Isothermal Vapor−Liquid Equilibrium of Ternary Mixtures Containing 2-Methyl-1-propanol or 2-Methyl-2-propanol, n-Hexane, and 1-Chlorobutane at 298.15 K

Abstract

Isothermal vapor-liquid equilibrium for the ternary mixtures 2-methyl-1-propanol + n-hexane + 1-chlorobutane and 2-methyl-2-propanol + n-hexane + 1-chlorobutane and for the binary mixtures 2-methyl1-propanol + n-hexane and 2-methyl-2-propanol + n-hexane have been studied at T ) 298.15 K. The experimental data were checked for thermodynamic consistency using the method of van Ness. The isothermal vapor-liquid equilibrium data of the ternary mixtures together with the corresponding constituent binary mixtures were correlated with the Wilson equation. The G E values obtained have been compared with those of the ternary mixtures 1-butanol or 2- butanol + n-hexane + 1-chlorobutane previously investigated. The study of vapor-liquid equilibrium (VLE) of multicomponent liquid mixtures in isothermal conditions provides experimental data of great interest in thermodynamics and chemical engineering and contributes decisively for the development of accurate methods to predict and correlate phase equilibrium. However, relatively few investigations on isothermal VLE of ternary mixtures can be found in the literature. In the past years, our laboratory has been involved in the study of several thermodynamic and transport properties of the ternary mixtures containing an isomer of butanol + n-hexane + 1-chlorobutane, 1-7 and we also have recently reported isothermal VLE data for the ternary systems 1-butanol or 2-butanol + n-hexane + 1-chlorobutane at 298.15 K. 8 To complete this systematic study, we report here vapor-liquid equilibrium data obtained at 298.15 K for the ternary systems 2-methyl-1-propanol or 2-methyl-2-propanol + n-hexane + 1-chlorobutane and for the binary mixtures 2-methyl-1-propanol or 2-methyl-2-propanol + n-hexane. Thermodynamic consistency of the experimental data has been checked by the method of van Ness. 9 We have also correlated activity coefficients of the components and excess Gibbs function of the mixtures using the Wilson equation. 10