Henry’s law constants and infinite dilution activity coefficients of cis-2-butene, dimethylether, chloroethane, and 1,1-difluoroethane in methanol, 1-propanol, 2-propanol, 1-butanol, 2-butanol, isobutanol, tert-butanol, 1-pentanol, 2-pentanol, 3-pentanol, 2-methyl-1-butanol, 3-methyl-1-butanol, and 2-methyl-2-butanol

Miyano, Yoshimori; Kobashi, Takahiro; Shinjo, Hiroshi; Kumada, Shinya; Watanabe, Yusuke; Niya, Wataru; Tateishi, Yoko

doi:10.1016/j.jct.2005.08.004

Cited by 16 publications

(10 citation statements)

References 15 publications

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“…As observed in the previous paper, the infinite dilution activity coefficients for asymmetric mixtures (mixture of nonpolar + strong polar substances) strongly depend on the temperature, and the partial molar excess enthalpies for these asymmetric mixtures have large values in general. On the other hand, for symmetric mixtures such as (nonpolar + nonpolar) or (strong polar + strong polar), the partial molar excess enthalpies have small values in general and the activity coefficients have values near to unity.…”

Section: Resultssupporting

confidence: 70%

Henry's Law Constants and Infinite Dilution Activity Coefficients of Propane, Propene, Butane, 2-Methylpropane, 1-Butene, 2-Methylpropene, trans-2-Butene, cis-2-Butene, 1,3-Butadiene, Dimethyl Ether, Chloroethane, and 1,1-Difluoroethane in 2-Methyl-3-buten-2-ol and 3-Methyl-3-buten-1-ol

et al. 2005

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Henry's law constants and infinite dilution activity coefficients of propane, propene, butane, 2-methylpropane, 1-butene, 2-methylpropene, trans-2-butene, cis-2-butene, 1,3-butadiene, dimethyl ether, chloroethane, and 1,1-difluoroethane in 2-methyl-3-buten-2-ol and 3-methyl-3-buten-1-ol in the temperature range of (250 to 330) K were measured by a gas stripping method, and partial molar excess enthalpies were calculated from the activity coefficients. The estimated uncertainties are about 2 % for the Henry's law constants and 3 % for the infinite dilution activity coefficients. In general the Henry's law constants followed the order of increasing Henry's law constant with decreases in the normal boiling point temperature of the liquefied gas except for 1,3-butadiene, and the partial molar excess enthalpies of gases followed the order of increasing partial molar excess enthalpy with decreases of the polarity of the gases except for chloroethane and 1,1-difluoroethane.

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Section: Resultssupporting

confidence: 70%

Henry's Law Constants and Infinite Dilution Activity Coefficients of Propane, Propene, Butane, 2-Methylpropane, 1-Butene, 2-Methylpropene, trans-2-Butene, cis-2-Butene, 1,3-Butadiene, Dimethyl Ether, Chloroethane, and 1,1-Difluoroethane in 2-Methyl-3-buten-2-ol and 3-Methyl-3-buten-1-ol

et al. 2005

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“…As observed in a previous paper, the infinite dilution activity coefficients for asymmetric mixtures (mixture of nonpolar + strong polar substances) strongly depend on the temperature, and the partial molar excess enthalpies for these asymmetric mixtures have large values in general. On the other hand, for symmetric mixtures such as (nonpolar + nonpolar) or (strong polar + strong polar), the partial molar excess enthalpies have small values in general, and the activity coefficients of symmetric mixtures have values near to unity.…”

Section: Resultssupporting

confidence: 69%

Henry's Law Constants and Infinite Dilution Activity Coefficients of Propane, Propene, Butane, 2-Methylpropane, 1-Butene, 2-Methylpropene, trans-2-Butene, cis-2-Butene, 1,3-Butadiene, Dimethyl Ether, Chloroethane, and 1,1-Difluoroethane in 2-Propen-1-ol

Miyano

2005

J. Chem. Eng. Data

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Henry's law constants and infinite dilution activity coefficients of propane, propene, butane, 2-methylpropane, 1-butene, 2-methylpropene, trans-2-butene, cis-2-butene, 1,3-butadiene, dimethyl ether, chloroethane, and 1,1-difluoroethane in 2-propen-1-ol in the temperature range of (250 to 330) K were measured by a gas stripping method. Partial molar excess enthalpies were calculated from the activity coefficients. A rigorous formula for evaluating the Henry's law constants from the gas stripping measurements was used for the data reduction of these highly volatile mixtures. The estimated uncertainties are about 2 % for the Henry's law constants and 3 % for the infinite dilution activity coefficients. In the evaluation of the infinite dilution activity coefficients, the nonideality (fugacity coefficient) of the solute cannot be neglected, especially at higher temperatures. The estimated uncertainty of the infinite dilution activity coefficients includes 1 % for the nonideality. In general, the Henry's law constants followed the order of increasing Henry's law constant with decreases in the normal boiling point temperature of the liquefied gas except for 1,3-butadiene, and the partial molar excess enthalpies of gases followed the order of increasing partial molar excess enthalpy with decreases of the polarity of the gases.

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“…Enthalpies of solution of several gas molecules [97][98][99][100][101][102][103][104][105][106], anthracene [107], acenaphthene [108,…”

Section: Data Sets and Solute Descriptorsmentioning

confidence: 99%

Enthalpy of solvation correlations for organic solutes and gases dissolved in 2-propanol, 2-butanol, 2-methyl-1-propanol and ethanol

et al. 2011

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Data have been assembled from the published literature on the enthalpies of solvation for 91 organic vapors and gaseous solutes in 2-propanol, for 73 gaseous compounds in 2-butanol, for 85 gaseous compounds in 2-methyl-1-propanol and for 128 gaseous compounds in ethanol. It is shown that an Abraham solvation equation with five descriptors can be used to correlate the experimental solvation enthalpies to within standard deviations of 2.24 kJ/mole, 1.99 kJ/mole, 1.73 kJ/mole and 2.54 kJ/mole for 2-propanol, 2-butanol, 2-methyl-1-propanol and ethanol, respectively. The derived correlations provide very accurate mathematical descriptions of the measured enthalpy of solvation data at 298 K, which in the case of ethanol span a range of 136 kJ/mole. Division of the experimental values into a training set and a test set shows that there is no bias in predictions, and that the predictive capability of the correlations is better than 3.5 kJ/mole.

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Cited by 16 publications

References 15 publications

Henry's Law Constants and Infinite Dilution Activity Coefficients of Propane, Propene, Butane, 2-Methylpropane, 1-Butene, 2-Methylpropene, trans-2-Butene, cis-2-Butene, 1,3-Butadiene, Dimethyl Ether, Chloroethane, and 1,1-Difluoroethane in 2-Methyl-3-buten-2-ol and 3-Methyl-3-buten-1-ol

Henry's Law Constants and Infinite Dilution Activity Coefficients of Propane, Propene, Butane, 2-Methylpropane, 1-Butene, 2-Methylpropene, trans-2-Butene, cis-2-Butene, 1,3-Butadiene, Dimethyl Ether, Chloroethane, and 1,1-Difluoroethane in 2-Methyl-3-buten-2-ol and 3-Methyl-3-buten-1-ol

Henry's Law Constants and Infinite Dilution Activity Coefficients of Propane, Propene, Butane, 2-Methylpropane, 1-Butene, 2-Methylpropene, trans-2-Butene, cis-2-Butene, 1,3-Butadiene, Dimethyl Ether, Chloroethane, and 1,1-Difluoroethane in 2-Propen-1-ol

Enthalpy of solvation correlations for organic solutes and gases dissolved in 2-propanol, 2-butanol, 2-methyl-1-propanol and ethanol

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