Isothermal Vapor–Liquid Equilibrium Measurements for the Pentan-2-one + Propan-1-ol/Butan-1-ol System within 342–363 K

Mavalal, Shivan; Chetty, Thavashni; Moodley, Kuveneshan

doi:10.1021/acs.jced.9b00100

Cited by 9 publications

(8 citation statements)

References 31 publications

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“…On the other hand, prop-2-en-1-ol–hexan-2-ol and prop-2-en-1-ol–4-methyl-pentan-2-ol showed a similar point of inflection at x 1 ≈ 0.2 with asymmetric activity coefficient plots, indicating that one of the components had a very low deviation from ideal behavior, supposedly the long-chain secondary alcohol. This asymmetric behavior was also evidenced for pentan-2-one/propanol, water/2-methylpyridine, and water/butane-2,3-diol systems. − …”

Section: Resultsmentioning

confidence: 60%

Isobaric Vapor–Liquid Equilibrium Data for Six Binary Systems: Prop-2-en-1-ol (1)–Hexan-2-ol (2), Prop-2-en-1-ol (1)–Hexan-2-one (2), Hexan-2-one (1)–Hexan-2-ol (2), Prop-2-en-1-ol (1)–4-Methyl-pentan-2-ol (2), Prop-2-en-1-ol (1)–4-Methyl-pentan-2-one (2), and 4-Methyl-pentan-2-one (1)–4-Methyl-pentan-2-ol (2) at 101.32 kPa

Vargas¹,

Katryniok²,

Araque³

2021

J. Chem. Eng. Data

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In this work, isobaric vapor−liquid equilibrium (VLE) measurements were conducted for the binary systems of prop-2-en-1-ol (1)−hexan-2-ol (2), prop-2-en-1-ol (1)−hexan-2-one (2), hexan-2-one (1)−hexan-2-ol (2), prop-2-en-1-ol (1)−4-methyl-pentan-2-ol (2), prop-2-en-1-ol (1)−4-methyl-pentan-2one (2), and 4-methyl-pentan-2-one (1)−4-methyl-pentan-2-ol (2) to assist with the design of the separation process by distillation. Measurements were determined using Fischer VLE 602 equipment at 101.32 kPa. The thermodynamic consistency of the measured VLE data was validated by modified Herington, Van Ness, pure component consistency, and Redlich−Kister total area tests. Moreover, data sets were correlated using the nonrandom two-liquid (NRTL), universal quasichemical (UNIQUAC), and Wilson thermodynamic models to obtain the binary interaction parameters using the Aspen Plus V11 commercial software. The root-mean-square deviations (RMSDs) of the equilibrium temperature (T) and the vapor mole fraction (y i ) were less than 0.24 and 0.0089, respectively, which indicate that these three thermodynamic models can be used to correlate the six binary systems and therefore they can be employed for the development and optimization of the separation process.

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Section: Resultsmentioning

confidence: 60%

Isobaric Vapor–Liquid Equilibrium Data for Six Binary Systems: Prop-2-en-1-ol (1)–Hexan-2-ol (2), Prop-2-en-1-ol (1)–Hexan-2-one (2), Hexan-2-one (1)–Hexan-2-ol (2), Prop-2-en-1-ol (1)–4-Methyl-pentan-2-ol (2), Prop-2-en-1-ol (1)–4-Methyl-pentan-2-one (2), and 4-Methyl-pentan-2-one (1)–4-Methyl-pentan-2-ol (2) at 101.32 kPa

Vargas¹,

Katryniok²,

Araque³

2021

J. Chem. Eng. Data

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“…The equilibrium still described by Joseph et al was used for the measurements and a schematic is shown in Figure . The apparatus and operating procedure have been described in detail in previous reported work. − The pressure in the still was measured using a WIKA P-10 transducer (0 to 101.3 kPa) calibrated against a WIKA CPH 6000. The reported uncertainty by the manufacturer on the P-10 transducer is 0.05% of full-scale.…”

Section: Methodsmentioning

confidence: 99%

“…Schematic of the apparatus of Joseph et al used in this work (as shown in ref ). 1, Equilibrium chamber; 2, Liquid sampling port; 3, Temperature measurement; 4, Boiling chamber; 5, Variable heat supply to boiler; 6, Heater cartridge and sleeve; 7, Magnetic stirrer and bead; 8, Boiler drain valve; 9, Condensate drain valve; 10, Vapor condensate sampling point; 11, Condenser; 12, Coolant line to condenser; 13, Coolant bath and controller; 14, Chiller; 15, Pressure measurement; 16, Isolation valves; 17, Ballast tank; 18, Cold trap; 19, Vacuum pump.…”

Section: Methodsmentioning

confidence: 99%

Isobaric Vapor–Liquid Equilibrium Data for Water (1) + 2-Methyl-propan-1-ol (2), 2-Methyl-propan-1-ol (1) + Pyridine (2), and Water (1) + 2-Methyl-propan-1-ol (2) + Pyridine (3) Systems

et al. 2020

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In this work, isobaric vapor–liquid equilibrium (VLE) measurements were conducted for the binary systems of water (1) + 2-methyl-propan-1-ol (2) and 2-methyl-propan-1-ol (1) + pyridine (2) at approximately 50, 80, and 100 kPa using a dynamic equilibrium apparatus. The water (1) + 2-methyl-propan-1-ol (2) system was found to be partially miscible for some intermediate compositions and exhibited azeotropic behavior, while a maximum boiling azeotrope was observed for the 2-methyl-propan-1-ol (1) + pyridine (2) system at 51 kPa and approximately x 1 = 0.23. Ternary VLE measurements were also conducted for the water (1) + 2-methyl-propan-1-ol (2) + pyridine (3) system at 101.3 kPa. The binary VLE data were modeled using the γ–Φ approach with the Nonrandom Two-Liquid and Universal Quasi-Chemical activity coefficient models and the virial equation of state. The measured data were found to be thermodynamically consistent using the point-type and infinite dilution tests. Ternary VLE data were predicted from the regressed binary interaction parameters and show satisfactory comparison to the experimentally determined VLE data.

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“…Schematic of the apparatus of Joseph et al used in this work, as shown in Mavalal et al (1) Equilibrium chamber. (2) Liquid sampling port.…”

Section: Methodsmentioning

confidence: 99%

Isothermal Vapor–Liquid Equilibrium (P–x–y) Measurements and Modeling of n-Hexane + Pentan-2-one/4-Methylpentan-2-one

2020

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Isothermal vapor−liquid equilibrium (VLE) data were measured for the hexane + pentan-2-one/4-methylpentan-2-one systems to characterize the separation limits. Phase equilibrium measurements were undertaken at approximately 313, 323, and 334 K at subatmospheric pressures using a dynamic apparatus. The γ−Φ regression approach was used with the nonrandom twoliquid or UNIQUAC activity coefficient models employed to account for the nonideality of the liquid phase, with the Hayden and O'Connell correlation in the virial equation of state, used to account for the vapor phase nonideality. Additionally, the data were modeled by the φ−φ approach with the Peng− Robinson and perturbed-chain statistical associating fluid theory equations of state, which exhibited an inferior performance in comparison to the modeling by the γ−Φ approach. The area and point thermodynamic consistency tests were applied to the data and showed that the measured data were thermodynamically consistent. Excess enthalpy predictions were found to correlate well with the available literature.

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Isothermal Vapor–Liquid Equilibrium Measurements for the Pentan-2-one + Propan-1-ol/Butan-1-ol System within 342–363 K

Cited by 9 publications

References 31 publications

Isobaric Vapor–Liquid Equilibrium Data for Water (1) + 2-Methyl-propan-1-ol (2), 2-Methyl-propan-1-ol (1) + Pyridine (2), and Water (1) + 2-Methyl-propan-1-ol (2) + Pyridine (3) Systems

Isothermal Vapor–Liquid Equilibrium (P–x–y) Measurements and Modeling of n-Hexane + Pentan-2-one/4-Methylpentan-2-one

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