Relevant bibliographies by topics / Gibbs surface excess of solutes

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Academic literature on the topic 'Gibbs surface excess of solutes'

Author: Grafiati
Published: 5 June 2025
Last updated: 24 June 2025

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Journal articles on the topic "Gibbs surface excess of solutes"

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A., Gani, Bhadra R., K. Chattoraj D., C. Mukherjee D., and Mitra Atanu. "Thermodynamics of excess binding of inorganic salts and organic solutes to crab hemocyanin." Journal of Indian Chemical Society 93, May 2016 (2016): 553–61. https://doi.org/10.5281/zenodo.5639349.

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Department of Food Technology and Biochemical Engineering, Jadavpur University, Kolkata-700 032, India Indian Institute of Chemical Biology, Kolkata-700 032, India Department of Chemistry, University of Calcutta, 92, Acharya Prafulla Chandra Road, Kolkata-700 009, India <em>Manuscript received 06 January 2016, accepted 23 March 2016</em> Using isopiestic vapor pressure technique, extents of water bound to complex metaloprotein hemocyanin obtained from crab have been determined in the absence and presence of inorganic salts, sucrose and urea at a fixed temperature. The water vapor absorption curve for hemocyanin in the range of water activity varying between zero to unity is type III BET isotherm. Moles of water absorbed per kg of hemocyanin at unit water activity a<sub>1</sub> have been evaluated by extrapolation method and the results support several models of bound water for different ranges of al. The standard free energies of adsorption &Delta;G0 for water-protein interaction at different temperatures have been calculated using Bull equation in integrated form. Based on Clausius-Clapeyron equation in integrated form, the integral enthalpy for water-hemocyanin interaction has also been evaluated. Using the isopiestic technique, values of excess binding ofsolute г<sup>2 1</sup> and г<sup>1 2</sup> excess binding of solvent per kg of hemocyanin in the presence of different bulk mole-fractions X<sub>2</sub> of solutes (LiCl, NaCl, KCl, NaBr, NaI, KSCN, urea, and sucrose) have been calculated in each case from the evaluated values of the Gibbs surface excess. In certain ranges of solute concentration, the plot of г1 2.X<sub><sup>2</sup></sub> vs X<sub>1</sub> becomes linear so that moles of water and solute bound per kg of hemocyanin respectively can be calculated. X<sub>1</sub> and X<sub>2</sub> stand for the mole-fraction of the solvent and solute in the bulk phase of the sample. Also, using integrated form of the Gibbs adsorption equation, standard free energy change (&Delta;G<sup>0</sup>) for the solute-hemocyanin and the solvent-hemocyanin interactions for different systems have been computed and the values have been compared critically.
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2

Tasneem, Shadma. "Tensiometric and Thermodynamic Study of Aliphatic and Aromatic Amine in Aqueous D-Glucose Solutions: A Comparative Study." Applied Sciences 13, no. 12 (2023): 7012. http://dx.doi.org/10.3390/app13127012.

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The surface tensions of aqueous taurine (TAU) and tyramine (TYR) with D-glucose mixed solvents were elevated from 298.15 to 318.15 K by the KSV sigma 702 tensiometer. The purpose of the study was to elucidate comparative studies of the thermodynamic and transport aggregation properties of aliphatic and aromatic amine, i.e., taurine and tyramine, which provide information in pharmacology and biochemistry. The experimental data investigated by this study were utilized to evaluate various interfacial parameters, including surface pressure, surface excess concentration, and other thermodynamic parameters of surface assembly, which are discussed in terms of solute–solvent and solute–solute interactions. The surface tension data have been analyzed using the Gibbs adsorption isotherm. The results signify that the negative isotherm exhibited by the ionic solute, i.e., taurine, an aliphatic amine, is contrary to the positive isotherm of tyramine, a biogenic aromatic amine. Both the amines exhibit surface properties such as surfactant molecules, which is elucidated in terms of ionic–hydrophilic and hydrophobic–hydrophobic interactions. The positive entropy values state that the process of surface formation is favored by entropy gain as well as the enthalpy effect. The present system provides a better understanding of the intermolecular interactions, which are required for their usefulness in the field of nutrition, pharmacy, and the food industry.
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3

Reddy, Ramana G., and Singareddy R. Reddy. "Derivation and consistency of the partial functions of a ternary system involving interaction coefficients." International Journal of Materials Research 95, no. 9 (2004): 806–12. http://dx.doi.org/10.1515/ijmr-2004-0149.

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Abstract Margules equations are used to express the thermodynamics of a ternary system containing one solvent and two solutes in the vicinity of solvent, in terms of first order interaction coefficients of binary and ternary systems. Considering just the first order Margules coefficients, the resultant excess Gibbs energy function was convergent and the derived logarithmic activity coefficients of solvent and solutes were thermodynamically consistent. In the present study Margules equations are modified to get consistent equations. Partial functions of a ternary system are deduced using these modified equations via the excess Gibbs energy function. Derived partial functions are thermodynamically consistent and also deduced results are the same as those obtained using Maclaurin infinite series. Using the activity coefficient expressions of solvent and solutes, the activity coefficients of solvent and solute are calculated in Ni– Cr–Fe and Fe–Ti –C ternary systems, which are in excellent agreement with the experimental data.
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4

Killmann, E. "Adsorption and the Gibbs surface excess." Journal of Colloid and Interface Science 112, no. 2 (1986): 602. http://dx.doi.org/10.1016/0021-9797(86)90132-3.

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5

Peterson, I. R. "Bulk aspects of the Gibbs surface excess parameters." Colloids and Surfaces A: Physicochemical and Engineering Aspects 102 (September 1995): 21–29. http://dx.doi.org/10.1016/0927-7757(95)03248-c.

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6

Postigo, Miguel A., José L. Zurita, María L. G. De Soria, and Miguel Katz. "Excess thermodynamic properties of n-pentane + dichloromethane system at 298.15 K." Canadian Journal of Chemistry 64, no. 10 (1986): 1966–68. http://dx.doi.org/10.1139/v86-325.

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Densities, refractive indices, viscosities, enthalpies, vapour–liquid equilibria, and surface tensions were determined for the n-pentane + dichloromethane system at 298.15 K. From the experimental results, excess molar volumes, excess viscosities, excess molar enthalpies, excess molar Gibbs free energies, and excess surface tensions were calculated. From these data, qualitative information could be obtained about the interaction between both chemical species.
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7

Sah, D. K., D. Adhikari, and S. K. Yadav. "Temperature-Dependence of Mixing Properties of Cu-Ti Liquid Alloy." Adhyayan Journal 10, no. 10 (2023): 1–10. http://dx.doi.org/10.3126/aj.v10i10.57306.

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In this study, the temperature-dependence of thermodynamic and surface properties of Cu-Ti binary liquid alloy were studied. In thermodynamic properties, excess Gibbs free energy of mixing, enthalpy of mixing, excess entropy of mixing, and activity of the system were computed at 1873 K. The surface properties were analyzed by computing the surface tension and surface concentration of the system. Thermodynamic properties were computed in the framework of the Redlich-Kister polynomial, and the surface properties were computed using the Butler model. At its melting point, the system exhibited a tendency for the formation of compounds, and as the Cu concentration was increased, the surface tension of the system gradually decreased. The excess Gibbs free energy of mixing, activity and surface tension of the system were also computed at different temperatures, in the range 1873-2173 K. With the increase in temperature of the system, the compound forming tendency of the system gradually decreased.
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8

DELGADO, Daniel R., Andrés R. HOLGUÍN, and Fleming MARTÍNEZ. "SOLUTION THERMODYNAMICS OF TRICLOSAN AND TRICLOCARBAN IN SOME VOLATILE ORGANIC SOLVENTS." Vitae 19, no. 1 (2012): 79–92. http://dx.doi.org/10.17533/udea.vitae.10838.

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Thermodynamic functions of Gibbs energy, enthalpy, and entropy for the solution processes of the antimicrobial drugs Triclosan and Triclocarban in five volatile organic solvents were calculated from solubility values at temperatures from 293.15 to 313.15 K. Triclosan and Triclocarban solubility was determined in acetone, acetonitrile (AcCN), ethyl acetate (AcOEt), methanol (MetOH), and cyclohexane (CH). The excess of Gibbs energy and the activity coefficients of the solutes were also calculated. The Triclosan solubilities were greater than those of Triclocarban in all the solvents studied. At 298.15 K the solubility diminished for Triclosan in the order, acetone &gt; AcOEt &gt; AcCN &gt; MetOH &gt; CH, while it diminished for Triclocarban in the order, acetone &gt; AcOEt &gt; MetOH &gt; AcCN &gt; CH. On the other hand, thermodynamic quantities relative to the transfer process of these drugs from CH to all other organic solvents, as well as from water to organic solvents for Triclosan were also calculated in order to estimate the hydrogen-bonding contributions.
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9

Yadav, S. K., N. Chaudhary, and D. Adhikari. "Thermodynamic, structural, surface and transport properties of Au-Ni liquid alloy at 1150 K." BIBECHANA 18, no. 1 (2021): 184–92. http://dx.doi.org/10.3126/bibechana.v18i1.30546.

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Thermodynamic, structural, surface, and transport properties of Au-Ni liquid alloy at 1150 K were computed using different theoretical approaches. The thermodynamic properties, such as excess Gibbs free energy of mixing, enthalpy of mixing, activity and excess entropy of mixing, and structural properties, such as concentration fluctuation in long-wavelength limit and Warren-Cowley short-range order parameter were computed in the framework of Flory’s model. The effect of positive and negative values of the interchange energy parameter on the excess Gibbs free energy of mixing and concentration fluctuation in the long-wavelength limit was also observed. The surface tension and surface concentration of the system were calculated using Butler’s model. In the transport property, the viscosity of the system was calculated using Kaptay and Budai-Benko-Kaptay (BBK) models.&#x0D; BIBECHANA 18 (2021) 184-192
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10

Tanaka, Toshihiro, Nev A. Gokcen, Dieter Neuschütz, Philip J. Spencer, and Zen-ichiro Morita. "Estimation of partial excess Gibbs energy of solutes in infinitely dilute liquid iron base binary alloys." Steel Research 62, no. 9 (1991): 385–89. http://dx.doi.org/10.1002/srin.199101317.

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Books on the topic "Gibbs surface excess of solutes"

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Chattoraj, D. Adsorption and the Gibbs Surface Excess. Springer London, Limited, 2012.

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Chattoraj, D. Adsorption and the Gibbs Surface Excess. Springer, 2013.

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Chattoraj, D. Adsorption and the Gibbs Surface Excess. Springer, 2013.

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Book chapters on the topic "Gibbs surface excess of solutes"

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Brezonik, Patrick L., and William A. Arnold. "Surface Chemistry and Sorption." In Water Chemistry, 2nd ed. Oxford University PressNew York, 2022. http://dx.doi.org/10.1093/oso/9780197604700.003.0012.

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Abstract This chapter focuses on how surfaces on suspended particles, nanoparticles, and sediments affect solute behavior and concentrations. The molecular structures of solids that yield various kinds of surfaces and interfaces are described, along with features of surfaces themselves. Forces that attract/repel solutes to/from surfaces are described with emphasis on electrical charge and excess surface energy, called surface tension. A major focus is on sorption, i.e., the accumulation of solutes onto surfaces. The Freundlich and Langmuir models that quantify this process are described along with more complicated models developed to overcome their limiting assumptions. Mechanistic models that consider the physics of the electrical double layer at solid-solution interfaces, e.g., the Gouy-Chapman double layer model, are developed, along with modern extensions. Surface complexation models that combine double-layer physics with a chemically oriented approach to quantify the interactions between ionic solutes and surfaces are described and examples of their use are given.
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Aveyard, Bob. "Adsorption of surfactants at liquid interfaces: thermodynamics." In Surfactants. Oxford University Press, 2019. http://dx.doi.org/10.1093/oso/9780198828600.003.0004.

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The thickness and hence material content of a surface is generally unknown, and there are two common definitions of a surface/interface. In one the surface is treated as a phase distinct from the surrounding bulk phases, and in the other, due to Gibbs, the Gibbs dividing surface is supposed to be a plane, parallel to the physical interface. The former model gives rise to the surface concentrationΓ‎s of a surfactant, and the Gibbs model introduces the surface excess concentration, Γ‎σ‎. Some thermodynamic quantities for surfaces (e.g. surface chemical potential and Gibbs free energy for surfaces) are defined. Adsorption lowers interfacial tension by an amount termed the surface pressure, and the Gibbs adsorption equation allows the calculation of Γ‎s or Γ‎σ‎ for a surfactant from the variation of interfacial tension of a liquid/fluid interface with surfactant concentration in bulk solution.
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Cantor, Brian. "The Gibbs-Thomson Equation." In The Equations of Materials. Oxford University Press, 2020. http://dx.doi.org/10.1093/oso/9780198851875.003.0006.

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The external surface of a material has an atomic or molecular structure that is different from the bulk material. So does any internal interface within a material. Because of this, the energy of a material or any grain or particle within it increases with the curvature of its bounding surface, as described by the Gibbs-Thomson equation. This chapter explains how surfaces control the nucleation of new phases during reactions such as solidification and precipitation, the coarsening and growth of particles during heat treatment, the equilibrium shape of crystals, and the surface adsorption and segregation of solutes and impurities. The Gibbs-Thomson was predated by a number of related equations; it is not clear whether it is named after J. J. Thomson or William Thomson (Lord Kelvin); and it was not put into its current usual form until after Gibbs’, Thomson’s and Kelvin’s time. J. J. Thomson was the third Cavendish Professor of Physics at Cambridge University. He discovered the electron, which had a profound impact on the world, notably via Thomas Edison’s invention of the light bulb, and subsequent building of the world’s first electricity distribution network. William Thomson was Professor of Natural Philosophy at Glasgow University. He made major scientific developments, notably in thermodynamics, and he helped build the first trans-Atlantic undersea telegraph. Because of his scientific pre-eminence, the absolute unit of temperature, the degree Kelvin, is named after him.
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Conference papers on the topic "Gibbs surface excess of solutes"

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Baselli, Silvia, and Alberto Molinari. "Cold Compacted Green Parts: A Focus On The Role Of The Structural Activity On Sintering Shrinkage." In World Powder Metallurgy 2022 Congress & Exhibition. EPMA, 2022. http://dx.doi.org/10.59499/wp225372160.

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The thermodynamic driving force of sintering is the decrease of the Gibbs free energy related to the excess of specific surface area of the powder. Nevertheless, for cold compacted green parts, the mass transport mechanisms which allow atoms to move to form the neck are promoted by the deformation in compaction that acts as a mechanical driving force expressed through the geometrical and structural activity. The powder particles are in contact over a surface, condition that affects the geometrical relationships in the neck region. The material is strain hardened, the concentration of structural defects is higher than that in the starting powder (enhanced diffusivity). The effect on sintering shrinkage of the geometrical activity has been explained in previous works and a theoretical model is available. To highlight how structural activity acts, a dilatometry study has been carried out on ferrous materials (plain iron and AISI 316L) and different powder morphology.
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