Abstract:An examination of the extent of quinhydrone formation between hydroquinone and p-benzoquinone in 20 dvferent pure and aqueous solvents indicated a reasonable correlation between extent of quinhydrone formation, as judged by the magnitude of the association constant and of the related standard free energy, and the surface tension (surface free energy) of the solvent. This supported the hypothesis of Sinanoglu and Abdulnur that the driving force of "hydrophobic bonding," e.g., in D N A double helix formation, is… Show more
“…In this case, when the scan rate is fast enough, since the slow formation of Q and QH 2 , the reduction of QH 2 could be inhibited which explained the disappearance of the corresponding reduction peak [19]. As for the assignment of the new peak, there was no conclusion, but possible processes suggested were the reduction of Q or (QH) 2 .…”
Section: Electro-oxidation Of Hydroquinone In Acetonitrilementioning
“…In this case, when the scan rate is fast enough, since the slow formation of Q and QH 2 , the reduction of QH 2 could be inhibited which explained the disappearance of the corresponding reduction peak [19]. As for the assignment of the new peak, there was no conclusion, but possible processes suggested were the reduction of Q or (QH) 2 .…”
Section: Electro-oxidation Of Hydroquinone In Acetonitrilementioning
“….H 2 Q? The old experimental data is ambiguous since for the formation of quinhydrone in water Kuboyama and Nagakura (1955) report negative values of DH (by a couple kcal/mol) while Moser and Cassidy (1965) report positive values of DG (by a couple kcal/ mol). Although these values are not necessarily contradictory, since we would expect the free energy change to be more positive than the enthalpy change for a complex formation reaction (we actually calculate a 10 kcal/mol difference, read infra), they do not generate a great deal of confidence.…”
Section: Energetics Of D:a Pair Formationmentioning
“…From the final p values, Dis(p-b) was calculated.The mean value, 7.2 x lo-'' m2/s, was used in the rest of the calculations. For a, the following equation was obtained: = 65,000 ro(15)…”
Theoretical calculations of reaction kinetics were done for one-step reactions catalyzed by cells immobilized in spherical beads. The reactions catalyzed by free cells were assumed to obey Michaelis-Menten kinetics for a one-substrate reaction. Both external (outside the beads) and internal (inside the beads) mass transfer of the substrate were considered for the immobilized preparations. The theoretical calculations were compared with experimental data for the oxidation of glycerol to dihydroxyacetone by Gluconobacter oxydans cells immobilized in calcium alginate gel. Glycerol was present in excess so that the reaction rate was limited by oxygen. The correlation between experimental data and theoretical calculations was quite good. The calculations showed how the overall effectiveness factor was influenced by, for example, the particle size and the cell density in the beads. In most cases the reaction rate was mainly limited by internal mass transfer of the substrate (oxygen). As shown previously, p-benzoquinone can replace oxygen as the electron acceptor in this reaction. The same equations for reaction kinetics and mass transfer were used with p-benzoquinone as the rate-limiting substrate. Parameters such as diffusivity, maximal reaction rate, and K were, of course, different. In this case also, the correlation between the model and the experimental results was quite good. Much higher production rates were obtained with p-benzoquinone as the electron acceptor compared to when oxygen was used. The reasons for this fact were that p-benzoquinone gave a higher maximal reaction rate for free cells and the solubility of p-benzoquinone was higher than for oxygen. Different methods of increasing the rate of microbial oxidation reactions are discussed.
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