Journal articles: 'Raoult's law'

1

Hermans, J. J. "Raoult's law as a limiting law." Recueil des Travaux Chimiques des Pays-Bas 60, no. 5 (September 3, 2010): 370–72. http://dx.doi.org/10.1002/recl.19410600508.

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Hawkes, Stephen J. "Raoult's Law Is a Deception." Journal of Chemical Education 72, no. 3 (March 1995): 204. http://dx.doi.org/10.1021/ed072p204.

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Kovac, Jeffrey. "Molecular size and Raoult's Law." Journal of Chemical Education 62, no. 12 (December 1985): 1090. http://dx.doi.org/10.1021/ed062p1090.

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Wilson, Archie S. "A visual demonstration of Raoult's law." Journal of Chemical Education 67, no. 7 (July 1990): 598. http://dx.doi.org/10.1021/ed067p598.2.

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5

Hawkes, Stephen J. "Strategic Consequences from Errors in Raoult's Law Paper." Journal of Chemical Education 73, no. 1 (January 1996): 41. http://dx.doi.org/10.1021/ed073p41.

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YIN, Xuebo. "Relationship and Difference among Raoult's Law, Henry's Law, and Azeotropic Solution." University Chemistry 33, no. 5 (2018): 61–65. http://dx.doi.org/10.3866/pku.dxhx201801010.

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Ferrero Vallana, Federico M., Ricardo P. Girling, H. Q. Nimal Gunaratne, Lynette A. M. Holland, Pauline M. Mcnamee, Kenneth R. Seddon, Jonathan R. Stonehouse, and Oreste Todini. "Ionic liquids as modulators of fragrance release in consumer goods." New Journal of Chemistry 40, no. 12 (2016): 9958–67. http://dx.doi.org/10.1039/c6nj01626j.

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8

Bowler, Michael G., David R. Bowler, and Matthew W. Bowler. "Raoult's law revisited: accurately predicting equilibrium relative humidity points for humidity control experiments." Journal of Applied Crystallography 50, no. 2 (March 29, 2017): 631–38. http://dx.doi.org/10.1107/s1600576717003636.

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The humidity surrounding a sample is an important variable in scientific experiments. Biological samples in particular require not just a humid atmosphere but often a relative humidity (RH) that is in equilibrium with a stabilizing solution required to maintain the sample in the same state during measurements. The controlled dehydration of macromolecular crystals can lead to significant increases in crystal order, leading to higher diffraction quality. Devices that can accurately control the humidity surrounding crystals while monitoring diffraction have led to this technique being increasingly adopted, as the experiments become easier and more reproducible. Matching the RH to the mother liquor is the first step in allowing the stable mounting of a crystal. In previous work [Wheeler, Russi, Bowler & Bowler (2012). Acta Cryst. F68, 111–114], the equilibrium RHs were measured for a range of concentrations of the most commonly used precipitants in macromolecular crystallography and it was shown how these related to Raoult's law for the equilibrium vapour pressure of water above a solution. However, a discrepancy between the measured values and those predicted by theory could not be explained. Here, a more precise humidity control device has been used to determine equilibrium RH points. The new results are in agreement with Raoult's law. A simple argument in statistical mechanics is also presented, demonstrating that the equilibrium vapour pressure of a solvent is proportional to its mole fraction in an ideal solution: Raoult's law. The same argument can be extended to the case where the solvent and solute molecules are of different sizes, as is the case with polymers. The results provide a framework for the correct maintenance of the RH surrounding a sample.

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9

González, Juan Antonio, Isaiés Garcié de la Fuentá, and Jose Carlos Cobos. "Thermodynamics of mixtures with strongly negative deviations from Raoult's Law." Fluid Phase Equilibria 168, no. 1 (February 2000): 31–58. http://dx.doi.org/10.1016/s0378-3812(99)00326-x.

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10

Berka, Ladislav H., and Nicholas Kildahl. "Experiments for Modern Introductory Chemistry: Intermolecular Forces and Raoult's Law." Journal of Chemical Education 71, no. 7 (July 1994): 613. http://dx.doi.org/10.1021/ed071p613.

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11

Nimtz, G., P. D. Marquardt, D. Stauffer, and W. Weiss. "Raoult's Law and the Melting Point Depression in Mesoscopic Systems." Science 242, no. 4886 (December 23, 1988): 1671–72. http://dx.doi.org/10.1126/science.242.4886.1671.

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12

Villa, S., R. Garriga, P. Pérez, M. Gracia, J. A. González, I. García de la Fuente, and J. C. Cobos. "Thermodynamics of mixtures with strongly negative deviations from Raoult's law." Fluid Phase Equilibria 231, no. 2 (April 2005): 211–20. http://dx.doi.org/10.1016/j.fluid.2005.01.013.

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Brown, Derick G., Lovleen Gupta, Horace Keith Moo-Young, and Andrew J. Coleman. "RAOULT'S LAW–BASED METHOD FOR DETERMINATION OF COAL TAR AVERAGE MOLECULAR WEIGHT." Environmental Toxicology and Chemistry 24, no. 8 (2005): 1886. http://dx.doi.org/10.1897/04-470r.1.

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14

Kugel, Roger W. "Raoult's Law: Binary Liquid-Vapor Phase Diagrams: A Simple Physical Chemistry Experiment." Journal of Chemical Education 75, no. 9 (September 1998): 1125. http://dx.doi.org/10.1021/ed075p1125.

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15

Peng, Ding-Yu. "Implications of standard states and ideal solution in terms of Raoult's law." Canadian Journal of Chemical Engineering 68, no. 3 (June 1990): 473–78. http://dx.doi.org/10.1002/cjce.5450680318.

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16

Goldfarb, Jillian L., and Eric M. Suuberg. "Raoult's Law and Its Application to Sublimation Vapor Pressures of Mixtures of Polycyclic Aromatic Hydrocarbons." Environmental Engineering Science 25, no. 10 (December 2008): 1429–38. http://dx.doi.org/10.1089/ees.2007.0195.

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17

Domanska, Urszula, and Juan Antonio Gonzalez. "Thermodynamics of mixtures containing a very strongly polar compound. Part II. Solid-liquid equilibria for sulfolane + nitrile systems and characterization of the sulfolane-nitrile and sulfolane-1-alkyne interactions in terms of DISQUAC." Canadian Journal of Chemistry 80, no. 5 (May 1, 2002): 476–82. http://dx.doi.org/10.1139/v02-066.

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Equilibrium temperatures for solidliquid transitions of mixtures formed by sulfolane and ethanenitrile, propanenitrile, butanenitrile, or pentanenitrile were measured by a dynamic method. The solidliquid equilibria phase diagrams show positive deviations from Raoult's law, except for the system with ethanenitrile, which is nearly ideal. The sulfolanenitrile and sulfolane1-alkyne interactions have been characterized in terms of the DISQUAC group contribution model. DISQUAC properly represents a complete set of thermodynamic properties: solidliquid equilibria, molar excess enthalpies, and natural logarithms of activity coefficients. DISQUAC predictions are valid over a wide temperature range.Key words: solidliquid equilibria, thermodynamics, mixtures, interactions.

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18

Cardinali, Mario Emilio, and Claudio Giomini. "Boiling temperature vs. composition: An almost-exact explicit equation for a binary mixture following Raoult's Law." Journal of Chemical Education 66, no. 7 (July 1989): 549. http://dx.doi.org/10.1021/ed066p549.

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19

Viswanathan, R., and G. Horowitz. "Integrating Computers into the First-Year Chemistry Laboratory: Application of Raoult's Law to a Two-Component System." Journal of Chemical Education 75, no. 9 (September 1998): 1124. http://dx.doi.org/10.1021/ed075p1124.

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20

Liron, Zvi, Shalom Srebrenik, Alfred Martin, and Sasson Cohen. "Theoretical derivation of solute-solvent interaction parameter in binary solution: Case of the deviation from Raoult's Law." Journal of Pharmaceutical Sciences 75, no. 5 (May 1986): 463–68. http://dx.doi.org/10.1002/jps.2600750509.

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21

González, Juan Antonio, Ismael Mozo, Isaías García de la Fuente, and José Carlos Cobos. "Thermodynamics of binary mixtures with strongly negative deviations from Raoult's Law. X. linear alkanoate + CHCl3or + 1,1,2,2-tetrachloroethane." Physics and Chemistry of Liquids 43, no. 4 (August 2005): 317–32. http://dx.doi.org/10.1080/00319100500062496.

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22

Stoeckli, F., D. Wintgens, A. Lavanchy, and M. Stöckli. "Binary Adsorption of Vapours in Active Carbons Described by the Combined Theories of Myers—Prausnitz and Dubinin (II)." Adsorption Science & Technology 15, no. 9 (October 1997): 677–83. http://dx.doi.org/10.1177/026361749701500904.

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The new MPD method, described recently, has been applied to the adsorption of benzene +1,2-dichloroethane vapours by a typical active carbon at 293 K. A total of 102 experiments have been carried out for adsorbed mole fractions between 0.06 and 0.94. Good agreement was found between the experimental and calculated values of the selectivity of the carbon for benzene, which decreased as the mole fraction of benzene increased. This variation reflects the heterogeneity of the carbon, which is taken into account by the DR equation. Although the liquid mixture is ideal, deviations from Raoult's law are observed in the adsorbed state, indicating a clear preference for benzene. The values of the activity coefficients obtained from the liquid/solid equilibrium improve the fit of the MPD method.

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23

Kayano, Satoshi, and David J. Wilson. "Soil Clean Up by in-situ Aeration. X. Vapor Stripping of Mixtures of Volatile Organics Obeying Raoult's Law." Separation Science and Technology 27, no. 12 (October 1992): 1525–54. http://dx.doi.org/10.1080/01496399208029222.

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24

Treble, Ronald G., Keith E. Johnson, and Evangeline Tosh. "The volatilities and conductivities of ionic liquids — GC–MS methodology and preliminary studies of acetic acid – base systems." Canadian Journal of Chemistry 84, no. 6 (June 1, 2006): 915–24. http://dx.doi.org/10.1139/v06-098.

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Gas chromatography – mass spectrometry studies of the headspaces above the binary systems pyridine (bp 115 °C) – acetic acid (bp 116 °C), 1-methylimidazole (bp 198 °C) – acetic acid, and triethylamine (bp 89 °C) – acetic acid show both components in the first case, acetic acid only in the second, and triethylamine only in the third. Negative deviations from Raoult's law are confirmed and proton transfer is evidenced by the downfield shift of the acidic proton as the addition of base proceeds. Specific conductances >2 mS cm–1 are found over wide composition ranges for all three systems with values >8 mS cm–1 at high (>2) mole ratios of acetic acid, suggesting the formation of acetatohydrogenate ionic liquids.Key words: GC–MS, air, vapor pressure, conductivity, ionic liquids, acetic acid.

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25

Castarède, Dimitri, and Erik S. Thomson. "A thermodynamic description for the hygroscopic growth of atmospheric aerosol particles." Atmospheric Chemistry and Physics 18, no. 20 (October 17, 2018): 14939–48. http://dx.doi.org/10.5194/acp-18-14939-2018.

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Abstract. The phase state of atmospheric particulate is important to atmospheric processes, and aerosol radiative forcing remains a large uncertainty in climate predictions. That said, precise atmospheric phase behavior is difficult to quantify and observations have shown that “precondensation” of water below predicted saturation values can occur. We propose a revised approach to understanding the transition from solid soluble particles to liquid droplets, typically described as cloud condensation nucleation – a process that is traditionally captured by Köhler theory, which describes a modified equilibrium saturation vapor pressure due to (i) mixing entropy (Raoult's law) and (ii) droplet geometry (Kelvin effect). Given that observations of precondensation are not predicted by Köhler theory, we devise a more complete model that includes interfacial forces giving rise to predeliquescence, i.e., the formation of a brine layer wetting a salt particle at relative humidities well below the deliquescence point.

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26

Zhang, Xiao Dong, Da Peng Hu, and Zong Chang Zhao. "Measurement and Correlation for Vapor Pressure and Excess Enthalpy of the New Working Pairs：Water/Ethanol/Methanol + Ionic Liquids 1-Ethyl-3-Methylimidazolium Diethylphosphate." Advanced Materials Research 524-527 (May 2012): 1697–701. http://dx.doi.org/10.4028/www.scientific.net/amr.524-527.1697.

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Three binary solutions composed of ionic liquid (IL), 1-ethyl-3-methylimidazolium diethylphosphate ([EMIM] [DEP]), and selected refrigerants (water, ethanol or methanol) were proposed as new working pairs for absorption heat pumps or absorption refrigerators. The vapor–liquid equilibrium (VLE) data were measured by a static method at different temperatures and at different ILs mole factions and correlated by the None-Random Two Liquids (NRTL) activity coefficient models, and the average relative deviation were less than 3.3%. The solutions showed strong negative deviation from the Raoult's Law and were able to absorb vapor of water, ethanol or methanol. The excess enthalpies were measured and correlated at 298.15 K and atmospheric pressure. The results indicated that the mixing of [EMIM] [DEP] with water, ethanol or methanol were exothermal. The proposed solutions were proved to possess one of the fundamental features that a working pair must have in absorption cycle.

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27

Banipal, T. S., B. S. Lark, and S. Singh. "Excess Gibbs energy for binary mixtures of acetonitrile with acetic acid, propionic acid, isobutyric acid, and trimethylacetic acid." Canadian Journal of Chemistry 69, no. 12 (December 1, 1991): 2117–21. http://dx.doi.org/10.1139/v91-305.

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Total vapour pressures for binary mixtures containing acetic acid, propionic acid, isobutyric acid, and trimethylacetic acid with acetonitrile have been measured for the entire composition range at 298.15 and 318.15 K using a static manometric method. All systems show positive deviations from Raoult's law, enhanced by both an increase in temperature and an increase in the methylation of acetic acid. Activity coefficients have been calculated by taking into consideration the dimerization of these carboxylic acids in the vapour phase. TSE values obtained from GE and earlier reported HE values are found to be negative for acetic acid, about zero for propionic and isobutyric acids, and positive for trimethylacetic acid for the whole composition range. The results have been interpreted in terms of various contributions such as depolymerization, heteromolecular dipole–dipole interactions, and the increasing dimerization constant and steric hindrance with increase of complexity of the acid. Key words: excess Gibbs energy, carboxylic acids, acetonitrile, activity coefficients

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28

Marshall, William L. "Modified Raoult's law including the solvent structural constant and solute solvation; Aqueous sodium chloride solutions, 25 to 300�C; Other electrolytes and urea, 25�C." Journal of Solution Chemistry 15, no. 5 (May 1986): 439–52. http://dx.doi.org/10.1007/bf00646267.

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29

Matteoli, Enrico. "Interactions in Mixtures: Evaluation of the Contributions of Long- and Short-Range Correlations to Raoult's Law Deviations by Means of the Fluctuation Theory of Mixtures." Zeitschrift für Physikalische Chemie 185, Part_2 (January 1994): 177–93. http://dx.doi.org/10.1524/zpch.1994.185.part_2.177.

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30

Donahue, N. M., S. A. Epstein, S. N. Pandis, and A. L. Robinson. "A two-dimensional volatility basis set: 1. organic-aerosol mixing thermodynamics." Atmospheric Chemistry and Physics Discussions 10, no. 10 (October 15, 2010): 24091–133. http://dx.doi.org/10.5194/acpd-10-24091-2010.

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Abstract. We develop the thermodynamic underpinnings of a two-dimensional volatility basis set (2-D-VBS) employing saturation concentration (Co) and the oxygen content (O:C) to describe volatility, mixing thermodynamics, and chemical evolution of organic aerosol. This is an extension of our earlier one-dimensional approach employing C* only (C*=γ Co, where γ is an activity coefficient). We apply a mean-field approximation for organic aerosol, describing interactions of carbon and oxygen groups in individual molecules (solutes) with carbon and oxygen groups in the organic-aerosol solvent. In so doing, we show that a linear structure activity relation (SAR) describing the single-component Co of a molecule is directly tied to ideal solution (Raoult's Law) behavior. Conversely, non-ideal solution behavior (activity coefficients) and a slightly non-linear SAR emerge from off-diagonal (carbon-oxygen) interaction elements. From this foundation we can build a self-consistent description of OA mixing thermodynamics, including predicted saturation concentrations and activity coefficients (and phase separation) for various solutions from just four free parameters: the carbon number of a hydrocarbon with a 1 μg m−3 Co, and the carbon-carbon, oxygen-oxygen, and non-ideal carbon-oxygen terms. This treatment establishes the mean molecular formula for organics within this 2-D space as well as activity coefficients for molecules within this space interacting with any bulk OA phase described by an average O:C.

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31

Sanz, Luis F., Juan A. González, Isasías García De La Fuente, and José C. Cobos. "Thermodynamics of mixtures with strongly negative deviations from Raoult's law. XI. Densities, viscosities and refractives indices at (293.15–303.15) K for cyclohexylamine+1-propanol, or +1-butanol systems." Journal of Molecular Liquids 172 (August 2012): 26–33. http://dx.doi.org/10.1016/j.molliq.2012.05.003.

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32

Antonio Gonzalez, Juan, Isaias Garcia de la Fuente, and and Jose Carlos Cobos. "Thermodynamics of mixtures with strongly negative deviation from Raoult's law Part 1Application of the DISQUAC model to mixtures of alkan-1-ols and propanal or linear alkanones and trichloromethane." Journal of the Chemical Society, Faraday Transactions 93, no. 21 (1997): 3773–80. http://dx.doi.org/10.1039/a704483f.

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33

Madronich, S., A. J. Conley, J. Lee-Taylor, L. I. Kleinman, A. Hodzic, and B. Aumont. "Non-linear partitioning and organic volatility distributions of urban aerosols." Faraday Discussions 189 (2016): 515–28. http://dx.doi.org/10.1039/c5fd00209e.

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Gas-to-particle partitioning of organic aerosols (OA) is represented in most models by Raoult's law, and depends on the existing mass of particles into which organic gases can dissolve. This raises the possibility of non-linear response of particle-phase OA mass to the emissions of precursor volatile organic compounds (VOCs) that contribute to this partitioning mass. Implications for air quality management are evident: a strong non-linear dependence would suggest that reductions in VOC emission would have a more-than-proportionate benefit in lowering ambient OA concentrations. Chamber measurements on simple VOC mixtures generally confirm the non-linear scaling between OA and VOCs, usually stated as a mass-dependence of the measured OA yields. However, for realistic ambient conditions including urban settings, no single component dominates the composition of the organic particles, and deviations from linearity are presumed to be small. Here we re-examine the linearity question using volatility spectra from several sources: (1) chamber studies of selected aerosols, (2) volatility inferred for aerosols sampled in two megacities, Mexico City and Paris, and (3) an explicit chemistry model (GECKO-A). These few available volatility distributions suggest that urban OA may be only slightly super-linear, with most values of the normalized sensitivity exponent in the range 1.1–1.3, also substantially lower than seen in chambers for some specific aerosols. The rather low exponents suggest that OA concentrations in megacities are not an inevitable convergence of non-linear effects, but can be addressed (much like in smaller urban areas) by proportionate reductions in emissions.

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34

Antonio González, Juan, Isías García de la Fuente, and Jose´ Carlos Cobos. "Thermodynamics of mixtures with strongly negative deviations from Raoult's law Part 2. Application of the DISQUAC model to mixtures of CHCl3 or CH2Cl2 with oxaalkanes. Comparison with Dortmund UNIFAC results." Physical Chemistry Chemical Physics 1, no. 2 (1999): 275–83. http://dx.doi.org/10.1039/a807600f.

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35

González, Juan Antonio, Isaias Garcia de la Fuente, and Jose Carlos Cobos. "Thermodynamics of mixtures with strongly negative deviations from Raoult's law. Part 3. Application of the DISQUAC model to mixtures of triethylamine with alkanols. Comparison with Dortmund UNIFAC and ERAS results." Canadian Journal of Chemistry 78, no. 10 (October 1, 2000): 1272–84. http://dx.doi.org/10.1139/v00-114.

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Binary mixtures of triethylamine (TEA) and alkanols have been investigated in the framework of DISQUAC. The systems are built by three contacts: aliphatichydroxyl, aliphaticnitrogen, and hydroxylnitrogen. The corresponding interaction parameters are reported and discussed. The former are avalilable in the literature but were modified (particularly the third dispersive (DIS) and quasichemical (QUAC) interchange coefficients) for sec- and tert-alkanols + n-alkanes using recent data on excess heat capacities at constant pressure (CEP) for systems of these alkanols with n-heptane. The interaction parameters for aliphatic-nitrogen contacts are purely dispersive. The structure dependence of the DIS and QUAC interchange coefficients of the hydroxyl-nitrogen contacts in 1-alkanols + TEA systems is similar to that found in other solutions previously investigated. The QUAC interchange coefficients remain constant from ethanol and are also valid for 2-alkanols and tert-butanol. Methanol behaves differently. A short discussion in terms of effective dipole moments is also included. DISQUAC represents well the thermodynamic properties examined: vapor-liquid equilibria (VLE), molar excess Gibbs energies (GE) and molar excess enthalpies (HE). DISQUAC provides better results than the Dortmund version of UNIFAC using the published geometrical and interaction parameters. ERAS parameters for 1-alkanols + TEA systems are also reported. Interactions between unlike molecules are stronger for solutions with methanol or ethanol. DISQUAC improves ERAS results on HE, while both models give similar results for GE. However, ERAS needs an specific parameter, with unknown temperature-dependence, to describe properly GE. The main advantage of ERAS is its ability to provide information on VE. Its main limitation is that can be only applied to those systems where association is expected. DISQUAC, a purely physical model, can be applied to any type of binary mixture, as it is followed from this and previous studies.Key words: theory, liquids, associated, thermodynamics, group contributions.

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Hevia, Fernando, Juan Antonio González, Ana Cobos, Isaías García de la Fuente, and Cristina Alonso-Tristán. "Thermodynamics of mixtures with strongly negative deviations from Raoult's law. XV. Permittivities and refractive indices for 1-alkanol + n -hexylamine systems at (293.15–303.15) K. Application of the Kirkwood-Fröhlich model." Fluid Phase Equilibria 468 (July 2018): 18–28. http://dx.doi.org/10.1016/j.fluid.2018.04.007.

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Hevia, Fernando, Ana Cobos, Juan Antonio González, Isaías García de la Fuente, and Luis Felipe Sanz. "Thermodynamics of mixtures with strongly negative deviations from Raoult's law. XVI. Permittivities and refractive indices for 1-alkanol + di-n-propylamine systems at (293.15–303.15) K. Application of the Kirkwood-Fröhlich model." Journal of Molecular Liquids 271 (December 2018): 704–14. http://dx.doi.org/10.1016/j.molliq.2018.09.040.

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38

González, Juan Antonio, Isaias Garcia de la Fuente, and Jose Carlos Cobos. "Thermodynamics of mi×tures with strongly negative deviations from Raoult's law. Part 3. Application of the DISQUAC model to mi×tures of triethylamine with alkanols. Comparison with Dortmund UNIFAC and ERAS results." Canadian Journal of Chemistry 78, no. 10 (2000): 1272–84. http://dx.doi.org/10.1139/cjc-78-10-1272.

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39

Akinin, N. I., and N. O. Melnikov. "Experimental and Calculated Values of the Flash Point of Solvent Mixtures Used in Industry." Occupational Safety in Industry, no. 12 (December 2020): 12–18. http://dx.doi.org/10.24000/0409-2961-2020-12-12-18.

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The experimental verification of the calculated flash point temperatures of solvent mixtures used in industry is presented, and the evaluation of the adequacy of the methods for calculating the rate of its evaporation is given. To verify these methods, acetone-benzene and acetone-chloroform mixtures were experimentally studied, for which a deviation from Raoult's law could be assumed. The dependences of the evaporated substance on time at room temperature are obtained. An increase in the saturated vapor pressure and an increase in the evaporation rate are observed in the first mixture, and a decrease in the second. In the first case, the amount of substance that is taking part in the explosion increases and must be taken into account when calculating the room pressure increase during explosion, and the second can be used to reduce the potential explosive hazard of solvent mixtures. The problem of predicting fire and explosion hazard of solvents is associated with the identification of the fact of the formation of explosive concentrations of their vapors and change of flash point temperatures of the mixed liquids. By the example of a number of binary mixtures of flammable liquids, the influence of the interaction of their components on the flash point is shown, the calculated and experimental (reference) data in a closed crucible are compared for the ratio of components in the range from 0 to 100 % in benzene-toluene and benzene-ethanol mixtures. It is noted that for mixtures with a similar molecular structure, the results of calculating the flash point are in good agreement with the experiment, otherwise, the calculation gives overestimated values for liquids of various classes. Therefore, for mixtures of solvents used in industry, the number of components of which is three or more, it is required to check the flash point experimentally in order to more accurately predict their fire and explosion hazard.

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40

Lewicki, Piotr P. "Raoult’s law based food water sorption isotherm." Journal of Food Engineering 43, no. 1 (January 2000): 31–40. http://dx.doi.org/10.1016/s0260-8774(99)00130-2.

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41

Clarke, Colin W., and David N. Glew. "Aqueous nonelectrolyte solutions. Part XV. The deuterium sulfide - deuterium oxide system and the deuterium sulfide D-hydrate." Canadian Journal of Chemistry 76, no. 8 (August 1, 1998): 1119–29. http://dx.doi.org/10.1139/v98-133.

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The univariant (l1l2g) saturation vapor pressure of liquid deuterium oxide (phase l1) with liquid deuterium sulfide (phase l2) in equilibrium with a gas phase (g) has been measured in a stirred titanium reaction vessel at 19 temperatures from 33.003 to 18.905°C and at total pressures from 2.4500 to 1.7428 MPa. The univariant (hl1g) saturation vapor pressure of deuterium sulfide D-hydrate (phase h) in equilibrium with liquid deuterium oxide and a gas phase has been measured at 58 temperatures from 30.666 to 2.798°C and at pressures from 2.2959 to 0.11629 MPa. The maximum temperature for deuterium sulfide D-hydrate with a gas phase, the invariant quadruple point Q(hl1l2g), has been determined from the cut of the (hl1g) and the (l1l2g) curves at temperature 30.770°C with standard error 0.0043°C and at pressure 2.3263 MPa with standard error 0.00018 MPa. The univariant (s1l1g) equilibrium of D-ice (phase s1) with liquid deuterium oxide and a gas phase containing deuterium sulfide has been measured at 11 temperatures from 3.8061 to 3.4540°C and at pressures between 0.00242 and 0.10542 MPa. The lowest temperature for stability of deuterium sulfide D-hydrate with liquid deuterium oxide, the invariant quadruple point Q(hs1l1g), has been determined directly at 3.3917°C with standard error 0.0009°C and at pressure 0.12364 MPa with standard error 0.000011 MPa. This quadruple point Q(hs1l1g) has also been defined by the cut of the (hl1g) and the (s1l1g) curves at temperature 3.3912°C with standard error 0.0006°C and at pressure 0.12363 MPa with standard error 0.000002 MPa. The deuterium sulfide - deuterium oxide gas mixture, represented by a Redlich-Kwong equation of state, has been used to evaluate the fugacities and compositions of the gaseous and liquid deuterium oxide phases for all equilibria. Raoult's law using fugacities has been used to evaluate the saturation mole fraction of deuterium oxide in liquid deuterium sulfide and the Henry's law constant for deuterium oxide solubility in liquid deuterium sulfide between 33.003 and 18.905°C. Data for the (l1l2g) and (s1l1g) equilibria have been accurately represented by simple two-parameter equations. Data for the (hl1g) equilibrium have required a model with seven significant parameters for proper representation betweem 30.666 and 2.798°C.Key words: deuterium sulfide - deuterium oxide system, clathrate D-hydrate of deuterium sulfide, deuterium sulfide D-hydrate stability, freezing of deuterium oxide - deuterium sulfide, phase equilibria of deuterium sulfide - deuterium oxide.

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Villa, S., N. Riesco, I. Garcı́a de la Fuente, J. A. González, and J. C. Cobos. "Thermodynamics of mixtures with strongly negative deviations from Raoult’s law." Fluid Phase Equilibria 190, no. 1-2 (November 2001): 113–25. http://dx.doi.org/10.1016/s0378-3812(01)00595-7.

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Villa, S., N. Riesco, I. Garcı́a de la fuente, J. A. González, and J. C. Cobos. "Thermodynamics of mixtures with strongly negative deviations from Raoult’s law." Fluid Phase Equilibria 198, no. 2 (May 2002): 313–29. http://dx.doi.org/10.1016/s0378-3812(01)00808-1.

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Bowman, Frank M., and Karen Eskelson. "Thermodynamic consistency of Raoult’s Law and Henry’s Law approaches for multiphase organic aerosol partitioning." Journal of Atmospheric Chemistry 64, no. 2-3 (December 2009): 179–93. http://dx.doi.org/10.1007/s10874-010-9176-8.

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Berdnikov, V. I., and Yu A. Gudim. "IDENTIFICATION OF ASSOCIATES IN SOLUTIONS WITH POSITIVE DEVIATIONS FROM RAOULT’S LAW." Izvestiya Visshikh Uchebnykh Zavedenii. Chernaya Metallurgiya = Izvestiya. Ferrous Metallurgy 60, no. 3 (January 1, 2017): 241–46. http://dx.doi.org/10.17073/0368-0797-2017-3-241-246.

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Hristova, Mariana. "Measurement and prediction of binary mixture flash point." Open Chemistry 11, no. 1 (January 1, 2013): 57–62. http://dx.doi.org/10.2478/s11532-012-0131-1.

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AbstractThe flash points of three binary mixtures, containing n-heptane, o-xylene, m-xylene and ethylbenzene, were measured by Pensky-Martens closed cup tester. The experimental data were compared with the calculated values using Liaw’s Model with the application of Raoult’s Law and Wilson equation. These equations were in good qualitative agreement.

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Husin, Nurul Aini, Jing Jing Khoo, Mulya Mustika Sari Zulkifli, Lesley Bell-Sakyi, and Sazaly AbuBakar. "Replication Kinetics of Rickettsia raoultii in Tick Cell Lines." Microorganisms 9, no. 7 (June 24, 2021): 1370. http://dx.doi.org/10.3390/microorganisms9071370.

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Rickettsia raoultii is one of the causative agents of tick-borne lymphadenopathy in humans. This bacterium was previously isolated and propagated in tick cell lines; however, the growth characteristics have not been investigated. Here, we present the replication kinetics of R. raoultii in cell lines derived from different tick genera (BME/CTVM23, RSE/PILS35, and IDE8). Tick cell cultures were infected in duplicate with cryopreserved R. raoultii prepared from homologous cell lines. By 12–14 days post infection, 100% of the cells were infected, as visualized in Giemsa-stained cytocentrifuge smears. R. raoultii growth curves, determined by rickettsiae-specific gltA qPCR, exhibited lag, exponential, stationary and death phases. Exponential phases of 4–12 days and generation times of 0.9–2.6 days were observed. R. raoultii in BME/CTVM23 and RSE/PILS35 cultures showed, respectively, 39.5- and 37.1-fold increases compared to the inoculum. In contrast, multiplication of R. raoultii in the IDE8 cultures was 110.1-fold greater than the inoculum with a 7-day stationary phase. These findings suggest variation in the growth kinetics of R. raoultii in the different tick cell lines tested, amongst which IDE8 cells could tolerate the highest levels of R. raoultii replication. Further studies of R. raoultii are needed for a better understanding of its persistence within tick populations.

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Berdnikov, V. I., and Yu A. Gudim. "Thermodynamic model of ideal associated solutions with positive deviation from Raoult’s law." Steel in Translation 44, no. 9 (September 2014): 635–39. http://dx.doi.org/10.3103/s0967091214090034.

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Hirata, Yoshihiro, Koichiro Matsushima, Shinichi Baba, Naoki Matsunaga, and Soichiro Sameshima. "Theoretical and Experimental Analyses of Colloidal Processing of Nanoparticles." Advances in Science and Technology 62 (October 2010): 131–40. http://dx.doi.org/10.4028/www.scientific.net/ast.62.131.

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The stability of dispersed and flocculated colloidal particles under 1 atm and applied pressure was discussed thermodynamically with the activity and chemical potential defined by Henry’s law and Raoult’s law. The calculated result under 1 atm is represented by a colloidal phase diagram as functions of surface potential and solid content of particles. Application of pressure accelerates the phase transition from dispersed to flocculated suspension. The phase transition pressure, which is observed in the applied pressure-suspension height relation during pressure filtration at a constant crosshead speed of piston, is affected by (1) particle concentration, (2) particle size, (3) surface potential, (4) degree of dissociation of polyelectrolyte dispersant and (5) applied electric field (DC and AC). The influence of above factors was discussed theoretically and experimentally.

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SHAH, WASEEM ULLAH, SYED MEHMOOD SHAH, MATIULLAH KHAN, DIL FARAZ KHAN, ATHANASIOS G. MAMALIS, and HAIQING YIN. "THERMODYNAMIC STUDY OF BINARY ALLOY SYSTEM (Co–Cr) USING CALPHAD METHOD." Surface Review and Letters 25, no. 02 (February 2018): 1850049. http://dx.doi.org/10.1142/s0218625x1850049x.

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This paper reports the thermodynamic analysis of (Co–Cr) system using THERMO-calc package (basis for CALPHAD) and PBIN database. Calculations involve binary phase diagram, Gibb’s energy curve and activity curve at three different elevated temperatures 2125[Formula: see text]K, 2150[Formula: see text]K and 2175[Formula: see text]K. Induced miscibility gap is observed at particular concentration. Binary phase diagram shows variation in phases in prescribed alloy with increasing temperature and mole fraction concentration of [Formula: see text]. The total Gibbs energy decreases with increasing temperature showing the stability of Co–Cr system. Activity showed thorough fluctuation resulting in negative deviation from Raoult’s law ideal curve.

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Journal articles on the topic 'Raoult's law'

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