Gibbs energy selected oxides

Practically in every general chemistry textbook, one can find a table presenting the Standard (Reduction) Potentials in aqueous solution at 25 °C, sometimes in two parts, indicating the reaction condition acidic solution and basic solution. In most cases, there is another table titled Standard Chemical Thermodynamic Properties (or Selected Thermodynamic Values). The former table is referred to in a chapter devoted to Electrochemistry (or Oxidation - Reduction Reactions), while a reference to the latter one can be found in a chapter dealing with Chemical Thermodynamics (or Chemical Equilibria). It is seldom indicated that the two types of tables contain redundant information since the standard potential values of a cell reaction ( n) can be calculated from the standard molar free (Gibbs) energy change (AG" for the same reaction with a simple relationship... 

C-H and C-C bond cleavage in a radical cations is feasible, but not a versatile option for synthetic use because of the very high oxidation potentials. Deprotonations in alkane radical cations have strongly negative Gibbs energies, with strong preference for tertiary over secondary or primary C-H bonds [118]. C-C bonds are selectively weakened in strained carbocycles [119]. 

An account of the gaseous species observed by Knudsen effusion mass spectrometry in the eqilibrium vapor of metals, alloys, oxides, halides, and technical systems is given. The fundamentals and recent developments of this method are briefly reported. Dissociation and atomization enthalpies of selected gaseous species are tabulated. Accounts of the equilibrium studies by Knudsen effusion mass spectrometry in order to obtain thermodynamic properties for condensed phases from gas phase data are additionally given for the aforementioned materials. Table 8 shows as an example the enthalpies and Gibbs energies of formation for different solid intermetallic compounds. A special section (Sect. 

Figure V-9 Comparison between the temperature dependence of the Gibbs energy of formation for NiO obtained from electrochemical as well as chemical reduc-tion/oxidation equilibrium measurements and the prediction based on the present selection of thermodynamic properties for NiO.

The 1978 publication is a 456 page monograph containing selected values for the entropy, molar volume, and for the enthalpy and Gibbs energy of formation for the elements, 133 oxides, and 212 other minerals and related substances at 298.15 K. Thermal functions are also given for those substances for which heat-capacity or heat-content data are available. The thermal functions are tabulated at 100 K intervals for temperatures up to 1800 K. The monograph includes detailed references to the source literature and a compound index. 

FIG. 6—Standard Gibbs energies of formation of selected oxides as a function of temperature ftII. 

Allen s book discusses equilibrium constants, entropy in terms of disorder, and formulae for the derivation of values of entropy from heat capacity measurements. An important part of the book discusses energy changes in relation to the Periodic classification and to chemical bonding. Gibbs energies of formation are plotted for some series of compounds (e.g. oxides and chlorides) against atomic number. There is a thermodynamic study of the problem of selection of a catalyst for the Deacon process. 

Let us consider a rock at temperature T whose chemical composition q (recipe) is expressed as the vector of all the molar fractions x0 of s elements or oxides. It is assumed that it can be made by an arbitrarily large number p s of mineral phases exclusive of solid solution. B is the component matrix of these minerals for the selected set of elements or oxides. Let nj be the number of moles of mineral j and gj its Gibbs free energy of formation AGf T estimated when formed from either the elements or the oxides. The function to be minimized is the Gibbs free energy G given by... 

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