Excess enthalpies and isothermal (vapour + liquid) equilibria of (1-methyl-2-pyrrolidone + 1-chloroalkane or +α,ω-dichloroalkane) mixtures
Introduction
The thermodynamic behaviour of mixtures containing amides is of considerable interest, not only because of the high polarity of these compounds [1] but also because they contain both the amino and the carbonyl group being used as simple models in biochemistry [2]. In this work we have studied the thermodynamic behaviour of a cyclic amide, 1-methyl-2-pyrrolidone in a polar medium which is different from water. The polar compounds used as second component are 1-chloroalkanes [3] or α,ω-dichloroalkanes [4] used widely in chemical industry as intermediates or final products.
Following with our studies on the thermodynamics of binary liquid mixtures containing amides and haloalkanes [5], [6], we report here the excess enthalpy , at T = (298.15 and 308.15) K, for liquid (1-methyl-2-pyrrolidone + 1-chlorobutane, or +1-chlorohexane, or +1-chlorooctane, or +1,2-dichloroethane, or +1,4-dichlorobutane, or +1,6-dichlorohexane) and the isothermal (vapor + liquid) equilibria (VLE), at T = (313.15, 323.15, and 333.15) K, for (1-methyl-2-pyrrolidone + 1-chlorobutane, or +1-chlorohexane, or +1,2-dichloroethane).
As far as we know, the only previous measurements on these mixtures are those for (1-methyl-2-pyrrolidone + 1,2-dichloroethane): at T = 298.15 K and the isobaric (vapour + liquid) equilibrium at 95.3 kPa [7].
Section snippets
Materials
1-Methyl-2-pyrrolidone (better than 99 mol% pure) and 1-chlorobutane (better than 99.8 mol% pure) were obtained from Riedel-de Häen. 1-Chlorooctane (better than 98 mol% pure), 1,2-dichloroethane (better than 99.5 mol% pure), and 1,4-dichlorobutane (better than 97 mol% pure) were supplied from Fluka AG Buchs, and 1-chlorohexane (better than 99.0 mol% pure) and 1,6-dichlorohexane (better than 98 mol% pure) were obtained from Aldrich Chem. Co. All the liquids were used without further purification.
In
Results and discussion
The experimental values, at T = (298.15 and 308.15) K, are collected in table 2 and are plotted as a function of the mole fraction, at T = 298.15 K, in figure 1. These results are fitted using the Redlich–Kister equation,where N is the total number of measurements and n is the number of coefficients Aj.
The coefficients Aj and the standard deviation calculated as follows:where N is the total number of measurements and n is the
Acknowledgements
P. García-Giménez acknowledges the financial support received by D.G.A, Departamento de Educación y Ciencia and the European Social Fund (B020/2003).
The authors are grateful for the financial assistance of D.G.A. to the G.E.T.T.A Group of research.
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