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Inmaculada Velasco - One of the best experts on this subject based on the ideXlab platform.
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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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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).
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excess volumes of bromochloromethane or 1 bromo 2 chloroethane heptane or cyclohexane or benzene or tetrachloromethane at the temperature 298 15 k
The Journal of Chemical Thermodynamics, 1995Co-Authors: Manuela Artal, Inmaculada Velasco, Munoz J Embid, S ToinAbstract:Abstract Excess molar volumesVEmof [x(BrCH2ClorBrCH2CH2Cl) + (1 -x){CH3(CH2)5CH3orc-(CH2)6or C6H6or CCl4}] have been determined from density measurements at the temperature 298.15 K, using a vibrating-tube densimeter. Excess molar volumesVEmfor these mixtures are positive, but noticeably less positive when C6H6or CCl4is the second substance.
Manuela Artal - One of the best experts on this subject based on the ideXlab platform.
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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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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 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).
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excess volumes of bromochloromethane or 1 bromo 2 chloroethane heptane or cyclohexane or benzene or tetrachloromethane at the temperature 298 15 k
The Journal of Chemical Thermodynamics, 1995Co-Authors: Manuela Artal, Inmaculada Velasco, Munoz J Embid, S ToinAbstract:Abstract Excess molar volumesVEmof [x(BrCH2ClorBrCH2CH2Cl) + (1 -x){CH3(CH2)5CH3orc-(CH2)6or C6H6or CCl4}] have been determined from density measurements at the temperature 298.15 K, using a vibrating-tube densimeter. Excess molar volumesVEmfor these mixtures are positive, but noticeably less positive when C6H6or CCl4is the second substance.
Santos Otin - One of the best experts on this subject based on the ideXlab platform.
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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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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 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).
Pilar Garciagimenez - One of the best experts on this subject based on the ideXlab platform.
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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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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.
Vanesa Gilhernandez - One of the best experts on this subject based on the ideXlab platform.
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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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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.
