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Journal articles on the topic 'Vapor-liquid equilibrium'

Author: Grafiati

Published: 4 June 2021

Last updated: 29 July 2024

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1

Wibowo, A. A., A. Mustain, M. Mufid, N. Hendrawati, A. W. Mustikarini, and S. Altway. "UNIFAC PREDICTION OF VAPOR LIQUID EQUILIBRIA INVOLVING GAMMA-VALEROLACTONE DERIVATIVE SYSTEMS." Azerbaijan Chemical Journal, no. 2 (May 7, 2024): 16–25. http://dx.doi.org/10.32737/0005-2531-2024-2-16-25.

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Researchers have studied the hydrogenation of Gamma-Valerolactone (GVL) over Ru/C to produce 2-methyltetrahydrofuran (2-MTHF), a biomass-based platform chemical with potential as a biofuel and green solvent. Other byproducts of this reaction include 2-butanol (2-BuOH), 2-pentanol (2-PeOH), and 1,4-pentanediol (1,4-PDO). In this study, UNIFAC activity coefficient models were used to predict the vapor-liquid equilibrium of several systems included in the process to explain the phase behavior which is important in purification process. The accuracy of the UNIFAC model is tested by comparing the experimental boiling points for the binary system of 2-propanol + 1-butanol and the vapor-liquid equi-librium of the GVL + 2-MTHF system. From this comparison, the Root Mean Square Deviation (RMSD) values for the boiling point measurements are obtained to be 3.153%, and for the liquid and vapor phases in the vapor-liquid equilibrium measurements, the RMSD values are 1.934% and 0.298% respectively. These RMSD values indicate the level of accuracy of the UNIFAC model in representing the experimental data for both boiling point measurements and vapor-liquid equilibrium phase behavior. The prediction results of vapor-liquid equilibrium data for GVL derivative systems showed that the 2-BuOH + 2-MTHF system does form an azeotrope when the mol fraction of 2-BuOH is 0.0031 at 79.780C. The calculation was performed using ChemCAD commercial software for chemical process modeling and simulation

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2

Renon, Henri. "Vapor-liquid equilibrium bibliographic database." Fluid Phase Equilibria 112, no. 1 (November 1995): 170–71. http://dx.doi.org/10.1016/0378-3812(95)90025-x.

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3

ZHANG, SHIMIN. "THE STABILITY OF LIQUID EVAPORATION EQUILIBRIUM." Surface Review and Letters 12, no. 01 (February 2005): 115–21. http://dx.doi.org/10.1142/s0218625x05006846.

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For the evaporation of the pure liquid under the condition of constant temperature and constant external pressure, the phase equilibrium of the liquid vapor in the bubble and the liquid outside the bubble is always a kind of stable equilibrium whether there is air or not in the bubble. If there is no air in the bubble, the bubble and liquid cannot coexist in the mechanical equilibrium when the vapor pressure of the liquid in the bubble is less than or equal to the external pressure; the bubble and liquid can coexist in an unstable equilibrium of mechanics when the vapor pressure of the liquid is greater than the external pressure. If there is air in the bubble, the bubble and liquid can coexist in a stable equilibrium of mechanics when the vapor pressure of the liquid is less than or equal to the external pressure; the bubble and liquid can coexist in a stable and an unstable equilibrium of mechanics when the vapor pressure of the liquid is greater than the external pressure and less than a certain pressure pm; the bubble and liquid cannot coexist in the mechanical equilibrium when the vapor pressure of the liquid is equal to or greater than pm.

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4

Oktavian, Rama, Agung Ari Wibowo, and Zuraidah Fitriah. "Study on Particle Swarm Optimization Variant and Simulated Annealing in Vapor Liquid Equilibrium Calculation." Reaktor 19, no. 2 (August 11, 2019): 77–83. http://dx.doi.org/10.14710/reaktor.19.2.77-83.

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Phase equilibrium calculation plays a major rule in optimization of separation process in chemical processing. Phase equilibrium calculation is still very challenging due to highly nonlinear and non-convex of mathematical models. Recently, stochastic optimization method has been widely used to solve those problems. One of the promising stochastic methods is Particle Swarm Optimization (PSO) due to its simplicity and robustness. This study presents the capability of particle swarm optimization for correlating isothermal vapor liquid equilibrium data of water with methanol and ethanol system by optimizing Wilson, Non-Random Two Liquids (NRTL), and Universal Quasi Chemical (UNIQUAC) activity coefficient model and also presents the comparison with bare-bones PSO (BBPSO) and simulated annealing (SA). Those three optimization methods were successfully tested and validated to model vapor liquid equilibrium calculation and were successfully applied to correlate vapor liquid equilibrium data for those types of systems with deviation less than 2%. In addition, BBPSO shows a consistency result and faster convergence among those three optimization methods. Keywords: Phase equilibrium, stochastic method, particle swarm optimization, simulated annealing and activity coefficient model

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5

Li, Xinyu, Baowei Niu, Wenjiao Ma, Wenying Zhao, Xiaoyan Sun, Li Xia, and Shuguang Xiang. "Equation of State Associated with Activity Coefficient Model Based on Elements and Chemical Bonds." Processes 11, no. 5 (May 15, 2023): 1499. http://dx.doi.org/10.3390/pr11051499.

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A new element- and chemical bond-dependent GE-EoS model(SRK-UNICAC) is proposed to consider the deviation of the vapor and liquid phases from the ideal state. The SRK-UNICAC model combines the UNICAC model and the SRK cubic equation of state. It uses the original interaction parameters of the UNICAC model and uses this model to calculate the GE. The SRK-UNICAC model predicted vapor-liquid equilibria for 87 binary systems under low- and medium-pressure conditions, 12 binary systems under high-pressure conditions, and 14 ternary systems; a comparison of the predictions with five other activity coefficient models were also made. The new model predicted the vapor-phase fraction and bubble-point pressure, and temperature for the binary system at high pressure, with a mean relative error of 3.75% and 6.58%, respectively. The mean relative errors of vapor-phase fraction and bubble-point temperature or bubble-point pressure for ternary vapor–liquid phase equilibrium were 6.50%, 4.76%, and 2.25%. The SRK-UNICAC model is more accurate in predicting the vapor–liquid phase equilibrium of high-pressure, non-polar, and polar mixtures and has a simpler and wider range of prediction processes. It can therefore be applied to the prediction of vapor–liquid equilibrium.

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6

Islam, Akand, and Vinayak Kabadi. "Universal liquid mixture model for vapor-liquid and liquid-liquid equilibria in hexane-butanol-water system over the temperature range 10 - 100 °C." Chemical and Process Engineering 32, no. 2 (June 1, 2011): 101–15. http://dx.doi.org/10.2478/v10176-011-0009-3.

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Universal liquid mixture model for vapor-liquid and liquid-liquid equilibria in hexane-butanol-water system over the temperature range 10 - 100 °C This is an extended research of the paper (Islam et al., 2011) conducted to obtain a universal set of interaction parameters of the model NRTL over the temperature range 10 - 100 °C for hexane-butanol-water system; meaning for binary pairs hexane-butanol, butanol-water and hexane-water; and for ternary system hexane-butanol-water. Thorough investigations of data selections for all binary pairs (Vapor-Liquid Equilibrium (VLE), Liquid-Liquid Equilibrium (LLE)), infinite dilution activity coefficient (γ∞), infinite dilution distribution coefficient (Dsw), excess enthalpy (HE), and for ternary system (LLE of hexane-butanol-water) were carried out. Finally quadratic temperature dependent interaction parameters were estimated regressing all the mentioned data and in each case calculated results were compared with literature values. The comparisons showed an overall percentage of error within 15% for the mentioned phase equilibrium calculations.

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7

Ilčin, Michal, Martin Michalík, Klára Kováčiková, Lenka Káziková, and Vladimír Lukeš. "Water liquid-vapor equilibrium by molecular dynamics: Alternative equilibrium pressure estimation." Acta Chimica Slovaca 9, no. 1 (April 1, 2016): 36–43. http://dx.doi.org/10.1515/acs-2016-0007.

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Abstract The molecular dynamics simulations of the liquid-vapor equilibrium of water including both water phases — liquid and vapor — in one simulation are presented. Such approach is preferred if equilibrium curve data are to be collected instead of the two distinct simulations for each phase separately. Then the liquid phase is not restricted, e.g. by insufficient volume resulting in too high pressures, and can spread into its natural volume ruled by chosen force field and by the contact with vapor phase as vaporized molecules are colliding with phase interface. Averaged strongly fluctuating virial pressure values gave untrustworthy or even unreal results, so need for an alternative method arisen. The idea was inspired with the presence of vapor phase and by previous experiences in gaseous phase simulations with small fluctuations of pressure, almost matching the ideal gas value. In presented simulations, the first idea how to calculate pressure only from the vapor phase part of simulation box were applied. This resulted into very simple method based only on averaging molecules count in the vapor phase subspace of known volume. Such simple approach provided more reliable pressure estimation than statistical output of the simulation program. Contrary, also drawbacks are present in longer initial thermostatization time or more laborious estimation of the vaporization heat. What more, such heat of vaporization suffers with border effect inaccuracy slowly decreasing with the thickness of liquid phase. For more efficient and more accurate vaporization heat estimation the two distinct simulations for each phase separately should be preferred.

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8

Gomis, Vicente, Ana Pequenín, and Juan Carlos Asensi. "Isobaric vapor–liquid–liquid equilibrium and vapor–liquid equilibrium for the system water–ethanol-1,4-dimethylbenzene at 101.3kPa." Fluid Phase Equilibria 281, no. 1 (July 2009): 1–4. http://dx.doi.org/10.1016/j.fluid.2009.03.024.

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9

Luo, T., and A. Yu Chirkov. "Thermodynamic Property Calculation in Vapor-Liquid Equilibrium for Multicomponent Mixtures using Highly Accurate Helmholtz Free Energy Equation of State." Herald of the Bauman Moscow State Technical University. Series Mechanical Engineering, no. 3 (138) (September 2021): 108–21. http://dx.doi.org/10.18698/0236-3941-2021-3-108-121.

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Thermodynamic properties of multicomponent mixtures in phase equilibrium were studied. The tangent plane criterion was used for stability analysis, and the Gibbs energy minimization was employed for phase equilibrium calculation when the successive substitution didn't converge. Thermodynamic properties of a 12-component natural gas mixture in vapor-liquid equilibrium were calculated with highly accurate Helmholtz free energy equation of state GERG--2008, simplified GERG--2008 and common cubic Peng --- Robinson (PR) equation of state. Results show that in vapor-liquid equilibrium, GERG--2008 has high accuracy and works better than simplified GERG--2008 and PR-equation of state. Simplified GERG--2008 and PR-equation of state both work unsatisfactorily in vapor-liquid equilibrium calculation, especially near the saturation zone. The deviation function in GERG--2008 can significantly affect the accuracy of GERG--2008 when calculating thermodynamic properties of mixtures in vapor-liquid equilibrium

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10

Yeh, G. C., B. V. Yeh, S. T. Schmidt, M. S. Yeh, A. M. McCarthy, and W. J. Celenza. "Vapor-liquid equilibrium in capillary distillation." Desalination 81, no. 1-3 (July 1991): 161–87. http://dx.doi.org/10.1016/0011-9164(91)85052-v.

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11

Palavra, A. M. F. "Vapor-liquid equilibrium at high temperature." Pure and Applied Chemistry 68, no. 8 (January 1, 1996): 1515–20. http://dx.doi.org/10.1351/pac199668081515.

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12

Frolkova, Anastasia V. "Topological Invariants of Vapor–Liquid, Vapor–Liquid–Liquid and Liquid–Liquid Phase Diagrams." Entropy 23, no. 12 (December 10, 2021): 1666. http://dx.doi.org/10.3390/e23121666.

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The study of topological invariants of phase diagrams allows for the development of a qualitative theory of the processes being researched. Studies of the properties of objects in the same equivalence class may be carried out with the aim of predicting the properties of unexplored objects from this class, or predicting the behavior of a whole system. This paper describes a number of topological invariants in vapor–liquid, vapor–liquid–liquid and liquid–liquid equilibrium diagrams. The properties of some invariants are studied and illustrated. It is shown that the invariant of a diagram with a miscibility gap can be used to distinguish equivalence classes of phase diagrams, and that the balance equation of the singular-point indices, based on the Euler characteristic, may be used to analyze the binodal-surface structure of a quaternary system.

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13

Seybold, Paul G., Matthew J. O'Malley, Lemont B. Kier, and Chao-Kun Cheng. "Cellular Automata Simulations of Vapor–Liquid Equilibria." Australian Journal of Chemistry 59, no. 12 (2006): 865. http://dx.doi.org/10.1071/ch06230.

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Phase transitions and phase equilibria are among the most fundamental phenomena in the physical and environmental sciences. In the present work an asynchronous stochastic cellular automata model for the equilibrium between a liquid and its vapor is presented. The model is visual, dynamic, and employs just two rules—an attraction probability and a gravitational preference. Application of the attraction rule alone yields a ‘mist’ within the vapor, whereas application of the gravitational rule by itself yields an isothermal atmospheric profile. Application of both rules together causes the vapor to evolve to a liquid phase with a vapor phase above it. Introduction of a third rule for short-range attraction/repulsion more clearly resolves the liquid/vapor interface.

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14

Malijevská, Ivona. "Evaluation of Heterodimerization Constant from Solid-Liquid and Vapor-Liquid Equilibrium Data." Collection of Czechoslovak Chemical Communications 65, no. 9 (2000): 1497–505. http://dx.doi.org/10.1135/cccc20001497.

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Activity coefficients obtained from the solid-liquid equilibrium data were used to fit the isobaric vapor-liquid equilibrium data to evaluate the vapor-phase equilibrium constant of heterodimerization of the system propanoic acid-trifluoroethanoic acid. The found hetero-dimerization constant is several times higher than that estimated on the basis of the "double-geometric-mean" rule and its temperature dependence has the form ln KAB = 7 196.7/T - 26.80.

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15

Johansson, Erik, Kim Bolton, and Peter Ahlström. "Simulations of vapor water clusters at vapor–liquid equilibrium." Journal of Chemical Physics 123, no. 2 (July 8, 2005): 024504. http://dx.doi.org/10.1063/1.1953532.

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16

Folas, Georgios K., Georgios M. Kontogeorgis, Michael L. Michelsen, and Erling H. Stenby. "Vapor–liquid, liquid–liquid and vapor–liquid–liquid equilibrium of binary and multicomponent systems with MEG." Fluid Phase Equilibria 249, no. 1-2 (November 2006): 67–74. http://dx.doi.org/10.1016/j.fluid.2006.08.021.

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17

Pequenín, Ana, Juan Carlos Asensi, and Vicente Gomis. "Quaternary isobaric (vapor+liquid+liquid) equilibrium and (vapor+liquid) equilibrium for the system (water+ethanol+cyclohexane+heptane) at 101.3kPa." Journal of Chemical Thermodynamics 43, no. 8 (August 2011): 1097–103. http://dx.doi.org/10.1016/j.jct.2011.02.016.

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18

Tang, Hong Bo, and Min Qing Zhang. "Thermodynamic Model for Vapor-Liquid Phase Equilibrium in an Exerted Magnetic Field." Advanced Materials Research 550-553 (July 2012): 2704–11. http://dx.doi.org/10.4028/www.scientific.net/amr.550-553.2704.

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Many researchers have shown a great deal of interest in the effects that magnetic fields have when applied in chemical reactions, crystallization, magnetic separation of materials, magnetic levitation, materials processing, and wastewater treatment. However, surprisingly little research has been done on the effects of magnetic fields on the vapor-liquid equilibrium and the thermodynamic model for vapor-liquid phase equilibrium. The influence of magnetic fields on vapor-liquid equilibrium of binary heterogeneous azeotrope was investigated with ethanol-water in this paper. It was found that the vapor-liquid equilibrium of an ethanol-water system is influenced by the external magnetic field, but that the azeotropic point of the ethanol-water system is not changed by the magnetic field when the magnetic intensity reaches 0.8 T. Rather, the exerted magnetic field reduces the equilibrium temperature and shortens the distance between T-x curve and T-y curve in T-x-y diagram of the vapor-liquid equilibrium of the ethanol-water system. A thermodynamic model for vapor-liquid phase equilibrium in the exerted magnetic field was derived theoretically, based on the fundamental thermodynamic theory. The results show that the logarithm value of the ratio of the composition of the certain component in a magnetic field to that without the magnetic field is proportional to the magnetic susceptibility of the solution, and to the square of magnetic field intensity. This template explains and demonstrates how to prepare your camera-ready paper for Trans Tech Publications. The best is to read these instructions and follow the outline of this text.

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19

Dubrovskii, Vladimir G. "Composition of Vapor–Liquid–Solid III–V Ternary Nanowires Based on Group-III Intermix." Nanomaterials 13, no. 18 (September 11, 2023): 2532. http://dx.doi.org/10.3390/nano13182532.

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Compositional control in III–V ternary nanowires grown by the vapor–liquid–solid method is essential for bandgap engineering and the design of functional nanowire nano-heterostructures. Herein, we present rather general theoretical considerations and derive explicit forms of the stationary vapor–solid and liquid–solid distributions of vapor–liquid–solid III–V ternary nanowires based on group-III intermix. It is shown that the vapor–solid distribution of such nanowires is kinetically controlled, while the liquid–solid distribution is in equilibrium or nucleation-limited. For a more technologically important vapor-solid distribution connecting nanowire composition with vapor composition, the kinetic suppression of miscibility gaps at a growth temperature is possible, while miscibility gaps (and generally strong non-linearity of the compositional curves) always remain in the equilibrium liquid–solid distribution. We analyze the available experimental data on the compositions of the vapor–liquid–solid AlxGa1−xAs, InxGa1−xAs, InxGa1−xP, and InxGa1−xN nanowires, which are very well described within the model. Overall, the developed approach circumvents uncertainty in choosing the relevant compositional model (close-to-equilibrium or kinetic), eliminates unknown parameters in the vapor–solid distribution of vapor–liquid–solid nanowires based on group-III intermix, and should be useful for the precise compositional tuning of such nanowires.

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20

Sun, Li, Jierong Liang, and Tingting Zhu. "A Numerical Study of Vapor–Liquid Equilibrium in Binary Refrigerant Mixtures Based on 2,3,3,3-Tetrafluoroprop-1-ene." Sustainability 15, no. 19 (October 4, 2023): 14482. http://dx.doi.org/10.3390/su151914482.

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The binary refrigerant mixtures containing 2,3,3,3-Tetrafluoroprop-1-ene are considered as excellent substitutes for traditional refrigerants. Weak hydrogen bonds exist in hydrofluorocarbons and hydrofluoroolefins. However, for several recently published binary refrigerant mixtures, there is no Vapor–Liquid Equilibrium calculation study considering hydrogen-bonding associations. This work presents a calculation work of the saturated properties of nine pure refrigerants using the Cubic-Plus-Association Equation of State, considering the hydrogen-bonding association in refrigerant fluids. The average relative deviations of the saturated vapor pressure, liquid, and vapor density are less than 1.0%, 1.5%, and 3.5%, respectively. The Vapor–Liquid Equilibrium of ten binary refrigerant mixtures containing 2,3,3,3-Tetrafluoroprop-1-ene is also calculated using the Cubic-Plus-Association Equation of State with the van der Waals mixing rule. The average relative deviations of the liquid-phase and vapor-phase mole fractions are less than 1.0% and 2.0%, respectively. Moreover, the Vapor–Liquid Equilibrium data and the model’s adaptability are analyzed and discussed.

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21

Andrea Jia Xin Lai, Tomoya Tsuji, Katsumi Tochigi, Lian See Tan, Hiroyuki Matsuda, and Kiyofumi Kurihara. "Prediction of Phase Equilibria and Transport Properties Using ASOG and PRASOG Group Contribution Methods: A Review." Journal of Advanced Research in Fluid Mechanics and Thermal Sciences 102, no. 2 (February 27, 2023): 66–80. http://dx.doi.org/10.37934/arfmts.102.2.6680.

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Half century has passed since the first version of Analytical Solution of Groups (ASOG) model was proposed. Now the ASOG model is well known as a group contribution method as well as UNIFAC. Although the ASOG model was designed for prediction of vapor-liquid equilibrium around the atmospheric pressure, the applications are extended to not only the phase equilibria in the wide temperature and pressure ranges but also the transport properties. The function forms in the ASOG model, basically composed of Flory-Huggins equation and Wilson equation, can be applied for the prediction of the phase equilibria (vapor-liquid, liquid-liquid, solid-liquid and vapor-solid) and the transport properties (kinematic viscosity, thermal conductivity) of the mixtures with some modifications.

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22

Pequenín, Ana, Juan Carlos Asensi, and Vicente Gomis. "Isobaric Vapor−Liquid−Liquid Equilibrium and Vapor−Liquid Equilibrium for the Quaternary System Water−Ethanol−Cyclohexane−Isooctane at 101.3 kPa." Journal of Chemical & Engineering Data 55, no. 3 (March 11, 2010): 1227–31. http://dx.doi.org/10.1021/je900604a.

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23

Penttilä, Anne, Petri Uusi-Kyyny, and Ville Alopaeus. "Distillable Protic Ionic Liquid 2-(Hydroxy)ethylammonium Acetate (2-HEAA): Density, Vapor Pressure, Vapor–Liquid Equilibrium, and Solid–Liquid Equilibrium." Industrial & Engineering Chemistry Research 53, no. 49 (November 26, 2014): 19322–30. http://dx.doi.org/10.1021/ie503823a.

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24

Reddy, P. Swapna, and K. Yamuna Rani. "A Simple Algorithm for Vapor–Liquid–Liquid Equilibrium Computation." Industrial & Engineering Chemistry Research 51, no. 32 (July 31, 2012): 10719–30. http://dx.doi.org/10.1021/ie2022064.

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25

Freitas, F. F. Martins, Fernando M. S. Silva Fernandes, and B. J. Costa Cabral. "Vapor-Liquid Equilibrium and Structure of Methyl Iodide Liquid." Journal of Physical Chemistry 99, no. 14 (April 1995): 5180–86. http://dx.doi.org/10.1021/j100014a045.

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26

Thomsen, Kaj, Martin Due Olsen, and Lucas F. F. Corrêa. "Modeling vapor-liquid-liquid-solid equilibrium for acetone-water-salt system." Pure and Applied Chemistry 92, no. 10 (October 25, 2020): 1663–72. http://dx.doi.org/10.1515/pac-2019-1013.

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AbstractA compilation of available experimental data for acetone-water mixtures with the reciprocal salt system Na+, K+ || Cl−, SO42− is presented. Significant inconsistencies among experimental data are pointed out. New freezing point measurements are reported for the binary acetone-water system at 12 different compositions. UNIQUAC parameters are determined on the basis of the available data from literature. Modeling results are presented. Vapor-liquid, liquid-liquid, and solid-liquid equilibria together with thermal properties are reproduced well by the model using only 14 parameters. The major drawback of the model is that the calculated liquid-liquid equilibrium regions of systems with KCl and NaCl are larger than the experimentally determined regions. The model is valid in the temperature range from −16 to 100 °C.

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27

Mathis, Hélène. "A thermodynamically consistent model of a liquid-vapor fluid with a gas." ESAIM: Mathematical Modelling and Numerical Analysis 53, no. 1 (January 2019): 63–84. http://dx.doi.org/10.1051/m2an/2018044.

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This work is devoted to the consistent modeling of a three-phase mixture of a gas, a liquid and its vapor. Since the gas and the vapor are miscible, the mixture is subjected to a non-symmetric constraint on the volume. Adopting the Gibbs formalism, the study of the extensive equilibrium entropy of the system allows to recover the Dalton’s law between the two gaseous phases. In addition, we distinguish whether phase transition occurs or not between the liquid and its vapor. The thermodynamical equilibria are described both in extensive and intensive variables. In the latter case, we focus on the geometrical properties of equilibrium entropy. The consistent characterization of the thermodynamics of the three-phase mixture is used to introduce two Homogeneous Equilibrium Models (HEM) depending on mass transfer is taking into account or not. Hyperbolicity is investigated while analyzing the entropy structure of the systems. Finally we propose two Homogeneous Relaxation Models (HRM) for the three-phase mixtures with and without phase transition. Supplementary equations on mass, volume and energy fractions are considered with appropriate source terms which model the relaxation towards the thermodynamical equilibrium, in agreement with entropy growth criterion.

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28

Gomis, V., A. Font, R. Pedraza, and M. D. Saquete. "Isobaric vapor–liquid and vapor–liquid–liquid equilibrium data for the system water+ethanol+cyclohexane." Fluid Phase Equilibria 235, no. 1 (August 2005): 7–10. http://dx.doi.org/10.1016/j.fluid.2005.07.015.

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29

Gomis, V., A. Font, R. Pedraza, and M. D. Saquete. "Isobaric vapor–liquid and vapor–liquid–liquid equilibrium data for the water–ethanol–hexane system." Fluid Phase Equilibria 259, no. 1 (October 2007): 66–70. http://dx.doi.org/10.1016/j.fluid.2007.04.011.

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30

Yao, Ganbing, Zhipeng Yang, Bin Zhang, Hui Xu, and Hongkun Zhao. "Vapor pressure and isobaric vapor–liquid equilibrium for dichloronitrobenzene isomers." Fluid Phase Equilibria 367 (April 2014): 103–8. http://dx.doi.org/10.1016/j.fluid.2014.01.034.

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31

Berberan-Santos, Mário N., Evgeny N. Bodunov, and Lionello Pogliani. "Liquid–vapor equilibrium in a gravitational field." American Journal of Physics 70, no. 4 (April 2002): 438–43. http://dx.doi.org/10.1119/1.1424264.

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32

Leu, Ah-Dong, and Donald B. Robinson. "Vapor−Liquid Equilibrium for Four Binary Systems." Journal of Chemical & Engineering Data 44, no. 3 (May 1999): 398–400. http://dx.doi.org/10.1021/je980213s.

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33

Bosse, Dennis, and Hans-Jörg Bart. "Binary Vapor−Liquid Equilibrium Predictions with COSMOSPACE." Industrial & Engineering Chemistry Research 44, no. 23 (November 2005): 8873–82. http://dx.doi.org/10.1021/ie0487991.

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34

Boudreaux, Andrew, and Craig Campbell. "Student Understanding of Liquid–Vapor Phase Equilibrium." Journal of Chemical Education 89, no. 6 (April 24, 2012): 707–14. http://dx.doi.org/10.1021/ed2000473.

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35

Samin, Sela, and Yoav Tsori. "Vapor−Liquid Equilibrium in Electric Field Gradients." Journal of Physical Chemistry B 115, no. 1 (January 13, 2011): 75–83. http://dx.doi.org/10.1021/jp107529n.

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36

Łuszczyk, Marek, and Stanisław K. Malanowski. "Vapor−Liquid Equilibrium in α-Methylbenzenemethanol + Water." Journal of Chemical & Engineering Data 51, no. 5 (September 2006): 1735–39. http://dx.doi.org/10.1021/je060157s.

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37

Łuszczyk, Marek, and Stanisław K. Malanowski. "Vapor−Liquid Equilibrium in α-Methylbenzenemethanol + Water." Journal of Chemical & Engineering Data 51, no. 6 (November 2006): 2276. http://dx.doi.org/10.1021/je0604333.

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38

Wu, Huey S., and Stanley I. Sandler. "Vapor-liquid equilibrium of 1,3-dioxolane systems." Journal of Chemical & Engineering Data 34, no. 2 (April 1989): 209–13. http://dx.doi.org/10.1021/je00056a019.

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39

Renon, H. "Vapor—Liquid Equilibrium Data Collection, Vol. 1." Fluid Phase Equilibria 21, no. 1-2 (January 1985): 175. http://dx.doi.org/10.1016/0378-3812(85)90072-x.

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40

Renon, H. "Vapor—Liquid Equilibrium Data Bibliography Supplement III." Fluid Phase Equilibria 34, no. 1 (January 1987): 112. http://dx.doi.org/10.1016/0378-3812(87)85055-0.

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41

Liu, Yixiong, and R. M. German. "Contact angle and solid-liquid-vapor equilibrium." Acta Materialia 44, no. 4 (April 1996): 1657–63. http://dx.doi.org/10.1016/1359-6454(95)00259-6.

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42

Tamson, J., M. Mair, and S. Grohmann. "Vapor-liquid equilibrium of the nitrogen-argon system at 100 K." IOP Conference Series: Materials Science and Engineering 1240, no. 1 (May 1, 2022): 012159. http://dx.doi.org/10.1088/1757-899x/1240/1/012159.

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Abstract Mixed-refrigerant cycles (MRC) are state-of-the-art for efficient LNG production. The development of cryogenic mixed-refrigerant cycles (CMRC) at temperatures below 100 K relies on physical property data of cryogenic mixtures such as vapor-liquid equilibria and enthalpies. This data is insufficient for some binary mixtures and unavailable for most multi-component systems. The cryogenic phase equilibria test stand CryoPHAEQTS provides precise physical property data of cryogenic fluid mixtures at temperatures from 15 K to 300K and at pressures up to 150 bar. Contrary to previous apparatus in the literature, CryoPHAEQTS uses cooling of the equilibrium cell by a pulse-tube cryocooler. Temperature is measured by two CERNOX® sensors directly immersed in the liquid/vapor phase. Pressure is measured through a capillary and a differential pressure sensor connected to a secondary system containing three high precision sensors. Up to three occurring phases can be sampled directly from the cell and analyzed by gas chromatography. Measurement uncertainties are ±13mK in temperature, ±1 mbar in pressure and ±1% in composition. Prior to publishing new phase equilibrium data, the test stand is benchmarked against available vapor-liquid equilibrium data of the widely investigated nitrogen-argon system. In this paper, we report on the first measurement results of cryogenic mixtures in CryoPHAEQTS and compare them against the literature data.

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ZHANG, SHIMIN. "THE STABILITY OF VAPOR CONDENSATION EQUILIBRIUM." Surface Review and Letters 12, no. 03 (June 2005): 359–68. http://dx.doi.org/10.1142/s0218625x05007141.

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The system must get across an energy peak of unstable equilibrium during the condensation of pure vapor; as the supersaturated extent of vapor increases and the temperature decreases, the energy peak shortens and vapor condensation becomes easier. The system must get across an energy peak of unstable equilibrium first, and then get into an energy valley of stable equilibrium during the condensation of impure vapor; as the partial pressure of vapor decreases, the energy peak becomes taller, the energy valley more shallow, vapor condensation becomes more difficult and liquid evaporation becomes easier; when the partial pressure of vapor decreases to a certain extent, the energy peak and the energy valley combine into one, and vapor condensation becomes impossible.

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Gu, Feiyan, Lihua Wang, and Zhaoli Wu. "Vapor−Liquid and Liquid−Liquid Equilibrium for Octane + Maleic Anhydride System." Journal of Chemical & Engineering Data 47, no. 4 (July 2002): 643–47. http://dx.doi.org/10.1021/je000383g.

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Biryukov, D. A., D. N. Gerasimov, and E. I. Yurin. "Evaporation of a liquid, initiated by condensation of vapor on its surface." Journal of Physics: Conference Series 2088, no. 1 (November 1, 2021): 012002. http://dx.doi.org/10.1088/1742-6596/2088/1/012002.

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Abstract The paper considers mechanisms of initiation of liquid evaporation by contact with hot vapor (with temperature greater and much greater than the temperature of liquid). Two fundamentally different mechanisms of such initiation are distinguished - equilibrium and non-equilibrium. The process of non-equilibrium initiation of evaporation by hot vapor was studied using the method of molecular dynamics; the results agree with the theoretical estimate given in the work for determining the temperature of the beginning of the non-equilibrium mechanism of evaporation initiation.

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A. Mohammed, Ghazwan, Mahmoud O. Abdullah, and Talib B. Kashmoula. "Vapor-Liquid-Liquid Equilibrium (VLLE) Data for the Systems Ethyl acetate + Water, Toluene + Water and Toluene + Ethyl acetate + Water at 101.3 kPa. Using Modified Equilibrium Still." Iraqi Journal of Chemical and Petroleum Engineering 12, no. 3 (September 30, 2011): 1–10. http://dx.doi.org/10.31699/ijcpe.2011.3.1.

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Isobaric Vapor-Liquid-Liquid equilibrium data for the binary systems ethyl acetate + water, toluene + water and the ternary system toluene + ethyl acetate + water were determined by a modified equilibrium still, the still consisted of a boiling and a condensation sections supplied with mixers that helped to correct the composition of the recycled condensed liquid and the boiling temperature readings in the condensation and boiling sections respectively. The VLLE data where predicted and correlated using the Peng-Robinson Equation of State in the vapor phase and one of the activity coefficient models Wilson, NRTL, UNIQUAC and the UNIFAC in the liquid phase and also were correlated using the Peng-Robinson Equation of State in both the vapor and liquid phases.

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Luo, Weiping, Mengqi Yan, XiaoXiao Sheng, Bao Tao, Sile Shi, Wei Deng, Weijun Yang, and Siqi Luo. "A Unified Thermodynamics Model for Solid–Liquid Equilibrium, Liquid–Liquid Equilibrium, and Vapor–Liquid Equilibrium of Cyclohexane Oxidation Systems: NRTL Model." Industrial & Engineering Chemistry Research 58, no. 23 (May 16, 2019): 10018–30. http://dx.doi.org/10.1021/acs.iecr.9b00921.

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Cai, Jialin, Xianbao Cui, Ying Zhang, Rui Li, and Tianyang Feng. "Vapor−Liquid Equilibrium and Liquid−Liquid Equilibrium of Methyl Acetate + Methanol + 1-Ethyl-3-methylimidazolium Acetate." Journal of Chemical & Engineering Data 56, no. 2 (February 10, 2011): 282–87. http://dx.doi.org/10.1021/je100932m.

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Li, Rui, Xianbao Cui, Ying Zhang, Tianyang Feng, and Jialin Cai. "Vapor–Liquid Equilibrium and Liquid–Liquid Equilibrium of Ethyl Acetate + Ethanol + 1-Ethyl-3-methylimidazolium Acetate." Journal of Chemical & Engineering Data 57, no. 3 (February 13, 2012): 911–17. http://dx.doi.org/10.1021/je200869q.

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Subha, R., S. Praveena, B. V. S. Ramesh, Usha, and D. H. L. Prasad. "Vapor−Liquid Equilibrium in Methyl Ethyl Ketone + Ketazine and Liquid−Liquid Equilibrium in Water + Ketazine Mixtures." Journal of Chemical & Engineering Data 46, no. 6 (November 2001): 1497–98. http://dx.doi.org/10.1021/je010051r.

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