Gibbs energy enthalpy and entropy

Figure 3.3 Thermodynamic properties of an arbitrary ideal solution A-B at 1000 K. (a) The Gibbs energy, enthalpy and entropy, (b) The entropy of mixing and the partial entropy of mixing of component A. (c) The Gibbs energy of mixing and the partial Gibbs energy of mixing of component A.

Table 3.9 Standard Gibbs energy, enthalpy and entropy changes of solution for the sodium halides...

Tab. 2.6 Standard Gibbs energies, enthalpies, and entropies of transfer of ions from water to non-aqueous solvents (25 °C)1 ...

The state of a system is defined by its properties. Extensive properties are proportional to the size of the system. Examples include volume, mass, internal energy, Gibbs energy, enthalpy, and entropy. Intensive properties, on the other hand, are independent of the size of the system. Examples include density (mass/volume), concentration (mass/volume), specific volume (volume/mass), temperature, and pressure. 

Since K represents an equilibrium constant, it is possible to define quantities such as AG, A//, and A5 according to Eqs. (5-4) and (5-5), which are called the Gibbs energy, enthalpy, and entropy of activation, respectively. 

Association Constants, Gibbs Energies, Enthalpies, and Entropies of Ion-Pair Formation of Alkaii Metai and Tetraaikylammonium Iodides in 1-Propanol from Temperature-Dependent Conductivity Measurements... 

In order to study the mutual solubilities of hydrophobic but also hygroscopic imida-zolium-, pyridinium-, pyrrolidinium-, and piperidinium-based ILs in combination with the anions bis-(trifhioromethylsulfonyl)imide, hexafluorophosphate, and tricy-anomethane with water, UV spectroscopic measurements were carried out at temperatures between 288.15 and 318.15 K. Continuum model calculations were used to support these measurements of the Gibbs energy, enthalpy, and entropy. It was found that the hydrophobic tendency increases from imidazolium to pyridinium to pyrrolidinium to piperidinium and with increasing alkyl chain length within the same cation-varying anion ion pair [157],... 

Fig. 1.8 Excess Gibbs energy, enthalpy, and entropy for acetonitrile-water solutions at 25°C plotted against the mole fraction of acetonitrile.

Table 6.5 Solubilities and values of the changes in Gibbs energy, enthalpy and entropy of solution at 298 K for the halides of sodium and silver the entropy change is given in the form of a TASsot° term (T = 298 K). Hydrate formation by solid NaBr, Nal and AgF has been neglected in the calculation of AsoiG° for these compounds.

Figure 13 Thermodynamic parameters for the interaction between glucose oxidase and n-dodecyltrimethylammonium bromide (DTAB) as a function of the number of moles of DTAB bound per glucose oxidase molecule (v). AG- ( ), AH (A), and ASp (V) are the Gibbs energy, enthalpy, and entropy per mole of DTAB bound. The symbols and correspond to AG , and TASV corrected for statistical effects. (Data taken from Ref. 88.)...

Table VII-15 Standard molar Gibbs energies, enthalpies and entropies for the reactions + wHzOCl) Th COH) - + nit at 25°C.

VII.3.6.3 Standard molar Gibbs energies, enthalpies and entropies... 

Table VH-18 Selected standard molar Gibbs energies, enthalpies and entropies of formation for Th(IV) hydroxide complexes. In order to maintain a high level of numerical consistency, more digits are given than is justified by the precision of the data.

N. D. Douteau-Guevel, A. W. Coleman, J.-P. Morel, N. Morel-Desrosiers, Complexation of the basic amino acids lysine and arginine by three sulfonatocalix[n]arenes (n = 4, 6 and 8) in water microcalorimetric determination of the Gibbs energies, enthalpies and entropies of complexation, J. Chem. Soc., Perkin Trans. 2, 1999, 629-634. 

TABLE 1. Free Gibbs Energy, Enthalpy and Entropy of Formation of 1 Mole of Gallium Phosphide... 

Table 3.8 shows some values for the solvation Gibbs energy, enthalpy and entropy of cavity formation computed by Pierotti (1963, 1965) for water and benzene at 25°C and at latm. The effective diameters of argon and water for these calculations are [Pg.379]

If the world were made of pure substances, our development of the thermodynamic model would now be complete. We have developed a method, based on measurements of heat flow, that enables predictions to be made about which way reactions will go in given circumstances. But one of the reasons that the world is so complex is that pure substances are relatively rare, and strictly speaking they are nonexistent (even pure substances contain impurities in trace quantities). Most natural substances are composed of several components, and the result is called a solution. Therefore, we need to develop a way to deal with components in solution in the same way that we can now deal with pure substances - we have to be able to get numerical values for the Gibbs energies, enthalpies, and entropies of components in solutions. We will then be able to predict the outcome of reactions that take place entirely in solution, such as the ionization of acids and bases, and reactions that involve soUds and gases as well as dissolved components, such as whether minerals will dissolve or precipitate. Our thermodynamic model will then be complete. 

The standard Gibbs energy, enthalpy, and entropy changes for the hydrolysis of adeno ine-5 triphosphate to adenosine-5 -diphosphate are computed as a function of pH and aiagnesium ion concentration at 25 °C. A critical evaluation of the relevant literature data is included. Also see item [120]... 

Tabulated are single-ion entropies of about 110 diatomic and polyatomic ions in water Gibbs energies, enthalpies, and entropies of hydration of monatomic ions at 25 C partial molar volumes of about 120 common ions at 25 C ionic partial molar heat capacities of ions Gibbs energies of transfer of inorganic electrolytes from HjO to 020 and calorimetrically determined enthalpies of solution of salts in H2O and 020. 

Cell consisting of metal, metal oxide mixtures electrode, and a reference electrode can be used to determine thermodynamic values of Gibbs energy, enthalpy, and entropy firstly described by Kiukkola and Wagner [5] ... 

Gibbs energies, enthalpies, and entropies Appendix V (Cont.)... 

For the determination of standard Gibbs energies of reaction, a wide variety of experimental methods have been devised. These may be subdivided into e.m.f. measurements, equilibria with a gaseous phase, and distribution equilibria. From the temperature coefficients of the Gibbs energies, enthalpies and entropies of reaction can be deduced, but experience has shown that these cannot be relied upon when one or more solid phase takes part in the reaction, and errors are very difficult to assess. In such cases, it is recommended that the enthalpies of reaction are measured caloriraetrically and combined with the standard Gibbs energies to yield standard entropies of reaction. Calorimetric methods are also used to determine heat capacities, enthalpies of transformation, and enthalpies of fusion. Only for the determination of enthalpies of evaporation may... 

S.2.2.3 Thermodynamic Parameters The CMC value dependence on temperature is used for the determination of thermodynamic parameters applying models [60]. The mass action model, apparent and partial model, and phase separation model [14,59,60] are apphed to estimate the thermodynamic parameters Gibbs energy, enthalpy, and entropy of micelle formation. The enthalpy and entropy change for the miceUization can be determined using the Gibbs-Helmholtz equation [55]. 

The thermodynamic data, Gibbs energies, enthalpies and entropies of formation of intermetallic compounds have been obtained from a literature search. We have also consulted the handbook Selected values of thermodynamic properties of binary alloys by Hultgren et al. (1973a) and a compilation of thermodynamic data on transition metal based alloys done by de Boer et al. in 1988. For the actinide-based alloys a literature search and a critical analysis of the data was done by Rand and Kubaschewski (1963) for uranium compounds, by Rand et al. (1966) for plutonium alloys, by Rand et al. (1975) for thorium alloys, and more recently by Chiotti et al. (1981) for binary actinide alloys. We have included in our review the data obtained from the original publications and also the assessed data of Chiotti et al. (1981) when they were different. 

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