Thermodynamic properties of rigid polycyclic molecules

Excess molar enthalpies and volumes of binary mixtures of nonafluorobutylmethylether with ethylene glycol ethers at T=298.15K

“…This affect appears similarly to the value of V E;1 m;2 for this system.Values of H E;1 m;2 , D vap H 2 , D solv H 2 and V 1 m;2 are linearly related to V 2 for all the mixtures as shown in figures 7 and 8. The result supported the group contribution theory proposed by Barker and his co-workers[11][12][13], and the additive properties of the atomic group in D solv H i and V 1 m;i for aromatic hydrocarbon with multiple condensed ring systems reported recently by Ogawa et al and Ohba et al[14,15].…”

“…Excess molar enthalpies, H E m plotted against x for the nonafluorobutylmethylether (1) + ethylene glycol monoalkylether(2) systems at T = 298 15. K: (d) {xC 4 F 9 -O-CH 3 + (1 À x)CH 3 -OCH 2 CH 2 -OH}; (m) {xC 4 F 9 -O-CH 3 + (1 À x)CH 3 CH 2 -OCH 2 CH 2 -OH}; ---, {xC 4 F 9 -O-CH 3 + (1 À x)CH 3 (CH 2 ) 2 -OCH 2 CH 2 -OH}; and (n) {xC 4 F 9 -O-CH 3 + (1 À x)CH 3 (CH 2 ) 3 -OCH 2 CH 2 -OH}.EGE2,1-OCH 3 liquids, and dipolar, dispersion, and the hydrogen bonding intermolecular interactions in the pure EGEn,m-OH liquid.…”

Enthalpies of solution, partial molar volumes and isentropic compressibilities of polycyclic aromatic hydrocarbons in 1-methyl-2-pyrrolidone at 298.15K

“…The linear dependence of V ∞ m,1 and K ∞ s,m,1 is better shown by the series of zigzag structures than that of linear structures and includ- ing o-terphenyl. Such a variation for V ∞ m,1 can be explained using the Reference Interaction Site Model-Percus-Yevick approximation (RISM-PY) integral equation theory with the hard core sphere model by Ohba et al [2]. RISM integral equation theory was proposed to calculate the radial distribution function of liquid mixture by Chandler and Andersen [13].…”

“…The values of solv H and V ∞ m,1 for benzene and naphthalene dissolved in NMP compared with those in other solvents taken from our previous results [1,2] as listed in Table 5. The values of solv H of benzene and naphthalene in the polar solvents are larger than those in the non-polar solvents.…”

“…In the previous papers [1,2], enthalpies of solvation, solv H, and partial molar volumes at infinite dilution, V ∞ m,1 , of polycyclic aromatic hydrocarbons in different types of organic solvents were reported. Linear dependence, through the origin, on the number of carbon atoms contained in the solvated molecules was shown for all obtained data; these results were explained by the group contribution principle [3][4][5].…”