Showing papers on "Gibbs–Helmholtz equation published in 1986"
TL;DR: In this article, the authors constructed a consistent equation of state valid over a large part of the operating range of the diamond anvil cell, and derived the thermodynamic properties of molecular hydrogen.
Abstract: Using data available from literature for hydrogen in the liquid and solid phases the authors constructed a consistent equation of state valid over a large part of the operating range of the diamond anvil cell. A large part of the experimental data is reproduced within 0.1% and practically all data within 0.5%. From this equation of state they derived the thermodynamic properties of molecular hydrogen. The volume, entropy, Gibbs free energy and enthalpy are tabulated as a function of temperature and pressure for P
157 citations
TL;DR: In this paper, a set of parameter values describing the Gibbs energy of each individual phase as a function of temperature and pressure is given. And the experimental information on the P, T phase diagram and the thermodynamical data are compared with calculations made using the presented set of parameters.
97 citations
TL;DR: In this article, a comprehensive equation for the thermodynamic properties of aqueous NaI, CsF and HCl is generated by combining the heat capacity and density measurements reported by the first author with literature data for the enthalpy and Gibbs energy, or activity, as a function of molality at 298 K.
Abstract: Comprehensive equations for the thermodynamic properties of aqueous NaI, CsF, CsCl, CsI, NaIO3, KIO3, CsIO3, KClO4, and HCl are generated by combining the heat capacity and density measurements reported by the first author with literature data for the enthalpy and Gibbs energy, or activity, as a function of molality at 298 K. The composition dependence is represented by the equations of Pitzer, which combine a theoretical form and Debye–Huckel terms with empirically evaluated parameters for short-range ion interactions. Temperature dependencies are represented by simple empirical equations, which should be reliable to 413 K or a little higher.
13 citations
12 citations