1-Bromo-2-Chloroethane

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Inmaculada Velasco - One of the best experts on this subject based on the ideXlab platform.

Manuela Artal - One of the best experts on this subject based on the ideXlab platform.

Santos Otin - One of the best experts on this subject based on the ideXlab platform.

Pilar Garciagimenez - One of the best experts on this subject based on the ideXlab platform.

  • 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, 2005
    Co-Authors: Vanesa Gilhernandez, Pilar Garciagimenez, Manuela Artal, Santos Otin, Inmaculada Velasco
    Abstract:

    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.

  • 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, 2004
    Co-Authors: Pilar Garciagimenez, Vanesa Gilhernandez, Jose Munoz Embid, Manuela Artal, Santos Otin
    Abstract:

    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.

  • 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, 2005
    Co-Authors: Vanesa Gilhernandez, Pilar Garciagimenez, Manuela Artal, Santos Otin, Inmaculada Velasco
    Abstract:

    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.

  • 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, 2004
    Co-Authors: Pilar Garciagimenez, Vanesa Gilhernandez, Jose Munoz Embid, Manuela Artal, Santos Otin
    Abstract:

    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.