2002
DOI: 10.1006/jcht.2001.0877
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Excess thermodynamic properties of the ethylene carbonate–trifluoroethyl methyl carbonate and propylene carbonate–trifluoroethyl methyl carbonate systems at T= (298.15 or 315.15) K

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Cited by 59 publications
(25 citation statements)
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“…Ethylene carbonate is the only one demonstrating a large increase in entropy when LiF is dissolved: sol S 0 (LiF/EC) = 84.2 J K −1 mol −1 . Owing to the high symmetry of the molecule, EC is a structured solvent as indicated by the Kirkwood parameter value (g = 1.41 [11]) which is more than unity. In the solid state and, to a lesser extent, in solution, EC molecules are associated in pairs of opposite dipole moments like ␥-butyrolactone [13].…”
Section: H2omentioning
confidence: 99%
See 1 more Smart Citation
“…Ethylene carbonate is the only one demonstrating a large increase in entropy when LiF is dissolved: sol S 0 (LiF/EC) = 84.2 J K −1 mol −1 . Owing to the high symmetry of the molecule, EC is a structured solvent as indicated by the Kirkwood parameter value (g = 1.41 [11]) which is more than unity. In the solid state and, to a lesser extent, in solution, EC molecules are associated in pairs of opposite dipole moments like ␥-butyrolactone [13].…”
Section: H2omentioning
confidence: 99%
“…Polar solvents exhibit also a dipole moment which helps to dissolve salts by means of Van der Waals ion-dipole interactions as well as Lewis acid-base interactions. The electrostatic factor, f, (which is the product of dipole moment and dielectric constant), the molar polarization, P M , the Hildebrand parameter, ı, [10] and the Kirkwood parameter, g, [11], are also useful tools to analyse the solvating power of compounds. The solubility parameters of the alkylcarbonates under study are summarized in Table 3.…”
Section: Lif Solubilitiesmentioning
confidence: 99%
“…Presumably, the steric hindrance due to the presence of the methyl group in PC is responsible for its weaker structuredness respect to that of ethylene carbonate [33].…”
Section: Solubility Of Electrolytes and Ion Solvation In Pcmentioning
confidence: 99%
“…50 To calculate the activity coefficients, we place a single molecule of cation/anion at the center of a simulation cell with sides 20Å × 20Å × 20Å and calculate the electrolyte effect on solvation free energies (∆∆Ω) as a function of the electrolyte concentration (c ∞ i ). The mean activity coefficient is then calculated using equations (53) and (54). We consider two systems: electrolytes in aqueous and non-aqueous solvents which show negative and positive deviations from ideal solutions.…”
Section: A Activity Coefficientsmentioning
confidence: 99%