Peroxy nitric acid

C-polyaromatic hydrocarbons deoxyribonucleic acid environmental Protection Agency peroxy nitric acid nitric acid lipopolysaccharide nitrogen/Carbon isocynate radical N-nitrosodibuty lamine N-nitrosodiethylamine N-nitrosodiethanolamine N-nitrosodimethylamine N-nitrosodiphenylamine N-nitrosoethylmethylamine... 

According to Amels et al. (1996), the S(TV) oxidation by peroxy nitric acid can proceed very rapidly with the simultaneous formation of nitrate ... 

Both oxidation pathways, the NOs catalysed oxidation of S(IV) by molecular oxygen and the oxidation of S(IV) by peroxy nitric acid lead to the formation of sulphate anions and further studies are required to decide, which of the two pathways is the mot important (or... 

The production of peroxy nitric acid (HO2NO2) by the reaction of HO2 and NO2 has a possibility to act as the termination reaction of OH — HO2 radical chain reaction, but since HO2NO2 is thermally unstable and decomposes back to HO2 and NO2 at around the room temperature, it generally does not affect the formation of ozone... 

Oxidation. Acetaldehyde is readily oxidised with oxygen or air to acetic acid, acetic anhydride, and peracetic acid (see Acetic acid and derivatives). The principal product depends on the reaction conditions. Acetic acid [64-19-7] may be produced commercially by the Hquid-phase oxidation of acetaldehyde at 65°C using cobalt or manganese acetate dissolved in acetic acid as a catalyst (34). Liquid-phase oxidation in the presence of mixed acetates of copper and cobalt yields acetic anhydride [108-24-7] (35). Peroxyacetic acid or a perester is beheved to be the precursor in both syntheses. There are two commercial processes for the production of peracetic acid [79-21 -0]. Low temperature oxidation of acetaldehyde in the presence of metal salts, ultraviolet irradiation, or osone yields acetaldehyde monoperacetate, which can be decomposed to peracetic acid and acetaldehyde (36). Peracetic acid can also be formed directiy by Hquid-phase oxidation at 5—50°C with a cobalt salt catalyst (37) (see Peroxides and peroxy compounds). Nitric acid oxidation of acetaldehyde yields glyoxal [107-22-2] (38,39). Oxidations of /)-xylene to terephthaHc acid [100-21-0] and of ethanol to acetic acid are activated by acetaldehyde (40,41). 

The nomenclature for this homologous series is somewhat confused. The term PANs has been used historically to denote peroxyacyl nitrates, and this terminology continues to be used extensively in the literature, despite the lack of adherence to traditional IUPAC rules of nomenclature. Because the PANs can be considered to be mixed anhydrides of carboxylic acids and nitric acid, another suggestion (Roberts, 1990) has been peroxyacetic nitric anhydride for CH,C(0)00NO2 and peroxy carboxylic nitric anhydrides for the whole class of compounds. Although it does not follow the IUPAC rules, it would be consistent with the widespread use of the name PAN but also reflect the structure more accurately. Table 6.20 shows the structures and commonly used names of some PANs that have been observed in the atmosphere and/or in laboratory studies. 

The relationship between the peroxy radical concentration and the ozone photolysis rate constant for these higher NO conditions can be again approximated using steady-state analysis (Penkett et al., 1997 Carpenter et al., 1997). While OH is recycled in its reactions with CO and CH4 via H02, it is permanently removed at higher NOx concentrations by the reaction of OH with N02, forming nitric acid ... 

Phosphorus anri C-4 oxygen, nitric acid, chlorine in excess. Sensitized oxygen leads to 1.4 addition product 80, oxygen in benzene solution to 4.4 -peroxy phosphinic acid 68. With nitric acid, halogen in excess or autoxidation of 2-... 

At present, it is rather difficult to decide between these two formulae, but it seems certain that the substance contains methyleneamino groups N—CH2 and peroxy groups, —O—O—. This view is supported by the observation of T. Urban-ski and Szyc-Lewafiska [88] that the action of nitric acid on hexamethylenediamine in the presence of ammonium nitrate leads to the formation of cyclonite and formic acid. 

The main constraints on ARO at this time are highly concentrated, oxidative solutions like chromic acid, nitric acid and peroxy-sulfuric etchant. Their process rinses can be recovered and metals separated but, reconcentrating to near (40-70% of) bath strength, achievable with other solutions, shortens membrane life. WTI is working to develop membranes and operating procedures to improve system economies. Right now a life of 4-6 months is typical in most applications. 

The reactivity of nitric acid esters and in particular the complicated chemical composition of the products formed by their hydrolysis led some investigators [1, 37] to express the view that nitric esters may have the structure of peroxy-compounds (I) ... 

Periodates, 1 168 analysis of, 1 170 Periodic acid (EblOs), 1 172 solubility in nitric acid, 1 173 Peroxy compounds, of hafnium and zirconium, 3 72... 

Some unpublished and more recent work by these authprs examined the photoreduction of Pu(IV) in nitric acid solution that contained hydrazine. That reduction was shown to occur with or after the formation of a Pu(IV) peroxy complex. This complex is responsible for the enhanced rates of Pu(IV) reduction in dark periods following the photolysis. The photolysis of HNO3 in the presence of N2H produces H2O2, which then complexes with Pu(IV) it is known that H2O2 does not appear in the photolysis of pure HNO3 solutions, and its formation in the presence of N2Hi demonstrates some of the complex chemistry associated with N2H solutions. This may have useful application, because the peroxy complex of Pu(IV) is reduced at a faster rate with N2H than is the uncomplexed Pu ion. 

The temperature and density structure of the troposphere, along with the concentrations of major constituents, are well documented and altitude profiles have been measured over a wide range of seasons and latitudes for the minor species water, carbon dioxide, and ozone. A few profiles are available for carbon monoxide, nitrous oxide, methane, and molecular hydrogen, while only surface or low-altitude measurements have been made for nitric oxide, nitrogen dioxide, ammonia, sulfur dioxide, hydrogen sulfide, and nonmethane hydrocarbons. No direct measurements of nitric acid and formaldehyde are available, though indirect information does exist. The concentrations of a number of other important species, such as peroxides and oxy and peroxy radicals, have never been determined. Therefore, while considerable information concerning trace constituent concentrations is available, the picture is far from complete. 

Two principal exceptions are resin breakdown caused by sustained exposure to ionizing nuclear radiation and powerful chemical oxidizing agents such as nitric acid, chromic(VI) acid, chlorate(V) ions, halogens, and peroxy compounds. Even saturation levels of dissolved oxygen in the presence of transition metal cations may initiate chemical breakdown albeit only relatively slowly at ambient temperatures. 

Metal ions play a significant role in oxidative reactions as well as in biological dioxygen metabolism. Hydroperoxy coppo(ll) compound, graerated fivm coppeifll) acetate and hydrogen peroxi, is obtainable from copper(II) nitrate and hydrogen peroxide (Eqn. 1). The ensuing nitric acid in this reaction requires neutralization by a base to maintain a pH 5. 

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