Phase equilibria and the thermodynamic properties of methyl and ethyl esters of carboxylic acids. 1. Methyl n-butanoate and ethyl propanoate

The heat capacity of methyl n-butanoate in crystalline and liquid states was measured by vacuum adiabatic calorimetry over the temperature range from (8 to 372) K. The triple point temperature, the enthalpy and entropy of fusion, and the purity of the sample were determined. The saturated vapour pressure and the boiling temperatures were determined by comparative ebulliometry in the "atmospheric'' pressure range 10.8 6 <= (p/kPa) <= 6 99.6. The normal boiling temperature, T-n.b, and the enthalpy of vaporization at T = 298.15 K and T-n.b were derived. The thermodynamic functions (absolute entropy and changes of the enthalpy, and Gibbs free energy) were derived for the solid and liquid states in the temperature range studied and for the ideal gas state at T = 298.15 K. The ideal gas heat capacities and the absolute entropies of methyl n-butanoate (MeBu) and ethyl propanoate (EtPr) were calculated by statistical thermodynamics on the basis of the molecular constants determined by the use of density functional theory on the B3LYP level. The experimental vapour pressure of MeBu and EtPr [1] of moderate temperature intervals, Delta T-exp = (59/65) K, were extended to the entire range of the liquids, Delta T-liq = (364.7/345.7) K by the methods of the corresponding states law and simultaneous treatment of the pT-parameters and low-temperature heat capacities of the ideal gas and liquid, respectively. An additive contribution of the carbonyl group CO-(C,O) connected with C and O atoms was determined for calculation of the absolute molar entropies at T = 298.15 K, S-m(0)(g) (298 K), by additive Benson's scheme. (C) 2011 Elsevier Ltd. All rights reserved.