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Thermodynamics of fenoxycarb in solution
KTH, School of Chemical Science and Engineering (CHE), Chemical Engineering and Technology, Transport Phenomena. SSPC, University of Limerick, Ireland.ORCID iD: 0000-0002-6647-3308
KTH, School of Chemical Science and Engineering (CHE), Chemical Engineering and Technology, Transport Phenomena.
2013 (English)In: Journal of Chemical Thermodynamics, ISSN 0021-9614, E-ISSN 1096-3626, Vol. 66, 50-58 p.Article in journal (Refereed) Published
Abstract [en]

The solubility of fenoxycarb has been determined between 278 and 318 K in several organic solvents. The solid phase at equilibrium and some indication of polymorphism has been properly examined by powder XRD, DSC, Raman and ATR-FTIR spectroscopy, solution H-1 NMR and SEM. Using literature data the activity of the solid phase within a Raoult's law definition has been calculated, based on which solution activity coefficients have been estimated. In ethyl acetate, the van't Hoff enthalpy of solution is constant over the temperature range and equals the melting enthalpy. However, it is shown that the solution is slightly non-ideal with the heat capacity difference term compensating for the activity coefficient term. In toluene, the van't Hoff enthalpy of solution is constant as well but clearly higher than the melting enthalpy. In methanol, ethanol and isopropanol, van Hoff curves are strongly non-linear, the slope however clearly approaching the melting enthalpy at higher temperatures. In all solvents, positive deviations from Raoult's law are prevailing. The activity coefficients follow a decreasing order of isopropanol > ethanol > methanol > toluene > ethyl acetate, and in all solvents decrease monotonically with increasing temperature. The highest activity coefficient is about 18 corresponding to about 2.5 kJ/mol of deviation from ideality.

Place, publisher, year, edition, pages
Elsevier, 2013. Vol. 66, 50-58 p.
Keyword [en]
Solubility, Activity, Activity coefficient, Van't Hoff enthalpy, Ideal solution, Heat capacity
National Category
Chemical Engineering
URN: urn:nbn:se:kth:diva-129098DOI: 10.1016/j.jct.2013.06.007ISI: 000323600600007ScopusID: 2-s2.0-84880380345OAI: diva2:650262
Swedish Research Council, 621-2010-5391

QC 20130920

Available from: 2013-09-20 Created: 2013-09-19 Last updated: 2016-10-27Bibliographically approved

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