Isobaric vapour-liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101.31 kPa
New experimental vapour-liquid equilibrium (VLE) data, which is expected to be useful in industrial processes such as the design of separation processes is reported in the present article. Isobaric VLE data of an eco-sustainable, green solvent furfuryl alcohol (FFA) as a common component has been me...
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Elsevier
2025-03-01
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| Series: | Chemical Thermodynamics and Thermal Analysis |
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| Online Access: | http://www.sciencedirect.com/science/article/pii/S2667312624000269 |
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| author | K.A. Sasikala K. Rayapa Reddy P.V.S. Sairam G. Srinivasa Rao |
| author_facet | K.A. Sasikala K. Rayapa Reddy P.V.S. Sairam G. Srinivasa Rao |
| author_sort | K.A. Sasikala |
| collection | DOAJ |
| description | New experimental vapour-liquid equilibrium (VLE) data, which is expected to be useful in industrial processes such as the design of separation processes is reported in the present article. Isobaric VLE data of an eco-sustainable, green solvent furfuryl alcohol (FFA) as a common component has been measured for three binary systems (i) furfuryl alcohol + aniline (AN), (ii) furfuryl alcohol + N-methylaniline (NMA) and (iii) furfuryl alcohol + N-ethylaniline (NEA) in the complete concentration of FFA at a pressure of 101.31 kPa. The Antoine equation has been used to calculate the vapour pressure of pure samples. The reported VLE data is thermodynamically consistent according to the van Ness, Fredenslund and Herington area tests. The experimental observations of the three systems displayed non-ideal nature and negative deviation from Raoult's law. The Wilson and UNIQUAC activity coefficient models have been applied to correlate the experimental data. The information of the boiling point temperature (T), activity coefficients (γi) and variation of excess Gibbs energy (GE) with the concentration of FFA indicated the presence of dipole-dipole interactions and hydrogen bonding between the molecules of FFA and the selected amines. |
| format | Article |
| id | doaj-art-79bc682808a9449b83890fde00866194 |
| institution | Kabale University |
| issn | 2667-3126 |
| language | English |
| publishDate | 2025-03-01 |
| publisher | Elsevier |
| record_format | Article |
| series | Chemical Thermodynamics and Thermal Analysis |
| spelling | doaj-art-79bc682808a9449b83890fde008661942025-02-10T04:35:26ZengElsevierChemical Thermodynamics and Thermal Analysis2667-31262025-03-0117100153Isobaric vapour-liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101.31 kPaK.A. Sasikala0K. Rayapa Reddy1P.V.S. Sairam2G. Srinivasa Rao3Department of Physics, Acharya Nagarjuna University, A.P, India; Department of Physics, Dhanekula Institute of Engineering & Technology, A.P, IndiaDepartment of Chemistry, Andhra Loyola College, Vijayawada, A.P, IndiaDepartment of Physics, Andhra Loyola College, Vijayawada, A.P, IndiaDepartment of Physics, Andhra Loyola College, Vijayawada, A.P, India; Corresponding author.New experimental vapour-liquid equilibrium (VLE) data, which is expected to be useful in industrial processes such as the design of separation processes is reported in the present article. Isobaric VLE data of an eco-sustainable, green solvent furfuryl alcohol (FFA) as a common component has been measured for three binary systems (i) furfuryl alcohol + aniline (AN), (ii) furfuryl alcohol + N-methylaniline (NMA) and (iii) furfuryl alcohol + N-ethylaniline (NEA) in the complete concentration of FFA at a pressure of 101.31 kPa. The Antoine equation has been used to calculate the vapour pressure of pure samples. The reported VLE data is thermodynamically consistent according to the van Ness, Fredenslund and Herington area tests. The experimental observations of the three systems displayed non-ideal nature and negative deviation from Raoult's law. The Wilson and UNIQUAC activity coefficient models have been applied to correlate the experimental data. The information of the boiling point temperature (T), activity coefficients (γi) and variation of excess Gibbs energy (GE) with the concentration of FFA indicated the presence of dipole-dipole interactions and hydrogen bonding between the molecules of FFA and the selected amines.http://www.sciencedirect.com/science/article/pii/S2667312624000269Vapour-liquid equilibriumGreen solventGibbs energyActivity coefficient modelThermodynamic consistency testsMolecular interactions |
| spellingShingle | K.A. Sasikala K. Rayapa Reddy P.V.S. Sairam G. Srinivasa Rao Isobaric vapour-liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101.31 kPa Chemical Thermodynamics and Thermal Analysis Vapour-liquid equilibrium Green solvent Gibbs energy Activity coefficient model Thermodynamic consistency tests Molecular interactions |
| title | Isobaric vapour-liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101.31 kPa |
| title_full | Isobaric vapour-liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101.31 kPa |
| title_fullStr | Isobaric vapour-liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101.31 kPa |
| title_full_unstemmed | Isobaric vapour-liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101.31 kPa |
| title_short | Isobaric vapour-liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101.31 kPa |
| title_sort | isobaric vapour liquid equilibrium studies for binary systems of a green solvent furfuryl alcohol with aniline and substituted anilines at 101 31 kpa |
| topic | Vapour-liquid equilibrium Green solvent Gibbs energy Activity coefficient model Thermodynamic consistency tests Molecular interactions |
| url | http://www.sciencedirect.com/science/article/pii/S2667312624000269 |
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