The Vapor Pressure of Certain Ketones

Mayberry, M. Glenn; Aston, J. G.

doi:10.1021/ja01327a044

Cited by 14 publications

(3 citation statements)

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“…The vapor pressure values, Pl , were taken from our own data (7) in the cases of diethyl, dipropyl, and dibutyl ketones. Values for the two methyl propyl and the two methyl butyl ketones were calculated from, the equations given by Mayberry and Aston (6).…”

Section: Resultsmentioning

confidence: 99%

Energy and Volume Relations in the Solubilities of Some Ketones in Water.

Gross¹,

Rintelen²,

Saylor³

1939

J. Phys. Chem.

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A study has been made in this laboratory of the solubility in water of several series of slightly soluble organic compounds. Such systems are sufficiently dilute so that but little interaction is to be anticipated between the solute molecules themselves. They thus afford an opportunity to study the interactions between the solvent water molecules and the organic molecules as reflected in the solubility values and their change with temperature, and in the energy values associated with the solution process.The solubilities of several simple series of compounds, including aromatic hydrocarbons and halogenated aliphatic and aromatic hydrocarbons, have been measured, as well as of the series of aliphatic ketones for which data are given here. The ketones, while showing more complicated relationships, are presented here, since in the results for them certain interesting features are evident that are present in only a limited degree in the other cases.The experimentally determined solubility values are the concentrations in the water phase in equilibrium with the liquid solute phase, saturated with water. Inspection of these values shows but little correlation to exist among them in any of the series of compounds. However, when those energy terms involved in separating the solute molecules from their liquid phase are eliminated, regularities become evident at once. This may be done by recomputing the observed solubilities to vapor solubilities corresponding to a constant standard state of 100 mm. in the vapor. To compute these standard vapor solubilities from the observed solubility values and the vapor pressures of the organic liquids, Henry's law is employed. Except in a few cases (3) this law has not been commonly applied to such systems. While there seems little reason to doubt its validity in the case of dilute solutions, it was deemed better to determine

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Section: Resultsmentioning

confidence: 99%

Energy and Volume Relations in the Solubilities of Some Ketones in Water.

Gross¹,

Rintelen²,

Saylor³

1939

J. Phys. Chem.

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“…Products were identified by comparison of their retention time with those of authentic samples and by GC-MS analysis (HI) 5890 GC with a 50 m HP-1 capillary column + HP 5970 MSD). The values of hourly liquid space velocity (denoted HLSV) were calculated from data published in the literature [21,22] and also measured. The results were in good agreement.…”

Section: Methodsmentioning

confidence: 99%

Catalytic transfer hydrogenation of 2-butanone over oxide catalysts

Szőllősi

Bartók

1999

React Kinet Catal Lett

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Catalytic transfer hydrogenation of 2-butanone with 2-propanol was studied in gas phase over a series of oxides of different acid-base properties. Although the basic oxides (MgO, La203) gave high initial conversions, these oxides underwent deactivation during the reaction. This deactivation could be partially prevented by a previous treatment with chloroform of the oxide. The amphoteric oxides (TiO2, ZrO2, Al203) were also active in this reaction. Increasing the acidic character of the catalyst (Nb2Os, WO3) led to a pronounced dehydration of 2-propanol. The results obtained over a series of rare earth oxides (La203, Sm203, Gd203, Dy203, Er203) revealed that beside the role of basic and acid sites a correlation seems to exist between the number of unpaired electrons of the metal ion and the catalytic activity, indicating the role of one electron donor sites.

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“…When normal boiling point values appeared in Ambrose [41765], they were chosen as the tentative selected values and used as a guideline in the vapor pressure data fitting, hence our values are biased toward the Ambrose values Aston [13799] over the range 350 to 440 K, and on points from Dreisbach and Shrader [1361] tions were based on the vapor pressure data of Geisler and Ratzsch [18439] and the boiling point values reported by Deffet [5736] (446.681 K) , Bruhl [5842] (100.352 kPa at 446.080 K), Ceuterick [9712] (100.658 kPa at 446.180 K)…”

Section: Inorganic Chemistry Division Commission On Atomic Weights Imentioning

confidence: 99%

Definition of recommended values of certain thermodynamic properties for the ketones

Smith¹

1984

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Liquid density correlation equations used.Correlation test results for second virial coefficient data. Compound identification numbers.Relation between carbon number and the assigned compound identification number. Compound constant values. Comparison of selected normal boiling points with those of other compilations Range 1 vapor pressure correlations. Range 2 vapor pressure correlations. Range 3 vapor pressure correlations. Range 4 vapor pressure correlations. Definition of quality rating symbols for the property correlations. Range 1 liquid density correlations. Range 2 liquid density correlations. Range 3 liquid density correlations. Range 4 liquid density correlations. Parameters used in the Tsonopoulos equation.Literature references for individual property correlations.Citations for literature documents.

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The Vapor Pressure of Certain Ketones

Cited by 14 publications

References 0 publications

Energy and Volume Relations in the Solubilities of Some Ketones in Water.

Energy and Volume Relations in the Solubilities of Some Ketones in Water.

Catalytic transfer hydrogenation of 2-butanone over oxide catalysts

Definition of recommended values of certain thermodynamic properties for the ketones

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