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ammonium nitrite
The simulated results from the modified inhibition model expressed by FA and ammonium/nitrite concentrations were shown very similar to the experimental results.
      
Secondary aerosols or particulates, such as ammonium nitrate or ammonium nitrite, might have been important constituents of the PM2.5 at the residential site.
      
From these products, it is concluded that the reaction of NO2 with NH4Cl is a reverse disproportionation reaction where two moles of NO2 result in ammonium nitrite, NH4NO2, as an intermediate, and nitryl chloride, NO2Cl.
      
Exposing Fe/MFI first to NH3 then to flowing NO + O2 or using the reversed sequence, invariably leads to the formation of ammonium nitrite, NH4NO2.
      
In the first set, part of the NOx is reduced to NH3; in the second set ammonium nitrite, NH4NO2 is formed from this NH3 and NO + NO2.
      
Upon applying Redhead's equations for a first order desorption to the decomposition of ammonium nitrite, an activation energiy of 22.4 is calculated which is consistent with literature data.
      
For the reaction path via ammonium nitrite a consumption ratio of 1/1 for NO and NO2 is predicted and confirmed experimentally by injecting NO into a mixture of NH3 + NO2 flowing over a BaNa/Y catalyst.
      
Contact of adsorbed ammonium nitrite, NH4NO2, with HCl vapor or a solid acid such as the zeolite HY, significantly lowers the temperature of its decomposition to N2?+?H2O.
      
The decomposition of ammonium nitrite is one of the steps in the catalytic reduction of NOx with ammonia or other reductants.
      
The decomposition of ammonium nitrite in water creates a supersaturated solution of nitrogen.
      
Solvent and deuterium isotope effects on the decomposition of ammonium nitrite solutions
      
The process of decomposition, to nitrogen and water, of ammonium nitrite formed, competes with the formation of NO2- which is, otherwise, proportional to the radiation absorbed.
      
 

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