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Inmaculada Velasco - One of the best experts on this subject based on the ideXlab platform.
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Temperature and pressure dependence of the volumetric properties of binary liquid mixtures containing 1-propanol and dihaloalkanes
Physics and Chemistry of Liquids, 2005Co-Authors: V. Hernandez, Jose Munoz Embid, Pilar García-giménez, Manuela Artal, Inmaculada VelascoAbstract:Densities of 1-propanol + dibromomethane, or +bromochloromethane, or +1,2-diChloroethane, or +1-bromo-2-Chloroethane binary mixtures were measured at 288.15, 298.15 and 308.15 K, over the entire composition range. Thermal expansion coefficients, α, and excess molar volumes, , were calculated. Moreover, densities at 298.15 K and pressures up to 2 × 107 Pa were determined for the same mixtures. Isothermal compressibilities, κT, of the pure liquids and their mixtures were obtained.
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Temperature and Pressure Dependence of the Volumetric Properties of Binary Liquid Mixtures Containing Dihaloalkanes
International Journal of Thermophysics, 2005Co-Authors: Pilar García-giménez, Jose Munoz Embid, Inmaculada Velasco, V. Hernandez, Santos OtinAbstract:Densities of ethyl acetate + dibromomethane, + bromochloromethane, + 1,2-diChloroethane, or + 1-bromo-2-Chloroethane binary mixtures were measured at 288.15, 298.15, and 308.15 K over the entire composition range. Thermal expansion coefficients and excess molar volumes were calculated. Moreover, densities at 298.15 K at pressures up to 200 bar were determined for the same mixtures. Isothermal compressibilities of the pure liquids and their mixtures were obtained. The excess molar volumes are positive, and the excess isothermal compressibilities are negative for all the studied mixtures.
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vapour liquid equilibria for the binary mixtures 1 propanol dibromomethane or bromochloromethane or 1 2 diChloroethane or 1 bromo 2 Chloroethane at t 313 15 k
The Journal of Chemical Thermodynamics, 2005Co-Authors: Vanesa Gilhernandez, Pilar Garciagimenez, Manuela Artal, Santos Otin, Inmaculada VelascoAbstract:Abstract Isothermal (vapour + liquid) equilibria (VLE) at 313.15 K have been measured for liquid 1-propanol + dibromomethane, or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich–Kister equation taking into consideration the vapour phase imperfection in terms of the 2nd molar virial coefficients. The excess molar Gibbs free energies of all the studied mixtures are positive and ranging from 794 J · mol−1 for (1-propanol + bromochloromethane) and 1052 J · mol−1 for (1-propanol + 1-bromo-2-Chloroethane), at x = 0.5. The experimental results are compared with modified UNIFAC predictions.
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(Vapour + liquid) equilibria for the binary mixtures (1-propanol + dibromomethane, or + bromochloromethane, or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane) at T = 313.15 K
The Journal of Chemical Thermodynamics, 2005Co-Authors: V. Gil-hernández, Pilar García-giménez, Manuela Artal, Santos Otin, Inmaculada VelascoAbstract:Abstract Isothermal (vapour + liquid) equilibria (VLE) at 313.15 K have been measured for liquid 1-propanol + dibromomethane, or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich–Kister equation taking into consideration the vapour phase imperfection in terms of the 2nd molar virial coefficients. The excess molar Gibbs free energies of all the studied mixtures are positive and ranging from 794 J · mol−1 for (1-propanol + bromochloromethane) and 1052 J · mol−1 for (1-propanol + 1-bromo-2-Chloroethane), at x = 0.5. The experimental results are compared with modified UNIFAC predictions.
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isothermal vapor liquid equilibria of bromochloromethane or 1 bromo 2 Chloroethane tetrachloromethane or benzene experimental measurements and analysis in terms of group contributions
Fluid Phase Equilibria, 1999Co-Authors: Manuela Artal, Jose Munoz Embid, Santos Otin, Inmaculada VelascoAbstract:Abstract Isothermal vapor–liquid equilibria (VLE) have been measured for bromochloromethane+tetrachloromethane or benzene at 298.15 K and 313.15 K, and for 1-bromo-2-Chloroethane+tetrachloromethane or benzene at 313.15 K. Bromochloromethane+tetrachloromethane shows azeotropic behaviour in the temperature range covered. These experimental results, along with our previous ones on excess enthalpies, are interpreted with two group contribution models: DISQUAC (DISpersive-QUAsiChemical) and modified (Dortmund) UNIFAC (UNIquac Functional group Activity Coefficients).
Santos Otin - One of the best experts on this subject based on the ideXlab platform.
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Temperature and Pressure Dependence of the Volumetric Properties of Binary Liquid Mixtures Containing Dihaloalkanes
International Journal of Thermophysics, 2005Co-Authors: Pilar García-giménez, Jose Munoz Embid, Inmaculada Velasco, V. Hernandez, Santos OtinAbstract:Densities of ethyl acetate + dibromomethane, + bromochloromethane, + 1,2-diChloroethane, or + 1-bromo-2-Chloroethane binary mixtures were measured at 288.15, 298.15, and 308.15 K over the entire composition range. Thermal expansion coefficients and excess molar volumes were calculated. Moreover, densities at 298.15 K at pressures up to 200 bar were determined for the same mixtures. Isothermal compressibilities of the pure liquids and their mixtures were obtained. The excess molar volumes are positive, and the excess isothermal compressibilities are negative for all the studied mixtures.
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vapour liquid equilibria for the binary mixtures 1 propanol dibromomethane or bromochloromethane or 1 2 diChloroethane or 1 bromo 2 Chloroethane at t 313 15 k
The Journal of Chemical Thermodynamics, 2005Co-Authors: Vanesa Gilhernandez, Pilar Garciagimenez, Manuela Artal, Santos Otin, Inmaculada VelascoAbstract:Abstract Isothermal (vapour + liquid) equilibria (VLE) at 313.15 K have been measured for liquid 1-propanol + dibromomethane, or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich–Kister equation taking into consideration the vapour phase imperfection in terms of the 2nd molar virial coefficients. The excess molar Gibbs free energies of all the studied mixtures are positive and ranging from 794 J · mol−1 for (1-propanol + bromochloromethane) and 1052 J · mol−1 for (1-propanol + 1-bromo-2-Chloroethane), at x = 0.5. The experimental results are compared with modified UNIFAC predictions.
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(Vapour + liquid) equilibria for the binary mixtures (1-propanol + dibromomethane, or + bromochloromethane, or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane) at T = 313.15 K
The Journal of Chemical Thermodynamics, 2005Co-Authors: V. Gil-hernández, Pilar García-giménez, Manuela Artal, Santos Otin, Inmaculada VelascoAbstract:Abstract Isothermal (vapour + liquid) equilibria (VLE) at 313.15 K have been measured for liquid 1-propanol + dibromomethane, or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich–Kister equation taking into consideration the vapour phase imperfection in terms of the 2nd molar virial coefficients. The excess molar Gibbs free energies of all the studied mixtures are positive and ranging from 794 J · mol−1 for (1-propanol + bromochloromethane) and 1052 J · mol−1 for (1-propanol + 1-bromo-2-Chloroethane), at x = 0.5. The experimental results are compared with modified UNIFAC predictions.
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isothermal vapor liquid equilibria of ethyl acetate dibromomethane or bromochloromethane or 1 2 diChloroethane or 1 bromo 2 Chloroethane at t 313 15 k
Journal of Chemical & Engineering Data, 2004Co-Authors: Pilar Garciagimenez, Vanesa Gilhernandez, Jose Munoz Embid, Manuela Artal, Santos OtinAbstract:Isothermal vapor−liquid equilibria (VLE) at 313.15 K have been measured for liquid ethyl acetate + dibromomethane or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich−Kister equation by taking into consideration the vapor-phase nonideality in terms of the second molar virial coefficients, and the liquid activity coefficients were correlated by means of the Margules, van Laar, Wilson, NRTL, and UNIQUAC equations. The thermodynamic consistency of the experimental data was checked by means of the test of Van Ness et al. in the version of Fredenslund et al. The excess molar Gibbs energies of all of the studied mixtures are negative and range from −75 J mol-1 for ethyl acetate + 1-bromo-2-Chloroethane to −300 J mol-1 for ethyl acetate + bromochloromethane at a mole fraction of x = 0.5.
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Isothermal Vapor−Liquid Equilibria of Ethyl Acetate + Dibromomethane or + Bromochloromethane or + 1,2-DiChloroethane or +1-Bromo-2-Chloroethane at T = 313.15 K
Journal of Chemical & Engineering Data, 2004Co-Authors: Pilar García-giménez, Jose Munoz Embid, Manuela Artal, V. Hernandez, Santos OtinAbstract:Isothermal vapor−liquid equilibria (VLE) at 313.15 K have been measured for liquid ethyl acetate + dibromomethane or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich−Kister equation by taking into consideration the vapor-phase nonideality in terms of the second molar virial coefficients, and the liquid activity coefficients were correlated by means of the Margules, van Laar, Wilson, NRTL, and UNIQUAC equations. The thermodynamic consistency of the experimental data was checked by means of the test of Van Ness et al. in the version of Fredenslund et al. The excess molar Gibbs energies of all of the studied mixtures are negative and range from −75 J mol-1 for ethyl acetate + 1-bromo-2-Chloroethane to −300 J mol-1 for ethyl acetate + bromochloromethane at a mole fraction of x = 0.5.
Manuela Artal - One of the best experts on this subject based on the ideXlab platform.
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Temperature and pressure dependence of the volumetric properties of binary liquid mixtures containing 1-propanol and dihaloalkanes
Physics and Chemistry of Liquids, 2005Co-Authors: V. Hernandez, Jose Munoz Embid, Pilar García-giménez, Manuela Artal, Inmaculada VelascoAbstract:Densities of 1-propanol + dibromomethane, or +bromochloromethane, or +1,2-diChloroethane, or +1-bromo-2-Chloroethane binary mixtures were measured at 288.15, 298.15 and 308.15 K, over the entire composition range. Thermal expansion coefficients, α, and excess molar volumes, , were calculated. Moreover, densities at 298.15 K and pressures up to 2 × 107 Pa were determined for the same mixtures. Isothermal compressibilities, κT, of the pure liquids and their mixtures were obtained.
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vapour liquid equilibria for the binary mixtures 1 propanol dibromomethane or bromochloromethane or 1 2 diChloroethane or 1 bromo 2 Chloroethane at t 313 15 k
The Journal of Chemical Thermodynamics, 2005Co-Authors: Vanesa Gilhernandez, Pilar Garciagimenez, Manuela Artal, Santos Otin, Inmaculada VelascoAbstract:Abstract Isothermal (vapour + liquid) equilibria (VLE) at 313.15 K have been measured for liquid 1-propanol + dibromomethane, or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich–Kister equation taking into consideration the vapour phase imperfection in terms of the 2nd molar virial coefficients. The excess molar Gibbs free energies of all the studied mixtures are positive and ranging from 794 J · mol−1 for (1-propanol + bromochloromethane) and 1052 J · mol−1 for (1-propanol + 1-bromo-2-Chloroethane), at x = 0.5. The experimental results are compared with modified UNIFAC predictions.
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(Vapour + liquid) equilibria for the binary mixtures (1-propanol + dibromomethane, or + bromochloromethane, or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane) at T = 313.15 K
The Journal of Chemical Thermodynamics, 2005Co-Authors: V. Gil-hernández, Pilar García-giménez, Manuela Artal, Santos Otin, Inmaculada VelascoAbstract:Abstract Isothermal (vapour + liquid) equilibria (VLE) at 313.15 K have been measured for liquid 1-propanol + dibromomethane, or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich–Kister equation taking into consideration the vapour phase imperfection in terms of the 2nd molar virial coefficients. The excess molar Gibbs free energies of all the studied mixtures are positive and ranging from 794 J · mol−1 for (1-propanol + bromochloromethane) and 1052 J · mol−1 for (1-propanol + 1-bromo-2-Chloroethane), at x = 0.5. The experimental results are compared with modified UNIFAC predictions.
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isothermal vapor liquid equilibria of ethyl acetate dibromomethane or bromochloromethane or 1 2 diChloroethane or 1 bromo 2 Chloroethane at t 313 15 k
Journal of Chemical & Engineering Data, 2004Co-Authors: Pilar Garciagimenez, Vanesa Gilhernandez, Jose Munoz Embid, Manuela Artal, Santos OtinAbstract:Isothermal vapor−liquid equilibria (VLE) at 313.15 K have been measured for liquid ethyl acetate + dibromomethane or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich−Kister equation by taking into consideration the vapor-phase nonideality in terms of the second molar virial coefficients, and the liquid activity coefficients were correlated by means of the Margules, van Laar, Wilson, NRTL, and UNIQUAC equations. The thermodynamic consistency of the experimental data was checked by means of the test of Van Ness et al. in the version of Fredenslund et al. The excess molar Gibbs energies of all of the studied mixtures are negative and range from −75 J mol-1 for ethyl acetate + 1-bromo-2-Chloroethane to −300 J mol-1 for ethyl acetate + bromochloromethane at a mole fraction of x = 0.5.
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Isothermal Vapor−Liquid Equilibria of Ethyl Acetate + Dibromomethane or + Bromochloromethane or + 1,2-DiChloroethane or +1-Bromo-2-Chloroethane at T = 313.15 K
Journal of Chemical & Engineering Data, 2004Co-Authors: Pilar García-giménez, Jose Munoz Embid, Manuela Artal, V. Hernandez, Santos OtinAbstract:Isothermal vapor−liquid equilibria (VLE) at 313.15 K have been measured for liquid ethyl acetate + dibromomethane or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich−Kister equation by taking into consideration the vapor-phase nonideality in terms of the second molar virial coefficients, and the liquid activity coefficients were correlated by means of the Margules, van Laar, Wilson, NRTL, and UNIQUAC equations. The thermodynamic consistency of the experimental data was checked by means of the test of Van Ness et al. in the version of Fredenslund et al. The excess molar Gibbs energies of all of the studied mixtures are negative and range from −75 J mol-1 for ethyl acetate + 1-bromo-2-Chloroethane to −300 J mol-1 for ethyl acetate + bromochloromethane at a mole fraction of x = 0.5.
Donald R. Sadoway - One of the best experts on this subject based on the ideXlab platform.
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relative dielectric constant measurements in the butyronitrile Chloroethane system at subambient temperatures
Journal of The Electrochemical Society, 1997Co-Authors: Robin B. Michnick, Kevin G. Rhoads, Donald R. SadowayAbstract:By means of electrochemical impedance spectroscopy, the relative dielectric constant was measured as a function of composition and temperature in the butyronitrile-Chloroethane system from -35 to -105°C. A customized cell was designed by iterative optimization; the equivalent circuit was used to assess the impacts of the electrical properties of the sample, the limitations of the instrumentation, and the data reduction technique. To account for strong local ordering effects due to molecular association in these solutions, a new model, termed extended Kirkwood-Onsager (EKO), was developed. For solutions rich in Chloroethane, structural features are inferred with this model.
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Relative Dielectric Constant Measurements in the Butyronitrile‐Chloroethane System at Subambient Temperatures
Journal of The Electrochemical Society, 1997Co-Authors: Robin B. Michnick, Kevin G. Rhoads, Donald R. SadowayAbstract:By means of electrochemical impedance spectroscopy, the relative dielectric constant was measured as a function of composition and temperature in the butyronitrile-Chloroethane system from -35 to -105°C. A customized cell was designed by iterative optimization; the equivalent circuit was used to assess the impacts of the electrical properties of the sample, the limitations of the instrumentation, and the data reduction technique. To account for strong local ordering effects due to molecular association in these solutions, a new model, termed extended Kirkwood-Onsager (EKO), was developed. For solutions rich in Chloroethane, structural features are inferred with this model.
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Phase Diagram of Butyronitrile-Chloroethane Determined by Differential Thermal Analysis
The Journal of Physical Chemistry, 1996Co-Authors: Robin B. Michnick And, Donald R. SadowayAbstract:The temperature−composition phase diagram of the butyronitrile−Chloroethane system was determined by differential thermal analysis. The butyronitrile−Chloroethane system is a simple eutectic, the eutectic point being −185 °C (88 K) and 48 mol % butyronitrile. The thermodynamics of the liquid phase were tested against a number of solution models and were found to be best represented by the associated solution model with the solution consisting of free butyronitrile, free Chloroethane, and dimolecular complexes composed of one butyronitrile and one Chloroethane. This model was also used to estimate the vapor pressure of butyronitrile−Chloroethane solutions.
Jose Munoz Embid - One of the best experts on this subject based on the ideXlab platform.
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Temperature and pressure dependence of the volumetric properties of binary liquid mixtures containing 1-propanol and dihaloalkanes
Physics and Chemistry of Liquids, 2005Co-Authors: V. Hernandez, Jose Munoz Embid, Pilar García-giménez, Manuela Artal, Inmaculada VelascoAbstract:Densities of 1-propanol + dibromomethane, or +bromochloromethane, or +1,2-diChloroethane, or +1-bromo-2-Chloroethane binary mixtures were measured at 288.15, 298.15 and 308.15 K, over the entire composition range. Thermal expansion coefficients, α, and excess molar volumes, , were calculated. Moreover, densities at 298.15 K and pressures up to 2 × 107 Pa were determined for the same mixtures. Isothermal compressibilities, κT, of the pure liquids and their mixtures were obtained.
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Temperature and Pressure Dependence of the Volumetric Properties of Binary Liquid Mixtures Containing Dihaloalkanes
International Journal of Thermophysics, 2005Co-Authors: Pilar García-giménez, Jose Munoz Embid, Inmaculada Velasco, V. Hernandez, Santos OtinAbstract:Densities of ethyl acetate + dibromomethane, + bromochloromethane, + 1,2-diChloroethane, or + 1-bromo-2-Chloroethane binary mixtures were measured at 288.15, 298.15, and 308.15 K over the entire composition range. Thermal expansion coefficients and excess molar volumes were calculated. Moreover, densities at 298.15 K at pressures up to 200 bar were determined for the same mixtures. Isothermal compressibilities of the pure liquids and their mixtures were obtained. The excess molar volumes are positive, and the excess isothermal compressibilities are negative for all the studied mixtures.
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isothermal vapor liquid equilibria of ethyl acetate dibromomethane or bromochloromethane or 1 2 diChloroethane or 1 bromo 2 Chloroethane at t 313 15 k
Journal of Chemical & Engineering Data, 2004Co-Authors: Pilar Garciagimenez, Vanesa Gilhernandez, Jose Munoz Embid, Manuela Artal, Santos OtinAbstract:Isothermal vapor−liquid equilibria (VLE) at 313.15 K have been measured for liquid ethyl acetate + dibromomethane or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich−Kister equation by taking into consideration the vapor-phase nonideality in terms of the second molar virial coefficients, and the liquid activity coefficients were correlated by means of the Margules, van Laar, Wilson, NRTL, and UNIQUAC equations. The thermodynamic consistency of the experimental data was checked by means of the test of Van Ness et al. in the version of Fredenslund et al. The excess molar Gibbs energies of all of the studied mixtures are negative and range from −75 J mol-1 for ethyl acetate + 1-bromo-2-Chloroethane to −300 J mol-1 for ethyl acetate + bromochloromethane at a mole fraction of x = 0.5.
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Isothermal Vapor−Liquid Equilibria of Ethyl Acetate + Dibromomethane or + Bromochloromethane or + 1,2-DiChloroethane or +1-Bromo-2-Chloroethane at T = 313.15 K
Journal of Chemical & Engineering Data, 2004Co-Authors: Pilar García-giménez, Jose Munoz Embid, Manuela Artal, V. Hernandez, Santos OtinAbstract:Isothermal vapor−liquid equilibria (VLE) at 313.15 K have been measured for liquid ethyl acetate + dibromomethane or + bromochloromethane or + 1,2-diChloroethane or + 1-bromo-2-Chloroethane mixtures. The VLE data were reduced using the Redlich−Kister equation by taking into consideration the vapor-phase nonideality in terms of the second molar virial coefficients, and the liquid activity coefficients were correlated by means of the Margules, van Laar, Wilson, NRTL, and UNIQUAC equations. The thermodynamic consistency of the experimental data was checked by means of the test of Van Ness et al. in the version of Fredenslund et al. The excess molar Gibbs energies of all of the studied mixtures are negative and range from −75 J mol-1 for ethyl acetate + 1-bromo-2-Chloroethane to −300 J mol-1 for ethyl acetate + bromochloromethane at a mole fraction of x = 0.5.
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isothermal vapor liquid equilibria of bromochloromethane or 1 bromo 2 Chloroethane tetrachloromethane or benzene experimental measurements and analysis in terms of group contributions
Fluid Phase Equilibria, 1999Co-Authors: Manuela Artal, Jose Munoz Embid, Santos Otin, Inmaculada VelascoAbstract:Abstract Isothermal vapor–liquid equilibria (VLE) have been measured for bromochloromethane+tetrachloromethane or benzene at 298.15 K and 313.15 K, and for 1-bromo-2-Chloroethane+tetrachloromethane or benzene at 313.15 K. Bromochloromethane+tetrachloromethane shows azeotropic behaviour in the temperature range covered. These experimental results, along with our previous ones on excess enthalpies, are interpreted with two group contribution models: DISQUAC (DISpersive-QUAsiChemical) and modified (Dortmund) UNIFAC (UNIquac Functional group Activity Coefficients).