptanone + n-heptane J. Chem. Thermodyn. 1979,11, 857-860... 

Blanco, A. M. Ortega, J. Excess thermodynamic properties of rnixmres of alkyl benzoates with n-heptane Int. J. Thermophys. 1994,15, 699-710... 

Butcher, K. L. Ramasubramanian, K. R. Medani, M. S. Thermodynamic properties of the benzene and n-heptane system at elevated temperatures. J. Appl. Chem. Biotechnol. 1972, 22, 1139-1155. 

The optical purity of 91-93% was too low for downstream chemistry. The physical properties of 170 made enantiomeric enhancement by crystallization. The formation of a DABCO inclusion complex 171 in heptane and crystallization under thermodynamic control provided material that was 99% ee, 98% purity, and 79% recovery. This procedure produced 90 kg of 170, which was used to prepare an NK-1 receptor antagonist, Aprepitant (172), used for the treatment of chemotherapy-induced emesis.213... 

Already reported CAV/0 microemulsion technique was used to prepare the MLPs [12-15]. Briefly, this technique consists of an oil phase, a colloidal water phase, and surfactants and possesses specific physicochemical properties such as transparency, isotropy, and thermodynamic stability, n-Heptane was used as the oil phase, BrijSO as surfactant and tetraethoxysilane (TEOS) as silica precursor. This method is based on the hydrolysis and the condensation of TEOS. There is a major importance to the concentration and the order of addition of the different species. To the mixture of heptane/BrijSO we add slowly a colloidal suspension of y-Fe203 MPS in water (13 mg in 750 pL of water). After 15 min of stirring we added the cluster units in a mixture of Et0H H20 (1 1). Afterward we introduce an aqueous ammonia solution (28%). Finally the TEOS was added and the microemulsion was stirred during 3 days before several precipitation/resuspension to transfer our MLPs in water. 

For any process simulation that involves only vapor-liquid phases, certain key physical and thermodynamic properties must be available for each phase. Table 1.3 lists these properties for all phases. We can typically obtain these properties for pure components (i.e. n-hexane, n-heptane, etc.) from widely available databases such as DIPPR [2]. Commercial process simulation software (including Aspen HYSYS) also provides a large set of physical and thermodynamic properties for a large number of pure components. However, using these databases requires us to identify a component by name and molecular structure first, and use experimentally measured or estimated values from the same databases. Given the complexity of crude feed, it is not possible to completely analyze the crude feed in terms of pure components. Therefore, we must be able to estimate these properties for each pseudocomponent based on certain measured descriptors. 

FIG. 4-4 Property changes of mixing at 50 C for six binary liquid systems (a) chloroform(l)/n-heptane(2) (b) acetone(l)/ methanol(2)( (c) acetone(l)/chloroform(2)( (d) ethanol(l)/n-heptane(2) (e) ethanol(l)/chloroform(2) (/) ethanol(l)/water(2). [SmitK YanNesSy and Abbott, Introduction to Chemical Engineering Thermodynamics, 7thed.,p. 455, McGraw-Hill, New Yorb (2005).]... 

The experimental data for the partial solubility of perfluoro-n-heptane in various solvents has been plotted as a function of both mole fraction and volume ftaction in Fig. 11.2-3. It is of interest to notice that these solubility data are almost symmeuic functions of the volume fraction and nonsymmetric functions of the mole fraction. Such behavior has also been found with other thermodynamic mixture properties these observations suggest the use of volume fractions, rather than mole fractions or mass fractions, as the appropriate concentration variables for describing nonideal mixture behavior. Indeed, this is the reason that volume fractions have been used in both the regular solution model and the Wohl expansion of Eq. 94-8 for liquid mixtures. 

An interesting observation with respect to the supramolecular organization of 50 and 51 is the difference in the CD spectra in heptane solution. The bisig-nated CD spectrum of OPV 50 is opposite to that of 51 in sign and shape. However, in the case of 51 an inversion of the Cotton effect is observed with time (within 80 min), which is accompanied by a shift in the zero-crossing. The sign reversal of 51 shows first-order kinetics with a rate constant of k = 5.6 X 10 s . The initially formed hehx may be kinetically controlled, whereas the finally formed helix may be the thermodynamically stable form. Thus a variety of nano architectures of different shape, size and properties... 

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