Ternary (liquid–liquid) equilibrium data of furfuryl alcohol with organic solvents at T=298.2K: Experimental results and thermodynamic models (original) (raw)
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Journal of Chemical & Engineering Data, 2003
Liquid-liquid equilibrium results for mixtures of furfural + an aromatic hydrocarbon + an alkane at T) 298.15 K are reported, where an aromatic hydrocarbon is benzene or methylbenzene or 1,2dimethylbenzene or 1,3-dimethylbenzene or 1,4-dimethylbenzene and an alkane refers to n-hexane or n-dodecane or n-hexadecane. The data were measured using the titration method and show a large solubility gap for all mixtures studied. The selectivity values are large, indicating that furfural is capable of separating aromatic hydrocarbons from aliphatic hydrocarbons by solvent extraction. The data were correlated with the UNIQUAC equation, the NRTL equation, and three analytical equations.
Studia Universitatis Babeș-Bolyai Chemia, 2019
In this work, excess properties (e.g. excess molar volume (V E), excess viscosity (Ƞ E), excess Gibbs free energy of activation of viscos flow (∆G* E) and molar refraction changes (∆nD) of binary solvent mixtures of tetrahydrofurfuryl alcohol (THFA) with aromatic hydrocarbons (benzene, toluene and p-xylene) have been calculated. This was achieved by determining the physical properties including density ρ, viscosity Ƞ and refraction index nD of liquid mixtures at 298.15K. Results of the excess parameters and deviation functions for the binary solvent mixtures at 298.15 K have been discussed by molecular interactions that occur in these mixtures. Generally, parameters showed negative values and have been found to fit well to Redlich-Kister equation which has been used to obtain the coefficients and evaluate the standard error.
Rasayan Journal of Chemistry
To understand the nature of molecular aggregation between two solvents, excess properties (e.g. excess molar volume (V), excess Gibb's free energy of activation viscous flow (∆G* E) and viscosity deviation of binary mixtures) are therefore needed. Thus, in the current study, the refractive index (nD), viscosity (η), and density (ρ) of binary mixtures were measured for tetrahydrofurfuryl alcohol (THFA) with ethanol, 2-propanol and 2-butanol at 298.15K. Moreover and based on experimentally obtained results, the V , the refractive index deviation (∆nD), excess molar viscosity (η E) and ∆G* E were calculated. To correct and fit the experimental V , η E and ∆nD deviations, Redlich-Kister equation was used. The molecular interaction in binary mixtures was found to explain the variability of physical properties with the composition of the mixtures. In light of obtained results, factors influencing the molecular interactions (e.g. the length of the carbon chain and the position of hydroxyl groups in targeted alcohol) have been also discussed. In all cases the obtained V , η E , ∆G* E and ∆nD values were negative at 298.15K except for the binary system (THFA + 2butanol) where the results indicate the positive deviation in refractive indices.
Effects of salt on the LLE and tie-line data for furfuryl alcohol — n-butanol–water at T=298.15K
Journal of Molecular Liquids, 2016
Solubility and tie-line data for the systems containing water + furfuryl alcohol + n-butanol + NaCl were measured at T = 298.15 K and atmospheric pressure. The NRTL and UNIQUAC models were employed to compare the experimental liquid-liquid equilibrium (LLE) data. The binary interaction parameters were determined. The Othmer-Tobias, Hand and Bachman correlation equations were applied to validate the LLE data for these systems. Distribution coefficients and separation factors were calculated. It was noted that enlargement of the two-phase region occurred when the concentration of salt increased in the initial aqueous phase. Adding salt to the system proved beneficial in separating furfuryl alcohol from water.
The (vapor + liquid) equilibria of the pure components, furfuryl alcohol, and methyl isobutyl ketone along with the binary mixtures (2,5-dimethylfuran + furfuryl alcohol), or (2,5-dimethylfuran + methyl isobutyl ketone), were investigated experimentally by means of a static apparatus at temperatures between (313 and 393) K. The vapor pressures of the pure components were correlated with the Antoine equation. The experimental results for the mixtures were reduced by the Barker method using a third-order Redlich-Kister equation. The calculated values of the excess Gibbs free energy, G E , exhibit positive deviations for all investigated temperatures and over the whole composition range. The NRTL, UNIQUAC and Modified UNIFAC (Do) models have been applied to correlate the experimental VLE results.
Asian Journal of Chemistry, 2019
At the temperature 298.15 K, some physical properties such as: refractive indices (ni>), viscosities (q) and densities (p) were studied in four liquid-liquid mixtures: carboxylic acids (HCOOH, CH 3 COOH, CH 3 CH 2 COOH and CH 3 CH 2 CH 2 COOH) with tetrahydrofurfuryl alcohol (THFA) with the identified configuration set. These empirical data were utilized to estimate the excess molar volumes (VmE), refractive index perversions (AR), viscosity deviations (qE) and excess molar Gibbs free energy (AG *E). Values of Vj , q 1 , AG *1 and AR were plotted versus mole fraction of tetrahydrofurfuryl alcohol. In all cases, the values of VmK, q 1 , AG * 1 and AR that obtained in this study were found to be negative at 298.15 K. The excess parameters were applied in the Redlich-Kister equation by utilizing multi-parameter coefficients that concluded binary coefficients and in respect to the standard deviation. The difference of these characteristics with the formation of binary liquid systems indicates the absence of bipolar bond, variation in the shape and size of component molecules, hydrogen bonding and dipolar interaction among unlike molecules.
Thermo, 2021
Tetrahydrofuran (THF) is an aprotic solvent with multiple applications in diverse areas of chemical, petrochemical, and pharmaceutical industries with an important impact in chemical waste liquid with other solvents. In this work, 51 available VLE data, for isothermal binary mixtures of THF(1) + Benzene(2) and THF(1) + Cyclohexane(2) at 303.15 and 333.15 K, respectively, and isobaric THF(1) + Methanol(2) at 103 kPa and THF(1) + Ethanol(2) at 100 kPa were used in the development of the activity coefficient models. The quality of experimental data was checked using the Herington test. VLE binary data was correlated with models Wilson, NRTL UNIQUAC, and UNIFAC to obtain binary parameters and activity coefficients. The best thermodynamic consistency when conducting the Herington test for the VLE data was found for the THF(1) +Cyclohexane(2) isothermal system and THF(1) + Ethanol(2) isobaric system. The UNIQUAC model for isothermal systems THF(1) + Benzene(2) and THF(1) + Cyclohexane(2),...
Industrial & Engineering Chemistry Research, 2009
The use of 2,2,4-tri methyl pentane as a cosolvent for extraction of aromatic hydrocarbons from lube cut is studied. Optimized values of extraction temperature and amount of 2,2,4-tri methyl pentane are determined. The liquid-liquid equilibrium between {lube oil + furfural + cosolvent} is examined with the NRTL equation. The binary interaction parameters for the NRTL model are obtained by minimization of an objective function. General binary interaction parameters are computed and reported for estimating the liquid-liquid equilibrium products between 323.15 and 343.15 K. Also, a generalized model is presented for calculation of the refractive index and specific gravity of lube-oil fractions. The calculated results are in good agreement with the results of the experiments.
Vapor-liquid equilibriums. Systems p-xylene-furfural and ethylbenzene-furfural
Journal of Chemical & Engineering Data, 1970
Vapor-liquid equilibrium data are reported for the binary systems ethylbenzenefurfural and p-xylene-furfural at 723 mm of Hg pressure. Both the systems formed minimum boiling azeotropes. The activity coefficients were calculated, taking into consideration the vapor phase nonideality, tested for thermodynamic consistency, and correlated by Wilson's equation.