Isobaric Vapor–Liquid Equilibrium of Binary Systems (Isopropyl Acetate/Isopropyl Alcohol + Dibutyl Ether/ Anisole) at 101.3 kPa

As there is an azeotropic point between methanol and ethyl formate, they cannot be completely separated by ordinary distillation. In this paper, extractive distillation was applied and dimethyl sulfoxide (DMSO) and ethylene glycol (EG) were used as entrainers. Vapor−liquid equilibrium (VLE) data for methanol−ethyl formate, methanol−ethyl formate−DMSO, and methanol− ethyl formate−EG were measured at 101.3 kPa, and the NRTL model was applied for data fitting. It was found that the experimental value and the calculated value were accordant well through the deviation value. Then, the NRTL model was used for simulation by Aspen Plus to achieve the separation goal, and it verified the feasibility of the experimental scheme.

Section: Introductionmentioning

confidence: 99%

Vapor–Liquid Equilibrium Experiment and Process Simulation for Methanol and Ethyl Formate at 101.3 kPa

Han

Wang

et al. 2021

“…Because the experiment was carried out in a low pressure, the presence of ILs in the gas phase could be ignored. When the system reached equilibrium, the gas phase could be considered an ideal gas. − The formulas for γ i and α 12 are shown below. …”

Section: Resultsmentioning

confidence: 99%

Vapor–Liquid Equilibrium Experiment for Butanone and Ethyl Acetate at 101.3 kPa

Wang

Jin

et al. 2021

The formation of azeotrope brings severe challenges to the separation of butanone and ethyl acetate, two important chemical raw materials. In this article, two ionic liquids, 1-hexyl-3-methylimidazolium bis[(trifluoromethyland ethylene glycol (EG) were selected as entrainers to separate butanone and ethyl acetate. Vapor−liquid equilibrium data of butanone−ethyl acetate−[EMIM]-[NTf 2 ], butanone−ethyl acetate−[HMIM][NTf 2 ], and butanone−ethyl acetate−EG were measured at atmospheric pressure. The results show that the three extractants can effectively break the azeotrope of butanone−ethyl acetate, and the significant salt effect makes [EMIM][NTf 2 ] and [HMIM][NTf 2 ] show better separation ability than EG.Then, a non-random two liquid (NRTL) thermodynamic model was further used to fit the experimental data, and the average relative deviation was only 0.033, indicating that the NRTL model can well describe the influence of these three entrainers on the phase equilibrium behavior of butanone−ethyl acetate.

“…At 101.3 kPa, the experimental LLE data were obtained at 303.2, 313.2, and 323.2 K. The information of apparatus and means has been provided in previous papers. − First, the solvent (TCM or MIPK) and water, each weighing about 40 g, were loaded into a jacketed glass container and mixed for 4 h and then stabilized for at least 6 h. Next, FAL was added to the kettle several times (1–2 g each time) to determine different phase equilibrium points. A thermocouple thermometer was used to measure the temperature of each test system, with an accuracy of 0.1 K.…”

Section: Methodsmentioning

confidence: 99%

Liquid–Liquid Equilibrium Study of Ternary Systems of (Water + Furfuryl Alcohol + Solvents) at 303.2, 313.2, and 323.2 K

Yan

Han

et al. 2021

The liquid–liquid equilibrium (LLE) data of water + furfuryl alcohol + trichloromethane /methyl isopropyl ketone were determined at 303.2, 313.2, and 323.2 K under 101.3 kPa. The distribution coefficient (D) and separation factor (S) were evaluated for the separation effect of solvents. The nonrandom two-liquid and universal quasichemical models were used to correlate the experimental LLE data and obtain the binary interaction parameters. Meanwhile, the root mean square deviations and absolute average deviation of the two models did not exceed 0.0094 and 0.0066, respectively, which shows that the experimental LLE data can be accurately correlated through the two models. GUI-MATLAB was used to verify the consistency between the LLE data and the calculated binary interaction parameters. σ-Profiles were used to analyze the interaction between the molecules of each substance, further confirming the accuracy of the experimental results.