Journal of Chemical Thermodynamics最新文献

{"title":"Liquid−liquid equilibrium for ternary systems of 1-Octene +2-Hexanone + ionic liquid: Phase equilibrium measurement and correlation","authors":"Xianming Zhang ,&nbsp;Yanping Li ,&nbsp;Yongli Wu ,&nbsp;Yunfei Wang ,&nbsp;Panpan Yan ,&nbsp;Zhilei Zheng ,&nbsp;Hongyu Peng ,&nbsp;Yuexin Chu","doi":"10.1016/j.jct.2025.107483","DOIUrl":"10.1016/j.jct.2025.107483","url":null,"abstract":"<div><div>Liquid–liquid equilibrium (LLE) for the binary systems of 1-octene +1-ethyl-3-methylimidazolium acetate ([EMIM][Ac]), 1-octene +1-butyl-3-methylimidazolium acetate ([BMIM][Ac]), 1-octene +1-butyl-3-methylimidazolium tetrafluoroborate ([BMIM][BF₄]), 2-hexanone + [EMIM][Ac], and 2-hexanone + [BMIM][Ac], and the ternary systems of 1-octene +2-hexanone + [EMIM][Ac], 1-octene +2-hexanone + [BMIM][Ac], and 1-octene +2-hexanone + [BMIM][BF₄] were measured at 298.15 K, 303.15 K and 313.15 K under 101.3 kPa. The solute distribution coefficient (<em>D</em>) and selectivity (<em>S</em>) were calculated to investigate the efficiencies of [EMIM][Ac], [BMIM][Ac], and [BMIM][BF₄] as solvents. Moreover, the temperature dependencies of <em>D</em> and <em>S</em> were investigated in this study. NRTL and UNIQUAC models were applied to correlate the experimental LLE data.</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107483"},"PeriodicalIF":2.2,"publicationDate":"2025-03-11","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143621166","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Solubility determination, model evaluation, molecular simulation and thermodynamic analysis of sulfentrazone (Form I) in single and binary solvents","authors":"Haifang Mao ,&nbsp;Jiangmei Chen ,&nbsp;Qiyu Wang ,&nbsp;Mengjie Luo ,&nbsp;Zhiqing Li ,&nbsp;Changtao Zhou ,&nbsp;Bing Wei ,&nbsp;Jibo Liu ,&nbsp;Miaomiao Jin","doi":"10.1016/j.jct.2025.107475","DOIUrl":"10.1016/j.jct.2025.107475","url":null,"abstract":"<div><div>The molar fraction solubility of sulfentrazone (Form I) in ethanol, n-propanol, i-propanol, n-butanol, and binary solvents (ethanol + water) was measured by a laser dynamic method at temperatures from 278.15 <em>K</em> to 313.15 <em>K</em> under 101.6 <em>kPa</em> (standard uncertainty is <span><math><mi>u</mi><mfenced><mi>p</mi></mfenced></math></span> = 1.2 <em>kPa</em>). The solid-liquid phase equilibrium data were verified using five thermodynamic models: van't Hoff equation, modified Apelblat equation, <em>λh</em> equation, Wilson model, and modified Jouyban-Acree model. The modified Apelblat equation showed the best fitting results for the solubility correlation of sulfentrazone (Form I). In addition, the molecular interaction was analyzed using the Hirshfeld surface analysis, molecular electrostatic potential surface analysis, and Hansen solubility parameters to understand the dissolution mechanism of sulfentrazone (Form I). Molecular dynamics simulation was used to analyze the radial distribution function to explore intermolecular interactions of sulfentrazone (Form I) in ethanol + water binary solvents. Finally, the thermodynamic properties of sulfentrazone (Form I) in the studied solvents were also discussed using the van't Hoff equation, and the results implied that the dissolution of sulfentrazone (Form I) was an endothermic and entropy-driven process. The solubility data and the relevant thermodynamic analysis of sulfentrazone (Form I) provide fundamental guidance for the crystallization and purification of sulfentrazone (Form I).</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107475"},"PeriodicalIF":2.2,"publicationDate":"2025-02-28","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143548559","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Density, isothermal compressibility, isobaric thermal expansion, and related excess properties of mixtures of 2-(2-ethoxyethoxy)ethanol + 2-propanol at temperatures from 293.15 K to 353.15 K and pressures up to 70 MPa: Measurements, correlation, and PC-SAFT modeling","authors":"Mohamed Lifi ,&nbsp;Jean-Patrick Bazile ,&nbsp;Jean-Luc Daridon ,&nbsp;Eduardo A. Montero ,&nbsp;Fernando Aguilar ,&nbsp;Natalia Muñoz-Rujas","doi":"10.1016/j.jct.2025.107476","DOIUrl":"10.1016/j.jct.2025.107476","url":null,"abstract":"<div><div>High-temperature and high-pressure density data for the binary mixtures <em>x</em> 2-(2-ethoxyethoxy)ethanol + (1-<em>x</em>) 2-propanol are presented in this work, covering temperatures from 293.15 to 353.15 K and at pressures from 0.1 to 70 MPa. The experimental density data were generated using a vibrating tube densimeter with an uncertainty of 0.5 kg/m³. Experimental density data was fitted by using the Tait-like equation, yielding low standard deviations. Derivative properties such as excess molar volumes, isothermal compressibilities, excess isothermal compressibilities, and isobaric thermal expansions were calculated from the obtained density data. Additionally, the experimental measurements were modeled using PC-SAFT equation of state. The intermolecular interactions, as reflected in the derivative properties for each binary mixture, are thoroughly discussed.</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107476"},"PeriodicalIF":2.2,"publicationDate":"2025-02-28","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143548558","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Research on solubility, solvent effect and thermodynamics analysis of Lisinopril dissolution and molecular dynamics simulation","authors":"Yang Yu,&nbsp;Yue Wang,&nbsp;Cunbin Du","doi":"10.1016/j.jct.2025.107474","DOIUrl":"10.1016/j.jct.2025.107474","url":null,"abstract":"<div><div>The knowledge of solubility is indispensable in the pharmaceuticals development, crystal forms design, manufacturing and application. The high-quality solubility facilitates the selection of appropriate solvents for the formulation and purification of pharmaceutical products. In this study, the phase equilibrium of Lisinopril was established in ethanol, 1-propanol, 2-propanol, 1-butanol, acetone, acetonitrile, ethyl acetate, dimethyl sulfoxide (DMSO), <em>N,N</em>-dimethylformamide (DMF), <em>N</em>-methylpyrrolidone (NMP), as well as mixtures of DMSO + ethanol and DMSO +2-propanol. The solubility, solvent effect discussion, molecular dynamics (MD) simulations, molecular interaction analysis, model correlation and thermodynamics evaluation were all conducted. The outcomes of Lisinopril solubility in molarity show a direct correlation with temperature, and the rank was as listed: DMSO (1.013 × 10⁻³, 318.15 K) &gt; ethanol (3.887 × 10⁻⁴, 318.15 K) &gt; 1-propanol (3.277 × 10⁻⁴, 318.15 K) &gt; NMP (2.292 × 10⁻⁴, 318.15 K) &gt; 1-butanol (1.642 × 10⁻⁴, 318.15 K) &gt; DMF (1.217 × 10⁻⁴, 318.15 K) &gt; 2-propanol (8.504 × 10⁻⁵, 318.15 K) &gt; acetone (5.212 × 10⁻⁵, 318.15 K) &gt; acetonitrile (3.201 × 10⁻⁵, 318.15 K) &gt; ethyl acetate (1.851 × 10⁻⁵, 318.15 K). The solubility of Lisinopril in DMSO +2-propanol increased with the increasing content of DMSO, however, co-solvency phenomenon exhibited at <em>w</em> = 0.80 in mixture of DMSO + ethanol, and the maximum solubility is 1.271 × 10⁻³ (3.21-fold increase). The molecular interaction was discussed by preferential solvation in depth. Solvent effect was evaluated by KAT-LSER model which concluded that solute-solvent interactions significantly affect solubility more than solvent-solvent interactions. The contributions of solute-solvent interactions and solvent-solvent interactions 71.01 % and 28.99 %. Furthermore, MD simulation at the molecular level showed that hydrogen bonds can form more readily between molecules and play a crucial role in enhancing dissolution of Lisinopril. Additionally, the Apelblat, Wilson, Jouyban-Acree and Apelblat-Jouyban-Acree models were applied to correlate the Lisinopril solubility data. The greatest values of relative average deviation (<em>RAD</em>) and root-mean-square deviation (<em>RMSD</em>) values were 1.75 % and 1.68 × 10⁻⁵, respectively. Finally, the values of thermodynamic properties were all positive which indicated that the dissolution of Lisinopril was an endothermic and entropy increment process.</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107474"},"PeriodicalIF":2.2,"publicationDate":"2025-02-27","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143592414","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Gas mixture analysis by temperature-independent, multi-wavelength refractive mixing rules","authors":"J.B.S. Santos ,&nbsp;H.A. Helfstein ,&nbsp;M.T. Saita ,&nbsp;F.T. Degasperi ,&nbsp;R.B. Torres ,&nbsp;E.A. Barbosa","doi":"10.1016/j.jct.2025.107473","DOIUrl":"10.1016/j.jct.2025.107473","url":null,"abstract":"<div><div>The characterization of gaseous mixtures is an increasingly important issue in the fields of fuel analysis and aerosol research. Analyses by refractometry combined with refractive mixing rules are also powerful tools in this area. In this work a setup comprised by a six-laser interferometer and a vacuum system was projected and constructed in order to measure the refractivity of pure inert gases like N₂, CO₂, Ar and O₂ and to study the validity of the refractive mixing rules with binary mixtures of N₂ and Ar for different wavelengths. The light sources used in the experiments were a He<img>ne laser (632.8 nm), a frequency-doubled diode-pumped Nd:YAG laser (532 nm) and four diode lasers emitting at 406.4 nm, 453 nm, 655.3 nm and 825 nm. The experimental refractivity data of the binary mixtures were compared with the theoretical ones obtained from a modified, temperature invariant, Gladstone-dale based refractive mixing rule, by introducing the parameter thermal refractivity (TR). The results obtained by the modified refractive mixing rule proposed by us for dry air were also compared with the refractive measurements of atmospheric air for the six wavelengths. In general the experimental results have shown good agreement with the theoretical predictions, and the dispersive character of the thermal refractivities point out to promising applications in evaluating gas mixtures.</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107473"},"PeriodicalIF":2.2,"publicationDate":"2025-02-25","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143512352","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Solid-liquid equilibrium of abscisic acid in twelve pure solvents: Experiments, modeling, and molecular simulation","authors":"Ting Qin ,&nbsp;Jiawei Zhao ,&nbsp;Xiongtao Ji ,&nbsp;Jinyue Yang ,&nbsp;Na Wang ,&nbsp;Baohong Hou ,&nbsp;Ting Wang ,&nbsp;Hongxun Hao","doi":"10.1016/j.jct.2025.107472","DOIUrl":"10.1016/j.jct.2025.107472","url":null,"abstract":"<div><div>Abscisic acid (ABA) is one of the five natural growth regulators for plants and crystallization technology is used in the manufacturing of it. The thermodynamic behavior of it plays an important role in the development and design of crystallization processes. In this study, the solubility of ABA in twelve pure solvents was gravimetrically investigated over the temperature range of 278.15 K to 313.15 K. It was found that the solubility of ABA increased steadily with the rise of temperature. Four thermodynamic models (the modified Apelblat equation, <em>van't Hoff</em> equation, <em>λh</em> model and NRTL model) were applied to correlate the experimental solubility data, and the modified Apelblat equation model showed better fitting performance. The mixed thermodynamic properties of ABA in various pure solvents were also calculated, indicating that the mixed process is spontaneous and entropy-driven. Furthermore, to further explore the solid–liquid equilibrium behavior, Hirshfeld surface of ABA crystal was calculated and molecular dynamics simulations of different systems were performed. Based on equilibrium configurations of different systems, solute–solvent interaction energy was calculated, providing a reasonable explanation for the solubility of ABA. Meanwhile, the radial distribution function (RDF) plots were also employed to analyze the hydrogen bonding interactions between ABA molecules and solvent molecules.</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107472"},"PeriodicalIF":2.2,"publicationDate":"2025-02-21","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143509486","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Determination of the thermodynamic quantities for complex formation of U(VI) with amino acids in aqueous solution","authors":"Akira Kirishima ,&nbsp;Masahide Takei ,&nbsp;Akihiro Uehara ,&nbsp;Daisuke Akiyama","doi":"10.1016/j.jct.2025.107469","DOIUrl":"10.1016/j.jct.2025.107469","url":null,"abstract":"<div><div>The thermodynamic quantities (Δ<em>G</em>, Δ<em>H</em>, and Δ<em>S</em>) for the formation of U(VI) complexes with three amino acids, L-serine, L-phenylalanine, and L-cysteine were determined, where the stability constants were obtained by potentiometric titration and the reaction enthalpies were directly measured by calorimetric titration. Prior to the U(VI) complexation study, the Δ<em>G</em>, Δ<em>H</em>, and Δ<em>S</em> of the protonation of the three amino acids were determined using the same techniques. The obtained thermodynamic quantities are compared to discuss the complex formation's driving forces and mechanism. The obtained thermodynamic data indicates that U(VI)-L-serine and U(VI)-L-phenylalanine complexes are entropy-driven reactions, whereas a significant enthalpy benefit drives L-cysteine complexation. From the comparison between the obtained thermodynamic data in this study and the spectroscopic and theoretical analyses in previous research, it was suggested that the complex formation of the amino acid with U(VI) proceed without significant involvement of the amino group while the thiol group in L-cysteine significantly contributes to the complexation with U(VI).</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107469"},"PeriodicalIF":2.2,"publicationDate":"2025-02-20","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143534154","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"OA","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Phase transition thermodynamics of organic semiconductors N,N,N′,N′-tetraphenyl-p-phenylenediamine, N,N′-diphenyl-N,N′-di-p-tolylbenzene-1,4-diamine, and 4,4′-bis(m-tolylphenylamino)biphenyl","authors":"Airat A. Notfullin,&nbsp;Dmitrii N. Bolmatenkov,&nbsp;Andrey A. Sokolov,&nbsp;Ilya S. Balakhontsev,&nbsp;Alexander D. Kachmarzhik,&nbsp;Boris N. Solomonov,&nbsp;Mikhail I. Yagofarov","doi":"10.1016/j.jct.2025.107470","DOIUrl":"10.1016/j.jct.2025.107470","url":null,"abstract":"<div><div>In this paper, we report a comprehensive analysis of the thermodynamic properties of organic semiconductors, namely, <em>N,N,N′,N′</em>-tetraphenyl-<em>p</em>-phenylenediamine (DDP), <em>N,N′</em>-diphenyl-<em>N,N′</em>-di-<em>p</em>-tolylbenzene-1,4-diamine (<em>p-</em>TTP), and 4,4′-bis(<em>m</em>-tolylphenylamino) biphenyl (TPD). Vapor pressures above crystalline and liquid (including supercooled liquid) phases over a wide temperature range were measured using thermogravimetry-fast scanning calorimetry method (TG- FSC). Based on the vapor pressures, the vaporization and sublimation enthalpies of the studied compounds were derived. Heat capacities of condensed phases, melting points and fusion enthalpies of DDP, <em>p-</em>TTP, and TPD were measured by differential scanning calorimetry. Using the measured heat capacities of the liquid and crystalline phases and the computed heat capacities of the ideal gas phase, the experimental data obtained in the present work were adjusted to 298.15 K and compared with the available literature values. For additional verification of the obtained results, the solution calorimetry method was applied, providing an independent way to determine fusion enthalpies at 298.15 K. The obtained data can be used for optimization of the vacuum deposition processes and determination of thermodynamic properties of glasses.</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107470"},"PeriodicalIF":2.2,"publicationDate":"2025-02-20","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143480425","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Thermodynamic properties and thermodynamic modelling for aqueous mixed system containing sodium tetraborate and sodium pentaborate","authors":"Ruyi Lin ,&nbsp;Shuaiqi Sun ,&nbsp;Qingfen Meng ,&nbsp;Dan Li ,&nbsp;Yong Ma ,&nbsp;Lingzong Meng ,&nbsp;Yafei Guo ,&nbsp;Tianlong Deng","doi":"10.1016/j.jct.2025.107471","DOIUrl":"10.1016/j.jct.2025.107471","url":null,"abstract":"<div><div>The solubilities and physicochemical properties in the system Na₂B₄O₅(OH)₄–NaB₅O₆(OH)₄–H₂O at 323.15 K were studied with the isothermal dissolution method. The phase diagram in the system is composed of one co-saturation point, two solubility curves and two single-salt crystallization regions for Na₂B₄O₅(OH)₄·8H₂O and NaB₅O₆(OH)₄·3H₂O. The water activities and osmotic coefficients were determined based on the sodium chloride standard reference solution with the isopiestic method. With the assumption of only two boron species B₄O₅(OH)₄²⁻ and B₅O₆(OH)₄⁻ in the solution, the single salt parameters of NaB₅O₆(OH)₄ and mixing ion interaction parameters in the system were fitted with the solubilities and water activities based on Pitzer model. The dissolution equilibrium constants of NaB₅O₆(OH)₄·3H₂O were obtained with the activity product constant method. The agreement for the calculated solubilities and water activities with the experimental results in the system shows that the Pitzer model with the above assumption can be used to describe the experimental values.</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"206 ","pages":"Article 107471"},"PeriodicalIF":2.2,"publicationDate":"2025-02-20","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143488906","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}

{"title":"Solubility determination, correlation, solvent effect and thermodynamic properties of tolnaftate in ten mono-solvents and binary solvent systems from 283.15 K to 328.15 K","authors":"Kejia Wang ,&nbsp;Wei Zhang ,&nbsp;Yuanmo Ren ,&nbsp;Ting Li ,&nbsp;Shiyu Lin ,&nbsp;Funeng Xu ,&nbsp;Haohuan Li ,&nbsp;Xianxiang Wang ,&nbsp;Huaqiao Tang ,&nbsp;Gang Shu ,&nbsp;Juchun Lin ,&nbsp;Xiaoyang Ai ,&nbsp;Hualin Fu","doi":"10.1016/j.jct.2025.107468","DOIUrl":"10.1016/j.jct.2025.107468","url":null,"abstract":"<div><div>Tolnaftate (TNF) is a local antifungal agent. The determination of its solubility can serve as a valuable reference for its crystallization and formulation design, an area that has not yet been comprehensively investigated. In this study, the static method was carried out to determine the solubility of TNF in 10 mono-solvents (methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, n-octanol, 1,2-propanediol, ethylene glycol, acetic acid) and the binary mixed solvents (acetic acid + ethylene glycol) at T = (283.15 to 328.15) K and <em>P</em> = 0.1 MPa. The experiment results showed that TNF dissolves best in acetic acid and worst in ethylene glycol among investigated mono-solvents. And the solubility in mixed solvents was observed to increase as the mole ratio of acetic acid augments. In all solvents, there is obviously increase in the solubility of TNF as temperature elevates. The Apelblat model, van't Hoff model, Jouyban model, GCM model, Sun model and Apelblat-Jouyban-Acree model were used to fit the solubility values. And the root mean square deviation (RMSD) between the calculated values and experimental values are less than 0.025 %, showing that the experimental values are accurate and the models have good fitting effects. At the same time, X-ray powder diffraction (PXRD) tests confirmed that the absence of crystal transformation during the process of TNF dissolution. In addition, according to the KAT-LSER model, the influence of solute-solvent interactions on the solubility of TNF exceeds that of solvent-solvent interactions. The thermodynamic properties including entropy (Δ<em>H</em>⁰_sol), enthalpy (Δ<em>S</em>⁰_sol), Gibbs free energy (Δ<em>G</em>⁰_sol), enthalpy contribution (%ξ_H) and entropy contribution (%ξ_S) were calculated, which proved that dissolution process of TNF is endothermic and entropy-driven, and enthalpy mainly affects Gibbs free energy.</div></div>","PeriodicalId":54867,"journal":{"name":"Journal of Chemical Thermodynamics","volume":"205 ","pages":"Article 107468"},"PeriodicalIF":2.2,"publicationDate":"2025-02-14","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":null,"resultStr":null,"platform":"Semanticscholar","paperid":"143427992","PeriodicalName":null,"FirstCategoryId":null,"ListUrlMain":null,"RegionNum":3,"RegionCategory":"工程技术","ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":"","EPubDate":null,"PubModel":null,"JCR":null,"JCRName":null,"Score":null,"Total":0}