Thermodynamic characteristics of the melting and dissolution of crystalline furan-2-carboxylic and 3-(furyl)-2-propenoic in organic solvent

Dibrivnyi²,

Horak³

et al. 2017

Abstract.1 The temperature dependencies of both acids solubility in acetonitrile, dimethylketone, isopropanol, ethylacetate and benzene were investigated. The results were represented by Shredder's equation according to which enthalpies, entropies and Gibbs energy of solubility at 298 K were determined. Fusion heats of the acids were determined using differential thermal analysis. In accordance with obtained values the enthalpies, entropies and Gibbs energy of mixing were calculated. The compensating effect of mixing was observed for al solvents with carboxy group.

Section: Introductionmentioning

confidence: 99%

“…Derivatograph cells were calibrated using standard samples of diphenyl (3.016 ± 0.032; 343.1 ± 0.3K) benzoic acid (3.413 ± 0.046; 396.8 ± 0.5K), adipic acid (10) More information about derivatograph calibration is presented in [10].…”

Section: Differential Thermal Analysismentioning

confidence: 99%

Thermodynamic properties of solubility of 2-methyl-5-arylfuran-3-carboxylic acids in organic solvents

Dibrivnyi²,

Horak³

et al. 2017

“…Since most reactions occur in solutions, the optimization of synthesis and purification of compounds with an arylfuran fragment is impossible without the determination of thermodynamic parameters of solubility. Some works regarding the thermodynamic properties of compounds with arylfuran fragment have appeared in recent years [12][13][14][15][16][17]. The presented work is the continuation of the previous research.…”

Section: Introductionmentioning

confidence: 82%

Thermodynamic Properties of 2-Methyl-5-arylfuran-3 Carboxylic Acids Chlorine Derivatives in Organic Solvents

Horak²,

Dibrivnyi³

et al. 2019

The temperature dependences of the solubility of 2-methyl-5-(2-chloro-5-trifluoromethylphenyl)-furan-3-carboxylic acid and 2-methyl-5-(2,5-dichlorophenyl)furan-3-carboxylic acid in acetonitrile, dimethyl ketone, isopropanol and ethyl acetate have been experimentally determined. The enthalpies of fusion of the investigated substances, as well as their enthalpies and entropies of mixing at 298 K have been calculated. The dependence of the saturated solution concentration on the values of enthalpy and entropy of solubility at 298 K has been determined. The compensating effect of mixing the investigated acids with all solvents containing the carbonyl group has been established.

“…3 where q fus and q vap -amount of heat absorbed during fusion and vaporization, respectively, J; m 0 -weight of the sample at the moment of fusion, g; ∆m vap -weight loss of the sample during the period to determine area S, g; Δ fus H and Δ vap H -specific enthalpies of fusion and vaporization at the fusion temperature, respectively, J/g; K -coefficient of heat transfer for the correspondence between the process heat efficiency and response as a peak area under DTA curve, J/K•s. The coefficient K was determined in [6] using standard solutions of silver nitrate, biphenyl, adipic and benzoic acids: K•10 2 = 3.668 -1.128•10 -2 Т + +2.723•10 -5 Т 2 ; S 2 = 5.96•10 -7 .…”

Section: B R H Solmentioning

confidence: 99%

“…of fusion ( Δ fus H 0 ) are calculated according to Eq. (5), where correction for weight loss during fusion is taken into account[6]:…”

mentioning

confidence: 99%

Thermodynamic Properties of 2-Cyano-3-[5-(Phenyl)-2-Furyl]-2-Propenamide and 2-Cyano-3-[5-(4-Methylphenyl)-2-Furyl]-2-Propenamide Solutions in Organic Solvents

Chetverzhuk²,

Horak³

et al. 2017

1 The fusion temperature of 2-cyano-3-[5-(phenyl)-2-furyl]-2-propenamide and 2-cyano-3-[5-(4-methylphenyl)-2-furyl]-2-propenamide and their temperature dependence of dissolution in acetonitrile, benzene, dimethylketone, ethyl acetate and 2-propanol have been determined. According to the temperature dependence the differential enthalpies and entropies of the solution were calculated. Taking into account the entropies of fusion the entropies and enthalpies of mixing were calculated at 298 K. The effect of intermolecular interaction in the investigated solutions on their solubility and enthalpies of mixing has been analyzed.