Oxidation reactions Gibbs free energy

The reaction Gibbs free energies are for pH = 7 but otherwise standard conditions.) What amount (in moles) of ATP could be formed if all the Gibbs free energy released in the oxidation of... 

Heavy water is deuterium oxide, D20. The standard reaction Gibbs free energy for the autoprotolysis of pure deuterium oxide is +84.8 kj-mol 1 at 298 K. (a) If pD is defined analogously to pH, what is the pD of pure D20 at 298 K ... 

Keywords Annihilation Pathway Electron-transfer reaction Gibbs free energy Energy sufficient reaction Reductive-oxidation co-reactant Oxidative-reduction co-reactant Hot-electron ECL... 

The direct oxidative addition of methane to ethylene shown in the equation below is a thermodynamically favorable reaction (Gibbs free energy of-69 Kcal/mole). 

The reaction takes place spontaneously if the total change in the Gibbs free energy AG, including the oxide formation Gibbs free energy AGr and the possible dissolution of the cations in the metallic matrix. 

Upon burial in the sediments, organic matter is microbially oxidized in a sequence dictated by the Gibbs Free Energy yield of each reaction (Froelich et at., 1979). The oxidants are used in this sequence respiration of oxygen,... 

Electrode reactions are inner-sphere reactions because they involve adsorption on electrode surfaces. The electrode can act as an electron source (cathode) or an electron sink (anode). A complete electrochemical cell consists of two electrode reactions. Reactants are oxidized at the anode and reduced at the cathode. Each individual reaction is called a half cell reaction. The driving force for electron transfer across an electrochemical cell is the Gibbs free energy difference between the two half cell reactions. The Gibbs free energy difference is defined below in terms of electrode potential,... 

Stripping of chlorine from hydroxides such as Cl2Sn(OH)2 could eventually lead to gas-phase SnO or Sn02. However, at the relatively low temperatures typical of tin oxide CVD ( 873-973 K), we do not expect these oxides to form, based on the equilibrium calculations described above. Thus, the formation of tin hydroxides is not only thermodynamically favored (i.e., based on minimization of the Gibbs free energy), but there are also exothermic reaction pathways that we expect to be kinetically favorable. The primary tin carrier in the CVD process could therefore be a tin hydroxide. Complete conversion to Sn02 would most likely occur via reactions on the surface. 

The variation of the standard state Gibbs free energy change for the oxidation reaction at any temperature from experimentally measured variations in Po2,e r can be fitted to an equation of the form ... 

The American convention would assign a positive value to E° for the Zn Zn2+(aq) half cell written as an oxidation, but a negative sign if written as a reduction. It is seen that the European convention refers to the invariant electrostatic potential of the electrode with respect to the SHE, whereas the American convention relates to the thermodynamic Gibbs free energy which is sensitive to the direction of the cell reaction. 

Standard half-cell potentials can be used to compute standard cell potentials, standard Gibbs free energy changes, and equilibrium constants for oxidation-reduction reactions. 

The standard electrode potential E° of a redox reaction is a measure of the potential that would be developed if both reductants and oxidants were in their standard states at equal concentrations and with unit activities. The units of E° are volts and ° can be calculated from the Gibbs free energy change (AG ) of the redox reaction from the relationships... 

Table 13.1 lists the Gibbs free-energy change and the corresponding equilibrium-potential differences for the reactions of the oxidation of some currently used and potential fuels. 

Figure 5.2.2 Plot of Gibbs free energy changes of the thermal reduction (green line) (Fe3(>4 = 3 FeO + 1/2 O2), FeO oxidation (red line) (3 FeO + CO2 = Fe3C>4 + CO), and overall reaction (blue line) (CO2 = CO + 1/2 O2) for the iron-oxide-based cycle. The vertical lines show the melting points of the indicated iron-oxide phases.

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