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

Abstract

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.

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

“…The VLE expression is thus simplified as shown in eq . Experimental VLE data with the corresponding experimental activity coefficients are listed in Tables – . To evaluate the ideality deviations of the systems under the same composition and pressure conditions, excess Gibbs energy ( G E ) was determined by eq , where R is the universal gas constant and T is the system temperature. For all binary systems, positive deviations are evidenced, considering that γ 1 and G E values are above 1 and 0, respectively (Tables –). …”

“…Hence, to develop separation and purification strategies for allyl alcohol from the DODH of glycerol, high-precision experimental phase equilibrium data are required. 7,8 The vapor−liquid equilibrium of prop-2-en-1-ol (1)−water (2) has already been reported in the literature, 9 and vapor− liquid−liquid equilibriums of solvent/water and ketone/water binary systems are given in the Aspen Plus V11 database. Thus, this work focuses on the experimental measurement of VLE data for the binary mixtures 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-2en-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 to calculate the adjustable binary interaction parameters from localcomposition models.…”

“…Considering the application of allyl alcohol as a monomer in the chemical industry, it is imperative to isolate it in high purity from the reaction mixture containing the solvent, the co-produced ketone, and water. Hence, to develop separation and purification strategies for allyl alcohol from the DODH of glycerol, high-precision experimental phase equilibrium data are required. , …”