Topological and thermodynamic investigations of molecular interactions in binary mixtures: Molar excess volumes and molar excess enthalpies

Densities, surface tensions, and derived surface thermodynamics properties of (trimethylbenzene+propyl acetate, or butyl acetate) from T=298.15K to 313.15K

“…It implies that the interaction between unlike molecules is very similar to the intramolecular interaction. Maken et al [28] reported the excess molar volumes of butyl acetate with benzene, toluene or xylene at T = 308.15 K. The absolute values of V E for the binary systems are also small. The results may be owing to the strength of the interactions between the acetate molecules that are nearly the same as those between acetate and benzene molecules.…”

Topological studies of molecular interactions of formamide with propanol and butanol at 298.15K

“…In spite of this qualitative description of the present V E m data, the degree of association of formamide and influence of alkanol on it remains to be investigated. For this purpose we analyzed the present V E m data in terms of an approach [12,13,19], that employs [20] the graph theoretical concept of molecular connectivity parameter of the third degree, 3 j, of the constituents of these mixtures.…”

Excess Gibbs free energy of butyl acetate with cyclohexane and aromatic hydrocarbons at 308.15K

“…These were taken from the literature [36] and reported in Table 4. Further, though the reduced density of the mixtures can in principle be evaluated from the following equation of state of the mixture proposed by Lacombe and Sanchez [39] (21) where for the binary mixture (22) (23) (24) (25) yet very few mixtures actually satisfy [40][41][42] this equation of state.…”

“…In our earlier paper [21], the measured V E and H E data for n-butyl acetate+cyclohexane or benzene or toluene or o-or mor p-xylene were interpreted in terms of a graph theoretical approach [22]. In this paper, we are reporting the excess molar Gibbs free energies of mixing (G E ) for these systems at 308.15±0.01 K calculated from the measured vapor pressure data using Barker's method [23].…”