Vapor-liquid-equilibrium 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. 

Two additional illustrations are given in Figures 6 and 7 which show fugacity coefficients for two binary systems along the vapor-liquid saturation curve at a total pressure of 1 atm. These results are based on the chemical theory of vapor-phase imperfection and on experimental vapor-liquid equilibrium data for the binary systems. In the system formic acid (1) - acetic acid (2), <() (for y = 1) is lower than formic acid at 100.5°C has a stronger tendency to dimerize than does acetic acid at 118.2°C. Since strong dimerization occurs between all three possible pairs, (fij and not... 

Figure 15 shows results for a difficult type I system methanol-n-heptane-benzene. In this example, the two-phase region is extremely small. The dashed line (a) shows predictions using the original UNIQUAC equation with q = q. This form of the UNIQUAC equation does not adequately fit the binary vapor-liquid equilibrium data for the methanol-benzene system and therefore the ternary predictions are grossly in error. The ternary prediction is much improved with the modified UNIQUAC equation (b) since this equation fits the methanol-benzene system much better. Further improvement (c) is obtained when a few ternary data are used to fix the binary parameters. 

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). 

Note that good vapor-liquid equilibrium data for low pressure conditions are very scarce and difficult to locate. However, for proper calculations they are essential. See References 151 and 152 dealing with this. 

Table 14.9 Vapor-Liquid Equilibrium Data for the Methanol (l)-Isobutane...

Table 15.8 Vapor-Liquid Equilibrium Data for Ethylbenzene (l)-o-Xylene (2)...

Galivel - Solastiuk F., S. Laugier and D. Richon, "Vapor-Liquid Equilibrium Data for the Propane-MethanoI-C02 System", Fluid Phase Equilibria, 28, 73-85 (1986). 

Miles, D. H. and Wilson, G. M. "Vapor-Liquid Equilibrium Data for Design of Sour Water Strippers", Annual Report to the American Petroleum Institute for 1974, October 1975 (Data in this report are also summarized in reference 2). 

Vapor-liquid equilibrium data for the two binary systems (11) were used to calculate the standard-state fugacities required in Equations 6 and 20. In the temperature range 0-50°C, there fugacities can be expressed by ... 

Kurihara, K., Takimoto, Y., Ochi, K., and Kojima, K. Vapor-liquid equilibrium data for the quaternary system acetone + chloroform-t methanol -t benzene at 101.3 kPa, J. Chem. Eng. Data, 45(5) 792-795, 2000. 

The Correlation of Vapor-Liquid Equilibrium Data for Salt-Containing Systems... 

Table II. Vapor—Liquid Equilibrium Data for 2-Propanol—Water—LiC104 System at 50° and 25°C...

Table I. Isobaric Vapor—Liquid Equilibrium Data for the Potassium Bromide—Ethanol—Water System at x = 0.206 0.001 (760 5 Torr)...

Maher, P. J., and B. D. Smith, Vapor-liquid equilibrium data for binary systems of chlorobenzene with acetone, acetonitrile, ethyl acetate, ethylbenzene, methanol and 1-pentene , J. Chem. Eng. Data, 24, 363-377 (1979). 

Distillation of Ammonium Bicarbonate Solutions. Vapor-liquid equilibrium data for ammonium bicarbonate solutions at the boil are apparently not available in the literature. The data in the literature, however, do indicate that when the temperature of such a solution is increased, or the pressure on it decreased, the gas that is evolved is predominantly carbon dioxide. Thus, it appears that such a distillation would be two consecutive processes first, a steam stripping of the carbon dioxide in the solution, followed by a distillation of ammonia from an ammonia-water mixture containing perhaps some carbon dioxide. Possibly the ammonia, carbon dioxide, and water in the distillate product would recombine completely in the condenser to form an ammonium bicarbonate solution. Perhaps an absorption tower would be necessary to effect the recombination. 

Jacoby, R.H., Vapor-Liquid Equilibrium Data for Use of Methanol in Preventing Gas Hydrates, in Proc. Gas Hydrocarbon. Control Conference. University of Oklahoma, Norman, OK (1953). 

To perform a further detailed process calculation on this multi-component absorption and stripping process, vapor liquid equilibrium data for methane, hydrogen, and carbon monoxide is... 

Parrish, W.R., Sitton, D.M. (1982) Vapor-liquid equilibrium data for the propane/-, n-butanc/-, isobutene/-, and propylene/isopropyl fluoride systems. J. Chem. Eng. Data 27, 303-306. 

Braun, W. G., Fenske, M. R., and Holmes, A. S., Bibliography of Vapor-Liquid Equilibrium Data for Hydrocarbon Systems, American Petroleum Institute, New York, 1963. 

Using the Redlich-Kister expansion (16) an expression for Y /acjj was developed at Kigh temperatures using vapor-liquid equilibrium data for... 

Vapor/liquid equilibrium data for the system l -dichloromethane(l)/methanol(2) at -as follows ... 

TABLE 1.8 Vapor-Liquid Equilibrium Data for Benzene(l)/n-Heptane(2) System at 80°C... 

Experimental vapor-liquid-equilibrium data for benzene(l)/n-heptane(2) system at 80°C (176°F) are given in Table 1.8. Calculate the vapor compositions in equilibrium with the corresponding liquid compositions, using the Scatchard-Hildebrand regular-solution model for the liquid-phase activity coefficient, and compare the calculated results with the experimentally determined composition. Ignore the nonideality in the vapor phase. Also calculate the solubility parameters for benzene and n-heptane using heat-of-vaporization data. 

---