Abstract:Densities and vapor-liquid equilibria were determined for tetrahydrofuran with propan-1-ol and propan-2-ol systems at 298.15 K. From the experimental results, excess molar volumes and excess Gibbs free energies were calculated. Information could be obtained from the possible interaction between both chemical species in the two systems. The Prigogine–Flory–Patterson method was applied to calculate excess molar volumes. Liquid activity coefficients were calculated and correlated with different expressions existi… Show more
“…Plot of V E at 298.15 K for { x THF + (1 − x )1-alkanol} mixtures: ○, this work; · and ___ , literature data agreeing with ours; ,,, gray symbols, other literature data. − Labels: ( a ), methanol; ( b ), ethanol; ( c ), 1-propanol; ( d ), 1-butanol.…”
Section: Resultssupporting
confidence: 55%
“…Dashed lines stand for the behavior of the homologous THP series 4 Plot of V E at 298.15 K for { x THF + (1 − x )1-alkanol} mixtures: ○, this work; · and ___ , literature data agreeing with ours; ,,, gray symbols, other literature data. − Labels: ( a ), methanol; ( b ), ethanol; ( c ), 1-propanol; ( d ), 1-butanol.
3 Redlich−Kister Coefficients and Standard Deviation s for the Systems Containing THF a A 1 A 2 A 3 A 4 A 5 s x THF + (1 − x )Nonane H E /J·mol -1 3590.2 474 0 441 538 2.7 x THF + (1 − x )Methanol 10 6 · V E /m 3 ·mol -1 −0.6091 0.1359 0.00069 C p E /J·mol -1 ·K -1 8.820 4.22 0 −3.5 0.057 x THF + (1 − x )Ethanol C p E /J·mol -1 ·K -1 12.365 1.93 −2.36 −1.65 0.018 x THF + (1 − x )1-Propanol C p E /J·mol -1 ·K -1 8.592 0.723 −2.44 0 −2.28 0.013 x THF + (1 − x )1-Butanol C p E /J·mol -1 ·K -1 5.473 0.968 −2.23 −0.26 −3.90 0.0051 x THF + (1 − x )1-Hexanol C p E /J·mol -1 ·K -1 −0.125 1.34 −6.01 0.027 x THF + (1 − x )1-Heptanol C p E /J·mol -1 ·K -1 −3.780 1.933 −6.20 −1.03 0.010 x THF + (1 − x )1-Octanol C p E /J·mol -1 ·K -1 −8.01 2.20 −7.45 0.044 x THF + (1 − x )1-Nonanol C p E /J·mol -1 ·K -1 −10.488 2.03 −7.64 0.032 x THF + (1 − x )1-Decanol 10 6 ·...
…”
Section: Resultsmentioning
confidence: 72%
“… 5 Plot of V E ( x = 0.5) versus C-atom number, n , of the alkanol for the series {THF + 1-alkanol} at 298.15 K. From right to left and from top to bottom: +, Piñeiro et al; gray cross, this work; ◇, Amigo et al; ◆, Canzonieri et al; ·, Chawla and Suri; ○, Valén et al; □, Keller et al. ; ▪, Salas et al; − , Hall and Hall ( x = 0.5036); ▵, Lepori and Matteoli; -, Matous et al Dashed line stands for the behavior of the homologous THP series 6 Plots of C p E and C p E / x (1 − x ) at 298.15 K for { x THF + (1 − x )1-alkanol} mixtures: □, methanol; ▪, ethanol; ◇, 1-propanol; ◆, 1-butanol; ▵, 1-hexanol; ▴, 1-heptanol; ○, 1-octanol; ·, 1-nonanol; *, 1-decanol.…”
Section: Resultsmentioning
confidence: 83%
“…In Figures , , and 5, smoothed values at equimolar fraction for H E or V E are plotted versus the C-atom number of the linear compound of the mixture. The collected data come from this work and from an extensive review of the literature. ,,− These plots allow us to visualize the trend of excess property changes when increasing the alkane or alkanol chain length and assist in a few cases in the comparison between our values and those previously reported by others.…”
Densities, F, and volumetric heat capacities, C p /V, have been measured at 298.15 K over the whole mole fraction range for the binary mixtures {tetrahydrofuran + methanol, + ethanol, + 1-propanol, + 1-butanol, + 1-hexanol, + 1-heptanol, + 1-octanol, + 1-nonanol, or + 1-decanol}. From experimental data, the excess molar isobaric heat capacities, C p E , were calculated. Excess molar volumes, V E , are reported for the systems containing methanol and 1-decanol. The apolar homomorph concept has been used in semiquantitative calculations intended to assess and to compare the degrees of heteroassociation in these mixtures by getting an approximation to the corresponding negative enthalpic contributions at equimolar fraction, H int . With this aim, excess molar enthalpies, H E , of {tetrahydrofuran + nonane} and {cyclopentane + 1-butanol, + 1-pentanol, + 1-hexanol, + 1-heptanol, + 1-octanol, + 1-nonanol, or + 1-decanol} have been measured at 298.15 K. The results are discussed in terms of molecular interactions. Particularly, the various steps of W-shape concentration dependence found in the C p E point to the occurrence of local nonrandomness in {THF + alkanol} mixtures.
“…Plot of V E at 298.15 K for { x THF + (1 − x )1-alkanol} mixtures: ○, this work; · and ___ , literature data agreeing with ours; ,,, gray symbols, other literature data. − Labels: ( a ), methanol; ( b ), ethanol; ( c ), 1-propanol; ( d ), 1-butanol.…”
Section: Resultssupporting
confidence: 55%
“…Dashed lines stand for the behavior of the homologous THP series 4 Plot of V E at 298.15 K for { x THF + (1 − x )1-alkanol} mixtures: ○, this work; · and ___ , literature data agreeing with ours; ,,, gray symbols, other literature data. − Labels: ( a ), methanol; ( b ), ethanol; ( c ), 1-propanol; ( d ), 1-butanol.
3 Redlich−Kister Coefficients and Standard Deviation s for the Systems Containing THF a A 1 A 2 A 3 A 4 A 5 s x THF + (1 − x )Nonane H E /J·mol -1 3590.2 474 0 441 538 2.7 x THF + (1 − x )Methanol 10 6 · V E /m 3 ·mol -1 −0.6091 0.1359 0.00069 C p E /J·mol -1 ·K -1 8.820 4.22 0 −3.5 0.057 x THF + (1 − x )Ethanol C p E /J·mol -1 ·K -1 12.365 1.93 −2.36 −1.65 0.018 x THF + (1 − x )1-Propanol C p E /J·mol -1 ·K -1 8.592 0.723 −2.44 0 −2.28 0.013 x THF + (1 − x )1-Butanol C p E /J·mol -1 ·K -1 5.473 0.968 −2.23 −0.26 −3.90 0.0051 x THF + (1 − x )1-Hexanol C p E /J·mol -1 ·K -1 −0.125 1.34 −6.01 0.027 x THF + (1 − x )1-Heptanol C p E /J·mol -1 ·K -1 −3.780 1.933 −6.20 −1.03 0.010 x THF + (1 − x )1-Octanol C p E /J·mol -1 ·K -1 −8.01 2.20 −7.45 0.044 x THF + (1 − x )1-Nonanol C p E /J·mol -1 ·K -1 −10.488 2.03 −7.64 0.032 x THF + (1 − x )1-Decanol 10 6 ·...
…”
Section: Resultsmentioning
confidence: 72%
“… 5 Plot of V E ( x = 0.5) versus C-atom number, n , of the alkanol for the series {THF + 1-alkanol} at 298.15 K. From right to left and from top to bottom: +, Piñeiro et al; gray cross, this work; ◇, Amigo et al; ◆, Canzonieri et al; ·, Chawla and Suri; ○, Valén et al; □, Keller et al. ; ▪, Salas et al; − , Hall and Hall ( x = 0.5036); ▵, Lepori and Matteoli; -, Matous et al Dashed line stands for the behavior of the homologous THP series 6 Plots of C p E and C p E / x (1 − x ) at 298.15 K for { x THF + (1 − x )1-alkanol} mixtures: □, methanol; ▪, ethanol; ◇, 1-propanol; ◆, 1-butanol; ▵, 1-hexanol; ▴, 1-heptanol; ○, 1-octanol; ·, 1-nonanol; *, 1-decanol.…”
Section: Resultsmentioning
confidence: 83%
“…In Figures , , and 5, smoothed values at equimolar fraction for H E or V E are plotted versus the C-atom number of the linear compound of the mixture. The collected data come from this work and from an extensive review of the literature. ,,− These plots allow us to visualize the trend of excess property changes when increasing the alkane or alkanol chain length and assist in a few cases in the comparison between our values and those previously reported by others.…”
Densities, F, and volumetric heat capacities, C p /V, have been measured at 298.15 K over the whole mole fraction range for the binary mixtures {tetrahydrofuran + methanol, + ethanol, + 1-propanol, + 1-butanol, + 1-hexanol, + 1-heptanol, + 1-octanol, + 1-nonanol, or + 1-decanol}. From experimental data, the excess molar isobaric heat capacities, C p E , were calculated. Excess molar volumes, V E , are reported for the systems containing methanol and 1-decanol. The apolar homomorph concept has been used in semiquantitative calculations intended to assess and to compare the degrees of heteroassociation in these mixtures by getting an approximation to the corresponding negative enthalpic contributions at equimolar fraction, H int . With this aim, excess molar enthalpies, H E , of {tetrahydrofuran + nonane} and {cyclopentane + 1-butanol, + 1-pentanol, + 1-hexanol, + 1-heptanol, + 1-octanol, + 1-nonanol, or + 1-decanol} have been measured at 298.15 K. The results are discussed in terms of molecular interactions. Particularly, the various steps of W-shape concentration dependence found in the C p E point to the occurrence of local nonrandomness in {THF + alkanol} mixtures.
“…Thermodynamic properties of alkylamines and THF have been studied earlier [4][5][6] and for other system studied we found no data in the literature. Here, experimental densities, viscosities, refractive indices, and derived properties of the ternary mixture of {2-methyl-2-butanol (1) + THF (2) + propylamine (3)} at a temperature of 298.15 K and the binary mixtures at temperatures of (288.…”
Literature values of the Ostwald solubility coefficient of gases and vapours in propan-1-ol at 298 K were combined with additional values calculated from solubilities in propan-1-ol and vapour pressures to yield a total of 79 log L PrOH values at 298 K. Seventy-seven of these values were correlated through the general solvation equation to give the regressionA correlation equation was also constructed for the transfer of solutes from water to propan-1-ol. Both equations suggest that propan-1-ol as a solvent is less dipolar, more acidic and less basic than methanol or ethanol, but the differences between the three alcohols are very small. Comparison with equations for transfer to wet alcohols shows that the addition of water to alcohols has little effect on their dipolarity/polarizability or hydrogen bond basicity, but considerably increases the hydrogen bond acidity. The wet alcohols are more hydrophilic (less hydrophobic) than the dry alcohols.
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