For hydrogen peroxide decomposition

In fact, carbon and graphite exhibit good electrochemical activities for oxygen reduction, high overpotential for hydrogen evolution, and low catalytic activity for hydrogen peroxide decomposition (Do and Chen 1994a, b Ponce-de-Leon and Pletcher 1995). 

It is possible that some acetate radicals are formed by the direct discharge of the ions as, it will be seen shortly, is the case in non-aqueous solutions but an additional mechanism must be introduced, such as the one proposed above, to account for the influence of electrode material, catalysts for hydrogen peroxide decomposition, etc. It is significant that the anodes at which there is no Kolbe reaction consist of substances that are either themselves catalysts, or which become oxidized to compounds that are catalysts, for hydrogen peroxide decomposition. By diverting the hydroxyl radicals or the peroxide into an alternative path, viz., oxygen evolution, the efficiency of ethane formation is diminished. Under these conditions, as well as when access of acetate ions to the anode is prevented by the presence of foreign anions, the reactions mentioned above presumably do not occur, but instead peracetic acid is probably formed, thus,... 

In non-aqueous solutions the Kolbe electrosynthesis takes place with high eflSciency at platinized platinum and gold, as well as at smooth platinum, anodes increase of temperature and the presence of catalysts for hydrogen peroxide decomposition, both of which have a harmful effect in aqueous solution, have relatively little influence. The mechanism of the reaction is apparently quite different in non-aqueous solutions and aqueous solutions in the former no hydroxyl ions are present, and so neither hydroxyl radicals nor hydrogen peroxide can be formed. It is probable, therefore, that direct discharge of acetate ions occurs at a potential which is almost independent of the nature of the electrode material in a given solvent. The resulting radicals probably combine in pairs, as in aqueous solution, to form acetyl peroxide, which subsequently decomposes as already described. ... 

Two different catalysts for hydrogen peroxide decomposition, the enzyme peroxidase (isolated from the horseradish root, HRP), and polymer-supported catalyst (acid form of poly-4-vinylpyri-dine functionalized by ferric sulfate, apFe) [99,100], are examined with an aim to compare their activity. The active center in the peroxidases is the ferric ion in protoporphyrin IX. Besides the complex made of ferric ion and protoporphyrin IX, that is ferricprotoporphyrin IX, also known as ferric heme or hemin, peroxidase possesses a long chain of proteins [101,102]. On the other hand, the macroporous acid form of polyvinyl pyridine functionalized by ferricsulfate is obtained from cross-linked polyvinyl pyridine in macroporous bead form [103]. Pyridine enables it to form coordination complexes or quaternary salts with different metal ions such as iron (111) [104]. An active center on the polymeric matrix functionalized by iron, as metallic catalyst immobilized on polymer by pyridine, has similar microenvironment conditions as active center in an enzyme [105]. 

By the presence of either HRP or apFe, the Bray-Liebhafsky reaction is changed in a similar manner. Some amounts of the mentioned catalysts influence decrease, whereas the other amounts influence increase of the characteristic periods Ti and Tend - In other words, some amounts of mentioned catalysts cause the acceleration of the reactions (R), (O), and (D), whereas the other amounts cause their inhibition. Anyhow, by the presence of either HRP or apFe in the BL reaction, the new reaction system for hydrogen peroxide decomposition is formed. 

Analyzing different catalysts by means of an oscillatory reaction conducted in open and closed reactors as a matrix, it was shown that their characterization under mentioned conditions is, generally, possible and useful. Thus, by comparison with respect to dynamical effects of several catalysts in the matrix reaction system, the stmcture of active centers should be discussed. Particularly, analyzing two catalysts for hydrogen peroxide decomposition, the natural enzyme peroxidase and synthetic polymer-supported catalyst, the similarity in their catalytic activity is found. Hence, we can note that the evolution of the matrix oscillatory reaction can be used for determination of the enzyme activity. Moreover, one can see that the analysis of the granulation and active surface may also be performed by the oscillatory reaction. 

Iron compounds have long been known to function as catalysts for hydrogen peroxide decomposition. ... 

The hydroxide coprecipitates were air calcined at 250 or 350 C. For selected systems BET surface areas and carbon monoxide chemisorption measurements were made. Xray diffraction measurements were made on selected samples to characterize crystallinity. Catalytic performance tests were conducted at 20° C for hydrogen peroxide decomposition and benzaldehyde oxidation by hydrogen peroxide. 

TABLE 3 Catalytic activity for hydrogen peroxide decomposition benzaldehyde oxidation and base adsorption capacity and... 

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