Showing papers on "Gibbs–Helmholtz equation published in 1988"
TL;DR: In this article, the limits of stability of methane in liquid water were determined by using a cubic equation of state, recently proposed by Trebble and Bishnoi (1987), and applying the diffusional stability criterion.
43 citations
TL;DR: In this article, general expressions for partial Gibbs energies are derived from the Redlich-Kister polynomial for substitutional and interstitial solutions, and for the more general case of solution phases with two sublattices.
26 citations
TL;DR: In this paper, a set of coefficients is used to describe the conventional Gibbs free energy of the pure components and stoichiometric intermetallic compounds and the excess Gibbs energies of the solution phases.
17 citations
14 citations
TL;DR: Using Gibbs Energies of compounds, as well as Gibbs Energy changes and equilibrium constants of biochemical reactions, the contributions of functional groups to the Gibbs Energy (in aqueous solution, temperature 25°C, and pH=7) have been estimated as discussed by the authors.
Abstract: Using Gibbs Energies of compounds, as well as Gibbs Energy changes and equilibrium constants of biochemical reactions, the contributions of functional groups to the Gibbs Energy (in aqueous solution, temperature 25°C, and pH=7) have been estimated. These contributions allow the estimation of the Gibbs Free Energy and the equilibrium constant of a biochemical reaction, given the structure of the reactants and products.
12 citations
TL;DR: In this article, the assumption of local equilibrium and the Gibbs equation can effectively and consistently be applied, and individual quantities of transport are discussed in harmony with absolute quantities introduced by de Groot and Mazur.
Abstract: In many standard monographs of nonequilibrium thermodynamics, there are inconsistent parts of confusion in terminology as well as in notation, especially in the area of thermal diffusion, between quantities of transport and transported. Such a situation is corrected at an elementary level. As a result, the chemical potential of a diffusing species should be the “transported” Gibbs energy per mole. Based on this notion, the assumption of local equilibrium and the Gibbs equation can effectively and consistently be applied. Referring to a binary mixture, individual quantities of transport are discussed in harmony with “absolute” quantities introduced by de Groot and Mazur, in connection with the relative quantities of transport in common use.
3 citations
TL;DR: In this paper, the standard enthalpy of formation of KAlO2 was determined by hydrofluoric acid solution calorimetry to be Δ-Hf,298.15XXX, = −272.60±1.43 kcal mol−1.
2 citations