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Journal ArticleDOI

Isothermal (vapor+liquid) equilibria of four binary mixtures

01 Jan 1984-The Journal of Chemical Thermodynamics (Academic Press)-Vol. 16, Iss: 1, pp 1-5
TL;DR: In this article, the isothermal equilibria of (acetone + tetrahydrofuran), (tetrahydroid-furan + acetonitrile), (Tetraydroid-furan + 1,2-dichloroethane), and (acetitrile + 1.2-dimethyl-1, 2-diclorosine) were measured at 302.15 K using the total-pressure method.
About: This article is published in The Journal of Chemical Thermodynamics.The article was published on 1984-01-01. It has received 16 citations till now. The article focuses on the topics: UNIQUAC & Tetrahydrofuran.
Citations
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Journal ArticleDOI
TL;DR: In this paper, the Kirkwood-Buff integrals and the volume-corrected preferential solvation parameters for the first solvation shell of binary mixtures of tetrahydrofuran with many organic solvents, calculated from reported thermodynamic data at the temperatures for which these data were available, are reported.
Abstract: The Kirkwood–Buff integrals and the volume-corrected preferential solvation parameters for the first solvation shell of binary mixtures of tetrahydrofuran with many organic solvents, calculated from reported thermodynamic data at the temperatures for which these data were available, are reported. The co-solvents include c-hexane, methyl-c-hexane, n-heptane, i-octane, benzene, toluene, ethylbenzene, 1-chlorobutane, dichloromethane, 1,2-dichloroethane, chloroform, 1,1,1-trichloroethane, tetrachlorom-ethane, tetrachloroethene, hexafluoro benzene, ethanol, 1-propanol, 2-propanol, dibutyl ether, acetic acid, acetone, dimethyl sulfoxide, tetramethylene sulfone (sulfolane), acetonitrile, pyrrolidine, and triethylamine. The preferential solvation parameters of these mixtures are discussed in terms of the interactions that occur.

126 citations


Cites methods from "Isothermal (vapor+liquid) equilibri..."

  • ...Excess Gibbs energy data for 303.15 K are available from Govindan et al. ( 23 ) and V E (xS) data at 298.15 K from Suri and Chawla, (24) and it was assumed that the temperature effect on V E (xS) over the 5 K interval is small and can be neglected....

    [...]

  • ...Excess Gibbs energy data for 303.15 K are available from Govindan et al. ( 23 ) and V E (xS) data at 298.15 K from Suri and Chowla, (24) and it was assumed that the temperature effect on V E (xS) over the 5 K interval is immaterial....

    [...]

  • ...Excess Gibbs energy data for 303.15 K are available from Govindan et al. ( 23 ) and V E (xS) data at 298.15 K from Suri and Chowla, (24) and it was assumed that the temperature effect on V E (xS) over the 5 K interval can be neglected....

    [...]

Journal ArticleDOI
TL;DR: In this article, the main solvent factors that aid partitioning into the ketones are polarizability/dipolarity, hydrogen-bond basicity and hydrophobicity of the ketone.
Abstract: Literature data on partitioning of compounds from the gas phase to ketones and from water to ketones has been collected and analyzed through the Abraham solvation equations. It is shown that for partition into both dry and wet ketones the main solvent factors that aid partitioning into the ketones are the polarizability/dipolarity, hydrogen-bond basicity and hydrophobicity (size) of the ketones. Reliable equations have been established for partitioning from the gas phase and from water to dry acetone, dry butanone, dry cyclohexanone and to wet methyl isobutyl ketone. It is further shown that partitioning into dry butanone and dry cyclohexanone leads to different equations than partitioning into the wet solvents, and that data on partitioning into the wet and dry ketones cannot be combined.

74 citations

Journal ArticleDOI
TL;DR: The solubility measurements in mixed solvent system can provide useful information about solvate formation and the estimated crystal energy term for C60 in tetrahydrofuran was different than that in the other solvents, indicating that the C60 solid phase in equilibrium with tetrahytochemical solution may be a solvated crystal.
Abstract: The potential large-scale production of fullerene C60 and its widespread use in consumer products may translate into occupational and public exposure and in long-term environmental exposure. To assess the risk and fate of C60 in the environment, it is important to understand its solvate formation in common industrial solvents as the solvates may affect various properties of C60 including reactivity and toxicity, particularly when solvates occur in C60 clusters. In this study, the solubility measurements in mixed solvent system can provide useful information about solvate formation. The solubility of C60 was measured in pure toluene, tetrahydrofuran, ethanol, and acetonitrile to be 3000, 11, 1.4, and 0.04 mg/L, respectively. Additionally, the solubility of C60 was measured in mixtures of toluene−acetonitrile, toluene−ethanol, toluene−tetrahydrofuran, and acetonitrile−tetrahydrofuran. The solubility data were modeled with some accuracy using Wohl’s equation. The estimated crystal energy term for C60 in tetr...

58 citations

Journal ArticleDOI
TL;DR: In this paper, the Kirkwood-Buff integrals and the volume-corrected preferential solvation parameters for the first solvation shell of binary mixtures of tetrahydrofuran with many organic solvents, calculated from reported thermodynamic data at the temperatures for which these data were available, are reported.
Abstract: The Kirkwood–Buff integrals and the volume-corrected preferential solvation parameters for the first solvation shell of binary mixtures of tetrahydrofuran with many organic solvents, calculated from reported thermodynamic data at the temperatures for which these data were available, are reported. The co-solvents include c-hexane, methyl-c-hexane, n-heptane, i-octane, benzene, toluene, ethylbenzene, 1-chlorobutane, dichloromethane, 1,2-dichloroethane, chloroform, 1,1,1-trichloroethane, tetrachlorom-ethane, tetrachloroethene, hexafluoro benzene, ethanol, 1-propanol, 2-propanol, dibutyl ether, acetic acid, acetone, dimethyl sulfoxide, tetramethylene sulfone (sulfolane), acetonitrile, pyrrolidine, and triethylamine. The preferential solvation parameters of these mixtures are discussed in terms of the interactions that occur.

37 citations

Journal ArticleDOI
TL;DR: In this article, the authors derived correlations between the water-to-1,2-dichloroethane partition coefficients and the Abraham solvation parameter model with standard deviations of 0.16 and 0.18 log units, respectively.

34 citations

References
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Journal ArticleDOI
TL;DR: In this article, the reliability and accuracy of the measured data are considered in terms of the activity coefficients and of the dependences of the molar excess Gibbs energies on composition of the data.

15 citations