Excess molar enthalpies of {methanol or ethanol + (2-butanone + benzene)} at 298.15 K

Excess molar enthalpies of (acetonitrile + butan-2-one) and (methanol+ acetonitrile + butan-2-one) atT= 298.15 K

“…The values of the association constants are the same as reported (1,4) previously for methanol; K 2 = 70, K 3 = 120, K = 100, and θ = 90 at T = 298.15 K; and for acetonitrile, K B = 8.7 and K B = 2.1 at T = 318.15 K. The enthalpies of the hydrogen bond formation are: h 2 = −21.2 kJ · mol −1 for the methanol dimer, h 3 = 2h−h 2 for the trimer, and h = −23.5 kJ · mol −1 for the higher polymers including the cyclic case; and h B = −8.7 kJ · mol −1 for the acetonitrile dimer and h B = −6.7 kJ · mol −1 for the acetonitrile polymer. The enthalpies of formation for these chemical equilibria were assumed to be independent of temperature.…”

“…(10) The binary parameters of the (methanol + acetonitrile) and (methanol + butan-2-one) were the same as those taken from the previous papers (1,4) and the non-randomness parameter α ji was set as 0.3 for all systems. Table 4 gives the binary parameters and the absolute arithmetic-mean deviations, |H E m | , between the binary experimental and calculated values.…”

“…The experimental H E m s for the binary and ternary mixtures were analysed by means of an association model based on mole fraction statistics (1,4) and an extended Flory-Huggins association model. (2,3) The detailed descriptions of these models are given elsewhere, so we describe an outline of the models shortly.…”

“…(1,2) As parts of the thermodynamic studies for the ternary mixtures containing associated molecules, we have carried out the measurements of excess molar enthalpies H E m for the ternary mixtures containing alcohol, acetonitrile, and polar components. (3,4) In this paper we report experimental binary and ternary H E m for {xCH 3 CN + (1 − x)CH 3 COCH 2 CH 3 } and {x 1 CH 3 OH + x 2 CH 3 CN + (1 − x 1 − x 2 )CH 3 COCH 2 CH 3 } at T = 298.15 K, measured by using a flow microcalorimeter. The binary results are correlated by using association models taking account into the self-association of methanol and acetonitrile as well as solvation between unlike molecules with allowance for non-polar interactions.…”

Experimental and theoretically estimated excess molar enthalpies for (ethyl propionate+n -hexane + 1-pentanol) atT= 298.15 K

“…The binary experimental data were fitted with a variable degree polynomial due to Redlich-Kister. (6) The ternary contribution to the excess enthalpy was correlated on the basis of the Cibulka (7) and Nagata and Tamura (8) equations. Ternary magnitude contributions were also used in two equations proposed in an earlier study.…”