Phasengleichgewichtsmessungen. IV. Die Phasengleichgewichte dampfförmig/flüssig des Systems Phenol/n‐Butylacetat/Wasser bei 44,4°C

Weller, Rolf; Schuberth, H.; Leibnitz, E.

doi:10.1002/prac.19630210502

Cited by 15 publications

(5 citation statements)

References 11 publications

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“…The operating conditions of the chromatograph were as follows: injection and (5, 6) give the Antoine vapor pressure equations for phenol and activity coefficients of phenol at infinite dilution, based on the experimental data (3,4). Each 300-mL flask had about 250 mL of phenol The aqueous phenol solutions were prepared by dissolving the proper amount of reagent grade phenol (Kanto Chemicals Co., Tokyo) with a stated purity of 99+ % in a known amount of deionized water.…”

Section: Methodsmentioning

confidence: 99%

“…The Hen&'s constants estimated from the literature data (3,4), selected by (jmehling et al (5,6), are ako included in Table I. The data of Schreinemakers (3) and Welier et al (4) are those obtained from the distillation measurements in phenolwater system at low pressures, whereas our data are from the measurements of phenol concentration in a phenol-water-air system at atmospherlc pressure.…”

Section: Methodsmentioning

confidence: 99%

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Henry's constants for phenol over its diluted aqueous solution

Abdel-Bary¹,

Hamoda²,

Tanisho³

et al. 1986

J. Chem. Eng. Data

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229for silver sulfate and silver acetate (Table VI) is positive and passes through a maximum at X,,, = 0.45 with LX = 5.8 and 5.1, respectively. Thus an increase of 3.0 and 3.7 moles of AN occurs in the case of dioxane + AN mixtures for silver sulfate and silver acetate and an increase of 5.8 and 5.1 moles of Me,SO occurs in the case of dioxane + Me,SO for silver sulfate and silver acetate, respectively, per faraday, relative to the mean molar velocity of the solvent mixtures as reference (23) in the cathode compartment when the solutions of these salts are electrolyzed at the given composition of the solvent mixtures. The enrichment of AN or Me,SO in the cathode compartment arises largely through their transport by the silver ion while the anion transports dioxane in the opposite directlon, i.e., toward the anode. These two effects add together and thus a heteroselective solvation results in large A values. These results support the conclusions based on the transfer energy variation of the ions observed earlier.Henry's constants for phenol over its aqueous solutlon were measured In the temperature range from -2 to 27 OC. An equation was proposed to correlate these data and those estimated from the lllerature data at 44-90 OC.

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Section: Methodsmentioning

confidence: 99%

Section: Methodsmentioning

confidence: 99%

Henry's constants for phenol over its diluted aqueous solution

Abdel-Bary¹,

Hamoda²,

Tanisho³

et al. 1986

J. Chem. Eng. Data

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“…Nagata reported the VLE data for the butyl acetate + cyclohexane binary system at 101.325 kPa. Water + butyl acetate VLE data were presented by Schuberth at 13.33 kPa and by Weller et al at 317.55 K, respectively. Cho et al published VLE data for the water + butyl acetate binary system at 101.325 kPa.…”

Section: Introductionmentioning

confidence: 99%

Determination and Prediction of Vapor–Liquid Equilibria for a System Containing Water + Butyl Acetate + Cyclohexane + Ethanol

2012

J. Chem. Eng. Data

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The separation of butyl acetate from aqueous solution by distillation is energyconsuming. However, azeotropic distillation may be a commercially economical way when cyclohexane is added as an entrainer. The vapor−liquid equilibria (VLE) data were measured by the quasi-static ebulliometric method for the following systems at (29.77, 58.85, and 87.65) kPa:(1) butyl acetate + cyclohexane; (2) water + butyl acetate + ethanol; (3) water + butyl acetate + cyclohexane; (4) water + ethanol + butyl acetate + cyclohexane. The VLE data for binary and ternary systems were used to regress the nonrandom two-liquid (NRTL) interaction parameters, namely, pairs of butyl acetate−cyclohexane and water−butyl acetate, with aid of Aspen Plus platform. The newly regressed parameters were verified by the comparison between predicted VLE values and experimental data for ternary and quaternary systems without parametrization. The average relative deviations are only 0.19 % and 0.17 %, respectively. Furthermore, the NRTL thermodynamic model with new parameters was applied to construct the distillation residue curve map for the water + butyl acetate + cyclohexane ternary system, which provides the VLE information for the production of the butyl acetate by new azeotropic distillation.

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“…This is probably a poor assumption for phenolic solutes, but it used to obtain reasonable estimates. (Markuzin, 1961;Schulek et al, 1964;Bogart et al, 1948;Weller et al, 1963;and Shreinemakers, 1900).…”

Section: Hiqh Performance Liquid Chromatoqraphymentioning

confidence: 99%

Irreversible adsorption of phenolic compounds by activated carbons

Grant¹,

King²

1988

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Phasengleichgewichtsmessungen. IV. Die Phasengleichgewichte dampfförmig/flüssig des Systems Phenol/n‐Butylacetat/Wasser bei 44,4°C

Cited by 15 publications

References 11 publications

Henry's constants for phenol over its diluted aqueous solution

Henry's constants for phenol over its diluted aqueous solution

Determination and Prediction of Vapor–Liquid Equilibria for a System Containing Water + Butyl Acetate + Cyclohexane + Ethanol

Irreversible adsorption of phenolic compounds by activated carbons

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