Nitric oxide reaction with chlorine 747 reduced

AZOTE (French) (10102-44-0) A powerful oxidizer. Reacts with water, forming nitric acid and oxygen. Violent reaction with strong reducing agents, anhydrous ammonia, alcohols, chlorinated hydrocarbons, cyclohexane, ethers, fluorine, formaldehyde, fuels, nitrobenzene, oxygen difluoride, petroleum, sodium, toluene. Incompatible with combustible materials, red phosphorus, petroleum products. Forms explosive material with propylene. Vapor reacts violently with phospham. Attacks many metals in the presence of moisture. 

In order to calculate the steady-state concentration of ozone in the stratosphere, we need to balance the rate of production of odd oxygen with its rate of destruction. Chapman originally thought that the destruction was due to the reaction O + 03 —> 2O2, but we now know that this pathway is a minor sink compared to the catalytic destruction of 03 by the trace species OH, NO, and Cl. The former two of these are natural constituents of the atmosphere, formed primarily in the photodissociation of water or nitric oxide, respectively. The Cl atoms are produced as the result of manmade chlorofluorocarbons, which are photodissociated by sunlight in the stratosphere to produce free chlorine atoms. It was Rowland and Molina who proposed in 1974 that the reactions Cl + 03 —> CIO + O2 followed by CIO + O —> Cl + O2 could act to reduce the concentration of stratospheric ozone.10 The net result of ah of these catalytic reactions is 2O3 — 3O2. 

Formation of C02 from C1C(0)02 may also occur by reaction with atomic oxygen (equation 85) or chlorine (equation 86). Furthermore, the chloroformylperoxy radical is reduced by nitric oxide (equation 87), like its fluorine analogue. However, the resulting chloroformyloxy radical C1C(0)0 is very unstable, and the exothermicity of reaction 87 would cause dissociation (equation 88) into C02 and atomic Cl. 

Proteins, due to the complexity of their chemical structures, undergo oxidative modifications in subsequent stages which depend both on the presence of oxidation-susceptible groups and on steric availability of these groups for oxidant attacks (S25). Some oxidative structural modifications produced in proteins are common in various oxidants. Some modifications, such as chlorinated and nitrated protein derivatives produced in reactions with hypochlorite, peroxynitrite, and nitric dioxide, are specific for the oxidants employed. Certain oxidative protein modifications, such as interchain or intrachain disulfide bond formation or thiolation, are reversible and may be reduced back to the protein native form when oxidative stress is over (Dl). Other changes, such as sulfone formation, chlorination, and nitration, are irreversible and effect protein denaturation and promote its subsequent degradation. 

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