Molecular Interactions in Binary Mixtures of Lactams with Cyclic Alkanones

Sharma, V.K.; Kataria, Jyoti; Solanki, S.

doi:10.1007/s10953-014-0152-9

Cited by 18 publications

(3 citation statements)

References 49 publications

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“…The relative permittivity ε r is the crucial parameter in the molecular solvent system and it usually can be used to measure the polarity of molecular solvents. In this work, the values of refractive index, n D , molar volume, V m , and Δ l g H m o (298) were collected from the literature, − and according to eqs – δ μ of some molecular solvents were obtained. These are listed in Table , and the corresponding relative permittivity ε r for these molecular solvents were collected − and also listed in Table .…”

Section: Resultsmentioning

confidence: 99%

Determination and Prediction for the Polarity of Ionic Liquids

Guan¹,

Chang²,

Yang³

et al. 2017

J. Chem. Eng. Data

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Ionic liquids (ILs) have attracted remarkable attention as a new class of novel reaction medium and soft functional materials in the framework of Green Chemistry, and the polarity of ionic liquids is one of the primary concerns in the scientific community. Here, we introduce a new and simple scale of polarity, δ μ , for ILs. Initially, two kinds of representative ionic liquids, {1-alkyl-3-methyllimidazolium acetate}) are prepared and confirmed by 1 H NMR spectroscopy and 13 C NMR spectroscopy, respectively. Furthermore, a spectroscopic method based on solvatochromic probes is used to obtain the polarity of room temperature ILs (RTILs). In this work we mainly introduce that the scale of solvent polarity, E T (30) values, is determined by means of Reichardt's dye (30), and π* values are determined by N,N-diethyl-4-nitroaniline. Simultaneously, in terms of the values of enthalpy of vaporization, δ μ values of these ILs are predicted. Moreover, the trend of δ μ values of the ionic liquids with the different alkyl chains are the same as the E T (30) and π* values. In addition, the new scale of polarities δ μ of some molecular liquids are also predicted, and the results are in good agreement with relative permittivity, ε r .

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Section: Resultsmentioning

confidence: 99%

Determination and Prediction for the Polarity of Ionic Liquids

Guan¹,

Chang²,

Yang³

et al. 2017

J. Chem. Eng. Data

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“…33 The standard uncertainty in temperature measurement is 0.01 K. The measured densities ρ, speeds of sound u, and heat capacities C P , of purified liquids at studied temperatures are listed in Table 2 and also compared with the literature values. [34][35][36][37][38][39][40][41][42][43][44][45][46][47][48][49]56 The excess molar enthalpies, H E , heat capacities, C P of (1 + 2) mixtures and molar heat capacities of pure liquids were measured as a function of composition in a microdifferential scanning calorimeter [model-μ DSC 7 EVO] that has been described elsewhere. 50,51 The calorimeter uses a double-temperature control peltiercooler and works between 228.15 to 393.15 K. A constant sweeping of nitrogen gas for about 4 h (0.3−0.4 MPa pressure) was supplied to avoid steam condensation in the calorimetric walls, and 0.08 MPa pressure of nitrogen gas was maintained after this period.…”

Section: Methodsmentioning

confidence: 99%

“…The working frequency for density and sound analyzer is 3 MHz . The standard uncertainty in temperature measurement is 0.01 K. The measured densities ρ, speeds of sound u , and heat capacities C P , of purified liquids at studied temperatures are listed in Table and also compared with the literature values. − , …”

Section: Methodsmentioning

confidence: 99%

Thermodynamic Studies of Molecular Interactions in Mixtures Containing Tetrahydropyran, 1,4-Dioxane, and Cyclic Ketones

2017

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The densities ρ, speeds of sound u, and molar heat capacities C P of tetrahydropyran or 1,4-dioxane (1) + cyclohexanone or cycloheptanone (2) mixtures at 293.15, 298.15, 303.15, and 308.15 K, and excess molar enthalpies, H E at 308.15 K and atmospheric pressure 0.1 MPa have been measured over the entire composition range. The excess molar volumes V E, excess isentropic compressibilities κS E, and excess heat capacities, C P E of the studied mixtures have been determined using the measured experimental data. The observed V E, κS E, H E, and C P E data have been tested in terms of graph theory. The analyses of V E data by graph theory suggest that while tetrahydropyran or 1,4-dioxane exists as a mixture of monomer and dimer; cyclohexanone or cycloheptanone exists as a mixture of open and cyclic dimer. Further, (1 + 2) mixtures are characterized by interactions between oxygen atom/s and hydrogen atom of tetrahydropyran or 1,4-dioxane with hydrogen atom/s and oxygen atom of cyclohexanone or cycloheptanone. The quantum mechanical calculations and analysis of IR spectral data of (1 + 2) mixtures also support this viewpoint. It has been observed that graph theory correctly predicts the V E, κS E, H E, and C p E data of the present mixtures.

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