Hydrogen peroxide decomposition photochemical

Thermal or Photochemical Decomposition of Hydrogen Peroxide Hydrogen peroxide decomposition can occur by homolytic or heterolytic scission... 

The radicals are then involved in oxidations such as formation of ketones (qv) from alcohols. Similar reactions are finding value in treatment of waste streams to reduce total oxidizable carbon and thus its chemical oxygen demand. These reactions normally are conducted in aqueous acid medium at pH 1—4 to minimize the catalytic decomposition of the hydrogen peroxide. More information on metal and metal oxide-catalyzed oxidation reactions (Milas oxidations) is available (4-7) (see also Photochemical technology, photocatalysis). 

The decomposition of liquid water and the following reactions are the results of a typical chemical effect. In this case, however, overall water splitting does not occur because oxygen is not obtained but hydrogen and hydrogen peroxide are. On the other hand, it is impossible to decompose water by photochemical reaction under illumination with a xenon lamp. Although it is possible to decompose water by photocatalytic reaction using a desirable photocatalyst and photoirradiation, it is difficult to decompose in practice because of rapid backward reaction, the formation and accumulation of intermediates onto the surface of photocatalyst,10) and other reasons. 

Temperature will affect the degradation rate of different organic pollutants. Weir et al. (1987) reported that benzene and hydrogen peroxide are insensitive to temperature because photochemically induced reactions often have low activation energies. Koubek (1975) stated that temperature has little effect on the oxidation of refractory organics however, Sundstrom et al. (1986) observed that the decomposition rates of some halogenated aliphatics increased with temperature. 

The acrylamide post-polymerization initiated by photochemical (k = 313 nm) decomposition of hydrogen peroxide in aqueous media can take place in the course of several days 78) after cutting off the UV source. Three structures of the terminal radicals have been suggested... 

In addition to the photoelectrochemical (catalysed by Ti02) mechanism discussed above, also the chemical and photochemical mechanisms of H2O2 decomposition are to be considered. In strongly irradiated, alkaline solutions the direct photolysis of hydrogen peroxide (strictly speaking-of HO2 ions) should seriously be taken into account for the... 

J.W. Moffett, O.C. Zafiriou (1993). The photochemical decomposition of hydrogen peroxide in surface waters of the Eastern Caribbean and Orinoco River. J. Geophys. Res., 98,2307-2313. 

J.P. Hunt, H. Taube (1952). The photochemical decomposition of hydrogen peroxide. Quantum yields, tracer and fractionation effects. Nature, 74, 5999-6002. 

Egerton [197, 198J found that hydrogen peroxide vapour and its radical decomposition products can degrade polymers. Also Egerton et al. [198, 199, 201] reported that many different dyes, such as acriflavin and eosin, sensitize the photochemical oxidation of textile fibres. 

However, although the Haber-Willstatter chain reactions have been assumed to occur in certain catalytic systems, notably the ferrous-ferric ion system (4), more recent evidence to be described subsequently, does not support this assumption. On the other hand, such reactions appear to offer the most plausible explanation for the photochemical decomposition of hydrogen peroxide, although even here a satisfactory analysis of the kinetics has yet to be made. 

It is well known that hydrogen peroxide which absorbs fairly strongly in the region below 3100 A. undergoes photochemical decomposition. 

Several pathways can account for the decomposition of hydrogen peroxide In natural waters. Some of these decay processes not only remove H2O2, but also result In the oxidation of chemicals, possibly Including various pollutants, that are present In natural waters. These processes Include direct oxidation (5), peroxidase-catalyzed oxidation (6), and free radical oxidation Initiated by photochemical or metal-catalyzed decomposition (7). Little Is known about the significance and rates of these various processes under environmental conditions, but they have all been shown to occur rapidly with certain organic substrates In the laboratory. 

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