Measurement of the vapor pressure of methanol- n -decanol and ethanol- n -decanol mixtures

Self Cite

Section: Introductionmentioning

confidence: 74%

“…1. Measurements of vapor pressures were made for 12 different (total) compositions and at 6 temperatures (20.0, 25.0, 30.0, 35.0, 40.0, and 50.0 "C) for each mixture.…”

Section: Methodsmentioning

confidence: 99%

Vapor–liquid equilibrium studies of n-propanol–n-decanol mixtures

Singh¹,

Benson²

1968

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“…Equilibrium vapor pressures of n~ixtures of known total composition were determined by the static method in a cell similar to that used by Singh and Benson (13). The pressure at 25.000 _+ 0.001 "C was measured to kO.OO5Torr with a quartz spiral gauge which was calibrated by comparison with a mercury manometer.…”

Section: Appararrrs Arid Teclirii~lrresmentioning

confidence: 99%

Thermodynamic Properties of Cyclopentanol + p-Dioxane Mixtures at 25 °C

Anand¹,

Grolier²,

Kiyohara³

et al. 1973

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Excess enthalpies, excess volumes, and total vapor pressures were measured for cyclopentanol + pdioxane mixtures at 25 "C. The method of Barker was used to calculate vapor-liquid equilibria and excess Gibbs free energies from the vapor pressure results. apparaitre que les proprietes thermodynamiques d'exces des melanges cyclopentanol + p-dioxane resultent principalement de la rupture de la structure du solvant p-dioxane, dans ces melanges.

“…The molar X of mixing, AXm is related to the standard X of complex formation AXe by [9] (NA + NB)AXm = nA Xe + AX* Use of the ideal associated solution model allows representation of AX* by the appropriate ideal solution expression.…”

Section: Discussionmentioning

confidence: 99%

“…lar to one used previously (9). A quartz spiral mounted in a pressure gauge (Texas Instruments Model 145) was used as the pressure sensor.…”

Section: Introductionmentioning

confidence: 99%

Vapor Pressures of Triethylamine + Chloroform and of Diethyl Ether + Chloroform at 298.15 K

Handa¹,

Jones²

1975

Can. J. Chem. 53,3299 (1975).Vapor pressures of triethylamine + chloroform and of diethyl ether + chloroform were measured at 298.15 K with a calibrated quartz spiral. The ideal associated solution model has been used to determine the equilibrium constants and standard enthalpies of formation of the complexes from the thermodynamic properties derived from the vapor pressure measurements and from earlier calorimetric measurements. These complex formation constants are compared with values obtained by calorimetric and spectroscopic methods.