Topic
Standard molar entropy
About: Standard molar entropy is a research topic. Over the lifetime, 1586 publications have been published within this topic receiving 29886 citations.
Papers published on a yearly basis
Papers
More filters
01 Apr 2012
3 citations
TL;DR: In this paper, the authors examined the thermodynamic properties of polyoxypropylene glycol fractions in methanol, experimentally determined as described in Part I, and concluded that strong orientation effects are operative in the polymer-solvent interaction, presumably through hydrogen bonding with the solvent.
Abstract: The thermodynamic properties of the polyoxypropylene glycol fractions in methanol, experimentally determined as described in Part I, have been examined in terms of various statistical mechanical theories. The Flory-Huggins interaction parameter χ has been calculated and enthalpic and entropic components of χ deduced from the experimental data. Deviations from the Flory-Huggins theory are discussed. The thermodynamic excess functions for free energy and entropy of mixing are calculated, and it is concluded that strong orientation effects are operative in the polymer–solvent interaction, presumably through hydrogen bonding with the solvent. The hydroxylic endgroups on the short chain fractions play an important role in determining the thermodynamic behavior of the solutions. The role of orientation effects is examined by calculating the partial molar heat content and the partial molar entropy of the solvent and applying the theory of Munster for polymer solutions in which solvent orientation effects are operative. A semiempirical treatment, less arbitrary than that used by Munster, gives satisfactory results for polymer fractions of M. W. 150 and 1120.
3 citations
TL;DR: In this article, the standard entropy change ΔS° for the reduction of nonmagnetic, nonconducting oxides, MmOn(s) = mM(s + (n2)O2(g), has been estimated as a function of m, n, and temperature T from motional entropies of oxygen molecules and vibrational entropy of solid phases.
3 citations
10 Jul 1966
TL;DR: In this article, the equilibrium between F centers and M centers in additively colored KC1 was studied at temperatures between 60C and 130C, and the M-center concentration at equilibrium varied approximately as the square of the F center concentration, verifying the stoichiometric equation: 2F = M.
Abstract: : The equilibrium between F centers and M centers in additively colored KC1 was studied at temperatures between 60C and 130C. The M-center concentration at equilibrium varied approximately as the square of the F-center concentration, verifying the stoichiometric equation: 2F = M. At 60C, the equilibrium constant was 1.7 x 10 to the-19th power cu.cm. Enthalpy change = -4.1 Kcal and entropy change = -98 cal/deg, for the standard state one center cu.cm. The entropy change value agrees with that calculated from the configurational entropy, i.e., R 1n 6/N, where N is the concentration of negative ion sites. (Author)
3 citations
TL;DR: In this article, the standard thermodynamic functions of transfer of naphthalene and 2-naphthoic acid from water to (water+ethanol) mixtures at T =298.15 K have been determined from solubility measurements at different temperatures.
3 citations