Showing papers in "Journal of Chemical & Engineering Data in 1976"
TL;DR: In this paper, a table of Bunsen solubility coefficients covering the temperature range -2' to 3OoC and the salinity range -0-40 parts per thousand was calculated from the fitted equation.
Abstract: Bunsen solubility coefficients for methane in distilled water
and in seawater at three salinities were determined with an
estimated accuracy of 0.5 YO. The experimental data were
fit by the least-squares method to an equation established
by Weiss. A table of Bunsen solubility coefficients covering
the temperature range -2' to 3OoC and the salinity range
0-40 parts per thousand was calculated from the fitted
equation. For seawater of salinity 34%0, the Bunsen
coefficients ranged from 0.04489 at O°C to 0.02368 at
3OoC. Solubility values for distilled water were in agreement
with those reported by Bunsen and Claussen and Polglase
but were 34% higher than those of Winkler and Morrison
and Billet.
660 citations
TL;DR: In this paper, the isothermal vapor-liquid equilibria for three binary systems of methanol-carbon dioxide, n-hexane-carbon dioxide, and benzene-carbin dioxide were measured at 25' and 4OoC by a static method.
Abstract: Isothermal vapor-liquid equilibrium data for the systems methanol-carbon dioxide, n-hexane-carbon dioxide, and benzene-carbon dioxide were measured by a static method at 25' and 4OoC. By use of the Lewis rule and the RedlichKwong equation of state for carbon dioxide in the vapor phase, the activity coefficients in the liquid phase and the fugacity coefficients in the vapor phase were evaluated from thermodynamic relationships. The isothermal vapor-liquid equilibria at high pressures for binary systems containing carbon dioxide were reported in previous papers, in which methanol-carbon dioxide and acetone-carbon dioxide systems were measured by a vapor recirculation method (3), and ethyl ether-carbon dioxide and methyl acetate-carbon dioxide systems by a static method In this study the vapor-liquid equilibria for three binary systems of methanol-carbon dioxide, n-hexane-carbon dioxide, and benzene-carbon dioxide were measured at 25' and 4OoC by the static method. The activity coefficients in the liquid phase and fugacity coefficients in the vapor phase were determined by using the Lewis rule and the Redlich-Kwong equation of state for carbon dioxide in the vapor phase. The liquid activity coefficients in the methanol-carbon dioxide system are the largest of the three systems, though those in n-hexane-carbon dioxide and benzene-carbon dioxide are also considerably large. Experimental
250 citations
164 citations
138 citations
TL;DR: In this article, the major pollutants of petroleum refinery wastewater streams: ammonia, hydrogen sulfide, phenols, chlorides, cyanides and thiocyanates, and alkyl mercaptans are presented.
Abstract: Ionization constants up to 150 O C are presented for the major pollutants of petroleum refinery wastewater streams: ammonia, hydrogen sulfide, phenols, chlorides, cyanides and thiocyanates, and alkyl mercaptans. New experimental data are obtained at 25-150 ‘C, by means of the spectrophotometric method, for hydrogen sulfide (first ionization constant), phenol, hydrogen cyanide, and ethyl mercaptan. The value of the second ionization constant of hydrogen sulfide is determined from pH measurements. A four-term equation is used to express the temperature dependence of the ionization constants and the ionic product of water.
115 citations
TL;DR: In this paper, the same solvent components were used and carbon dioxide was replaced with ethane having similar critical temperature to that of carbon dioxide, and the nonidealities of vapor and liquid phases of the ethane systems were determined with thermodynamic procedures and were compared between these 6 systems.
Abstract: Isothermal vapor-liquid equilibrium data for binary systems containing carbon dioxide at high pressure have been reported previously. In those studies, methanol, acetone, methyl acetate, ethyl ether, n-hexane, and benzene were chosen as the solvent components. In this study, the same solvent components were used and carbon dioxide was replaced with ethane having similar critical temperature to that of carbon dioxide. The nonidealities of vapor and liquid phases of the ethane systems were determined with thermodynamic procedures and were compared between these 6 systems. By use of the Redlick-Kwong equation of state and the Lewis rule for ethane in the vapor phase, the activity coefficients in the liquid phase and the fugacity coefficients in the vapor phase were evaluated. (10 refs.)
109 citations
109 citations
89 citations
TL;DR: In this article, the authors used the Lorentz-Lorenz molar refractivity relationship to determine phase densities by the use of the molar Refractive Index (MVI).
Abstract: To supply the data needed to perform reliable design calculations with petroleum reservoir fluids or natural gas systems, the University of Alberta determined the vapor and liquid equilibrium-phase compositions at 50.0/sup 0/, 1.1/sup 0/, and -49.3/sup 0/F for the carbon dioxide-n-butane system and at -49.3/sup 0/ and -99.4/sup 0/F for the nitrogen-hydrogen sulfide system. The data for the 50.0/sup 0/F isotherm for the carbon dioxide-n-butane system were taken in a variable-volume cell, and the remaining data in a constant-volume cell designed for operation at low temperatures. Refractive index measurements of the equilibrium phases were made for the carbon dioxide-n-butane system at 50.0/sup 0/ and 1.1/sup 0/F. These measurements were used to determine phase densities by the use of the Lorentz-Lorenz molar refractivity relationship.
60 citations
TL;DR: In this article, a semi-empirical equation is given which represents the osmotic coefficients of this electrolyte to within the experimental error of the data from 0.1 to 27.7 m.
Abstract: Among the most widely used isopiestic standards for aqueous solutions are NaCl, KCl, CaCl/sub 2/, and H/sub 2/SO/sub 4/. The purpose of this paper is to reexamine and update the osmotic coefficient data for H/sub 2/SO/sub 4/ at 25/sup 0/C. A semiempirical equation is given which represents the osmotic coefficients of this electrolyte to within the experimental error of the data from 0.1 to 27.7 m.
57 citations
TL;DR: Rice University used the elution technique to study the vapor-phase concentration along isotherms in the vapor liquid region surrounding the vapor solid region for the methane-carbon dioxide system at -65 to -184/sup 0/F, a temperature range that extends below methane's critical temperature as mentioned in this paper.
Abstract: Rice University used the elution technique to study the vapor-phase concentration along isotherms in the vapor--liquid region surrounding the vapor--solid region for the methane--carbon dioxide system at -65 to -184/sup 0/F, a temperature range that extends below methane's critical temperature. Pressure conditions ranged from the three-phase solid--liquid--vapor locus to the critical point or the vapor pressure of methane. Measurements were intensified near the critical temperature of methane. The isotherms obtained for the system below methane's critical temperature were consistently linear and differed markedly from the curvatures observed by other investigators.
TL;DR: Wilson, G. M., DeVaney, W. E., and Soave, M. D. as discussed by the authors, "Mark V Computer Program", available from the Gas Processors Association, Tulsa, Okla.
Abstract: . . Tech. Papers, 53, 57 (1974). (18) Pocock, G.. Wormald, C. J., J. Chem. SOC., Faraday Trans. 1, 71, 705 (1975). (19) Soave. G.. Chem. fng. Sci., 27, 1197 (1972). (20) Starling, K. E.. Han, M. S., Hydrocarbon Process., 5 1 (5), 129 (1972). (21) Vukalovich, M. P.. Altunin, V. V., Bulle, Kh., Rasskazov. D. S., Ertel. D.. Therm. Eng., (Engl. Trans.), 16 (11). 99 (1969). (22) Vukalovich. M. P., Bulle, Kh., Rasskazov, D. S., Ertel, D.. Therm. Eng. (Engl. Trans.), 17 (6). 93 (1970). (23) Vukalovich, M. P., Bulle, Kh., Ertel, D., Russ. ./. Phys. Chem., 46, 1475 (1972). (24) Wilson, G. M., DeVaney, W. E., "Mark V Computer Program", available from the Gas Processors Association, Tulsa, Okla. (25) Yen, L. C., Alexander, R. E.. AIChE J., 11, 334 (1965).
TL;DR: In this article, the authors measured the temperatures of combustion and standard enthalpies of 22 experimental organic explosives and one standard explosive, TNT, and compared the calculated velocities with experimental veloities where suitable values of the latter were available.
Abstract: As part of a study of thermally stable explosives, the heats of combustion and standard enthalpies of formation of 22 experimental organic explosives and of one standard explosive, TNT, were determined. The results of these measurements, together with the reported crystal densities, were used to calculate the detonation velocities and pressures by two different methods. The calculated velocities were compared with experimental velocities where suitable values of the latter were available. (auth)
TL;DR: In this article, Tripathi G Singh, S K, Upadhyay, S N, Ind J Chem fng Data, 20, 20 (1975) (42) Vliet, G C, Leppert, G, J Heat Transfer, 83, 163 (1961) (43) White, R R Churchill, S W, AlChEJ, 5, 354 (1959) (44) Wilke, C R, Chang, P ibid, 1, 264(1955) 1974
Abstract: (36) Steele L R, Geankoplis, C J, AlChf J, 5, 178 (1959) (37) Steinberger, R L, Treybal R E, ibid, 6, 227 (1960) (38) Stephen, H, Stephen, T, "Solubilities of Inorganic and Organic Compounds", Pergamon Press, New York, NY, 1963 (39) Topiey E Whytlawgray R Phil Mag, 4, 873 (1927) (40) Tripathi G Singh, S K, Upadhyay, S N, Ind J Techno/, 9 (1971) (41) Upadhyay, S N, Tripathi G J Chem fng Data, 20, 20 (1975) (42) Vliet, G C, Leppert, G, J Heat Transfer, 83, 163 (1961) (43) White, R R Churchill, S W, AlChEJ, 5, 354 (1959) (44) Wilke, C R, Chang, P ibid, 1, 264(1955) 1974
TL;DR: In this paper, the authors proposed a method to determine the solubility of water by dissolving small quantities of solid acid (the purity of which is greater than 99.5Y0) in a given quantity of pure water in a stirred vessel at controlled temperature.
Abstract: Solubility in water has been determined by dissolving small quantities of solid acid (the purity of which is greater than 99.5Y0) in a given quantity of pure water, in a stirred vessel at controlled temperature. After dissolution has stopped, stirring is continued for 5-6 hr to ensure that equilibrium has been reached. Then the remaining solid is quickly filtrated and dried. The concentration of the solution is determined by weighing the solid (method 1) or titrating the liquid with sodium hydroxyde (method 2). The results expressed in grams of monohydrate acid1100 g of pure water are presented in Table I . As shown in Figure 1, the agreement with Dalman’s data (2) which are recommended by Mullin ( 11) and Nyvlt ( 13) is very good and also with the data given by Perry ( 14), Kirk and Othmer (6), and Stephen and Stephen (15). On the contrary, the difference is more important with Kremann and Eitel’s data (7). Between 17’ and 33OC, experimental results can be correlated in the form:
TL;DR: The authors used the absolute capillary method to measure the viscosity of methane, hydrogen, and mixtures (nominally 20, 40, 60, and 80% hydrogen) at 0, -50, -75, and -100/sup 0/C at pressures from 4 up to 450 to 500 atm.
Abstract: Rice University used the absolute capillary method to measure the viscosity of methane, hydrogen, and mixtures (nominally 20, 40, 60, and 80% hydrogen) at 0, -50, -75, and -100/sup 0/C at pressures from 4 up to 450 to 500 atm. The maximum probable error of the calculated viscosity is estimated to be 0.5%. The viscosity data were fit by the least-squares method to give 1.193 +- 0.034 for the Hagenbach factor for the kinetic correction in the vicosity formula. The residual-viscosity concept was obeyed within +- 1% except for hydrogen and the 80% hydrogen mixture. The deviations for these are attributed to first-order quantum effects.
TL;DR: In this article, the ultraviolet and visible extinction coefficients of Cl 2O and Cl2O7 were measured from 180 to 800 nm and the results were comparable in shape with literature values, but different in magnitude.
Abstract: The ultraviolet and visible extinction coefficients of Cl2O and Cl2O7 were measured from 180 to 800 nm. The results are comparable in shape with literature values, but different in magnitude. The approximate extinction coefficients at the peaks of infrared absorption lines are also given.
TL;DR: Rossini et al. as discussed by the authors compared the solute mole fraction vs. reciprocal temperature experimental data with ideal predictions and showed that the ideal loci for the three systems studied are the li&t lines.
Abstract: 54. iai-ia4 i i ~ m -., . . ~ -.-,. (8) Rossini, F. C., Piker, K. S., Amet, R. L., Brown, R. M., Pimental, G. C., “Selected Values of Physical and Thermodynamic Properties of Hydrocarbons and Related Compounds”, Carnegie Press, Pittsburgh. Pa., 1953. Flgure 1. A comparison of the solute mole fraction vs. reciprocal temperature experimental data with ideal predictions. The heavy lines are the smoothed data presentations of Tables 1-111, while the li&t lines are the ideal loci for the three systems studied. Received for review December 1.1975. Accepted March 29,1976. The authors are grateful for suppat of this work provkled by the Gas Processors Association (Research Project No. 735). The research equipment had been built under research grants by the National Science Foundation.