Abstract
Molar excess enthalpies are reported for the systems (C2H5)3N + CDCl3, (C2H5)2O + CDCl3 and (C2H5)2O + CHCl3 at 298.15 K. Vapour pressures are reported for the system (C2H5)3N + CDCl3 at 283.15 K. The results are analysed in terms of the ideal associated solution model and the equilibrium constants and standard enthalpies of complex formation obtained are compared with spectroscopic values. Difference between the thermodynamic properties of corresponding CDCl3 and CHCl3 systems are discussed in terms of differences between the equilibrium constants and standard enthalpies of formation of the deuterium-bond and hydrogen-bond complexes. An analysis of calorimetric results at 298.15 K suggests that the equilibrium constant is smaller for the (C2H5)3N—CDCl3 complex than for the (C2H5)3N—CHCl3 complex, but that the magnitude of the standard enthalpy of formation is greater for the (C2H5)3N—CDCl3 complex.
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Schedule a callMore From: Journal of the Chemical Society, Faraday Transactions 1: Physical Chemistry in Condensed Phases
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