ChemInform Abstract: Production of Nitrogen Oxides on Platinum and Nickel from Atomic Nitrogen and Molecular Oxygen.

ChemInform ◽  
2010 ◽  
Vol 25 (22) ◽  
pp. no-no
Author(s):  
M. E. RYSKIN ◽  
S. V. SYROMIATNIKOV
Keyword(s):  
Nitrogen Oxides ◽  
Molecular Oxygen ◽  
Atomic Nitrogen

Determination of atomic nitrogen concentrations using titration with molecular oxygen

2005 ◽  
Vol 413 (4-6) ◽  
pp. 468-472 ◽  
Author(s):  
M. Ganciu ◽  
J. Orphal ◽  
A.-M. Pointu ◽  
M. Vervloet
Keyword(s):  
Molecular Oxygen ◽  
Atomic Nitrogen ◽  
Nitrogen Concentrations

The chemistry of the stratosphere

1980 ◽  
Vol 296 (1418) ◽  
pp. 149-160 ◽  
Keyword(s):  
Nitrogen Oxides ◽  
Molecular Oxygen ◽  
Chemical Reactions ◽  
Atomic Oxygen ◽  
Reaction Products ◽  
Simultaneous Measurements ◽  
Trace Species ◽  
Hydrogen Radicals ◽  
Catalytic Cycles ◽  
Odd Oxygen

The chemistry of the stratosphere is dominated by the processes that remove the ‘odd oxygen' (atomic oxygen and ozone) generated by the photolysis of molecular oxygen. In recent years it has been established that the Chapm an reaction, O+O 3 = O 2 + O 2, cannot account for all the observed destruction of odd oxygen. Catalytic cycles involving nitrogen oxides (NO, NO 2 ), hydrogen radicals (H, HO , HO 2 ) and chlorine species (Cl, CIO) have been shown to be im portant and it is now realized that these catalytic cycles are closely linked to each other. Measurements of these trace species, their precursors (e.g. N 2 O , H 2 O , CH 4 ) and their reaction products (e.g. HNO 3 , HCL) in the stratosphere are essential to understanding its chemistry. The natural variability of the stratosphere places a premium on simultaneous measurements of those trace species that are interconverted by rapid chemical reactions.

Kinetics of the reaction between atomic nitrogen and molecular oxygen in the ground ( 3 ∑ - g ) and first excited ( 1 ∆ g ) states

1970 ◽  
Vol 316 (1527) ◽  
pp. 539-550 ◽  
Keyword(s):  
Nitric Oxide ◽  
Molecular Oxygen ◽  
Rate Constants ◽  
Room Temperature ◽  
Atomic Nitrogen ◽  
D Region ◽  
Exponential Factors ◽  
The Difference ◽  
Kinetics Of ◽  
Arrhenius Expression

Rate constants for the reaction N + O 2 ( 1 ∆ g ) → k 1 NO + O (1) have been measured at four temperatures, and fitted to an Arrhenius expression, k 1 = A exp ( ─ E a / RT ). The results indicate that A ≤ 2 x 10 -14 molecule -1 cm 3 s -1 and < 1.2 kcal (5.0 kJ ) mol -1 : at room temperature (300 K ), k 1 = 2.7 ± 1.0 x 10 -15 molecule -1 cm 3 s -1 . Reaction (1) cannot, therefore, proceed fast enough at 200 K for it to be an important source of nitric oxide in the atmospheric D-region. The rate constant for the reaction N + O 2 ( 3 ∑ ─ g ) → k 2 NO + O (2) has been measured at 302 K to be 1.08 ± 0.10 x 10 -16 molecule -1 cm 3 s -1 . This value, taken together with the data of earlier workers, suggests that k 2 = 1.5 x 10 -11 exp (—7.1/ RT ) molecule -1 cm 2 s -1 . A possible explanation for the difference in pre-exponential factors for reactions (1) and (2) is presented.

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