Decomposition of nitric oxide

T.M. Giir, and R.A. Huggins, Decomposition of Nitric Oxide on Zirconia in a Solid-state electrochemical cell, J. Electrochem. Soc. 126(6), 1067-1075 (1979). 

Y. Matsumoto, T. Onishi, and K. Tamam, Effects of Sulphur on a Palladium Surface on the Adsorption of Carbon Monoxide and the Adsorption and decomposition of nitric oxide, J.C.S. Faraday I 76, 1116-1121 (1980). 

Kieken LD, Neurock M, Mei DH. 2005. Screening by kinetic Monte Carlo simulation of Pt-Au(lOO) surfaces for the steady-state decomposition of nitric oxide in excess dioxygen. J Phys Chem B 109 2234-2244. 

Iwamoto, M., Yokoo, S., Sakai, K. el al. (1981) Catalytic decomposition of nitric oxide over copper(II)-exchanged Y-type zeolites, J. Chem. Soc. Faraday Trans., 77, 1629. 

Tajima, N., Hashimoto, M., Toyama, F. et al. (1999) A theoretical study on the catalysis of Cu-exchanged zeolite for the decomposition of nitric oxide, Phys. Chem. Chem. Phys., 1, 3823. 

Aryafar, M. and Zaera, F. (1998) Isothermal kinetic study of the decomposition of nitric oxide over Rh(lll) surfaces , J. Catal., 175, 316. 

Because of its relevance to the chemistry of air at elevated temperatures the homogeneous decomposition of nitric oxide has received considerable attention from gas kineticists. References to early studies are given in the more recent work discussed below. The mechanisms for the decomposition and for the reverse reaction, the formation of NO from air, are well established and good quantitative data (Table 12) are available for the rate coefficients of the elementary steps. 

The decomposition of nitric oxide in oxygenated perfused organ baths is commonly assumed to occur by the third-order reaction of... 

The Thermal Decomposition of Nitric Oxide and the Union of Nitrogen and Oxygen to Nitric Oxide. 

The decomposition of nitric oxide at the surface of a hot platinum wire was found by Hinshelwood and Green to be apparently of the first order, from experiments on variation of the initial pressure. Retardation by oxygen was observed, but was not at first considered marked enough to have reduced the order from two to one. Further investigation by Bachmann and Taylor f shows that the oxygen retardation is very considerable and that therefore we have here an example of the reduction of the true order two to an apparent order of one. 

Kaufman and Decker247 investigated the thermal decomposition of nitric oxide in the temperature range 1378-1690°K. They determined the ratio of kig to the rate constant ksi of the reaction... 

In Part II (Sections 7-10) are described experiments on the decomposition of nitric oxide which was added to the explosive mixture in advance. These experiments establish a proportionality between the rate of decomposition and the square of the concentration of nitric oxide and give the heats of activation for the formation and decomposition of nitric oxide. The similarity theory and the exact mathematical theory of a reversible bimolecular... 

With the exception of the mixtures with a high hydrogen content, 32% and higher, in which heating decreases and cooling increases the yield of nitric oxide. In these mixtures, as will be shown below, fundamental importance attaches to the decomposition of nitric oxide as the explosion products cool off from the temperature of the explosion to that of the vessel. 

The hypothesis of the thermal nature of the oxidation of nitrogen leads to definite conclusions as to the relation between the formation and decomposition of nitric oxide in an explosion and the equilibrium concentration of nitric oxide at the explosion temperature. The equilibrium concentration may be computed independently from thermochemical data. The first task confronting us was to check up on these relations. 

It can be assumed that in the series of experiments with the same initial pressure p0 in vessels of the same dimensions the reaction time r will be the same and will depend on the cooling rate. Experiments which are confined to an analysis of the final nitric oxide content in the explosion products can only yield in principle the product of the rate constant into the time hr, but not each of these quantities separately. By studying the dependence of kr on the explosion temperature one can also find the temperature dependence of the activation heat of the reaction. In Fig. 13 log kr is plotted as a function of 1 /Tm. In each series with constant summary content of the mixture kr was calculated by utilizing the data on the formation of nitric oxide, NO0 = 0 (circles in Fig. 13) and on the decomposition of nitric oxide NO0 = 7 or 10 mm and is 2-5 times greater than NO (triangles in Fig. 13). 9... 

According to these data the heat of activation for the decomposition of nitric oxide, to which reaction the factor k refers, is A = 82 10 kcal/mole.10 It should be especially noted that there is no systematic divergence between the data on the formation and on the decomposition of nitric oxide this fact justifies the assumption that the rate of decomposition is directly proportional to the square of the nitric oxide concentration.11 The investigation covered the temperature range from 2000°K to 2900°K in which the rate varies by a factor of 300. As appears from Fig. 13, except for the scattering due to the inevitable errors of the experiments and computations, the points actually do fall on a straight line in the coordinates lg kr, 1/Tm, i.e., the Arrhenius temperature dependence of the reaction rate holds. The thermodynamic relation between the rates of the direct and reverse reactions permits determining the heat of activation A for the formation of nitric... 

It should be recalled that k is the rate coefficient for the formation and k for the decomposition of nitric oxide. Thus, the reaction time r of formula (9.10) is the time in which the rate of the direct reaction of formation of nitric oxide decreases by a factor e. 

The problem is easily solved for small fcm[NO]r. In this case NO/[NO] is also small, and neglecting the square of this quantity in the brackets, i.e., neglecting the decomposition of nitric oxide, we find... 

A comparison of the experimental data with the computations (the curves of Figs. 14 and 15, and the data on the decomposition of nitric oxide) shows a general qualitative agreement of experiment with the theory as regards both the form of the relationships and the numerical value of the maximum yield (experimental 0.65-0.68, computed 0.65). At the same time there are... 

The difference as compared with the former theory consists in that a more complex meaning is now attributed to k, the constant of the bimolecular reaction of decomposition of nitric oxide... 

The experiments which we used to determine the rate coefficient of the reactions of formation and decomposition of nitric oxide referred to an oxygen concentration which varied within comparatively narrow limits near 150 mm 02 at 17°C. Substituting in place of the old expression for the rate coefficient... 

The decomposition of nitric oxide pre-mixed with the explosive mixture is investigated. The heats of activation for the formation and decomposition of nitric oxide are determined. 

Melia, T. P. Decomposition of nitric oxide at elevated pressures. J. Inorg. Nucl. 

The first estimate of kinetic parameters for the thermal decomposition of nitric oxide were made by Zeldovich and Frank-Kamenetsky . From a study of nitric oxide formation in H2-O2-N2 flames these workers proposed a value of 82+10 kcal. mole for the activation energy of decomposition. Vetter studied the reaction over the temperature range 1200-1900 K. He found a small rate increase on addition of oxygen and postulated a chain process involving the reactions... 

Yuan et studied the decomposition of nitric oxide in packed Alundum vessels using chemical and photometric analysis to estimate the kinetics, they found the reaction to be homogeneous and second order above 1100 °C with an activation energy of 63.1 kcal.mole , which is in excellent agreement with that found by Kaufman et al. 

Reaction (64) is 32.1 kcal.mole endothermic and does not take place near room temperature. Kaufman and Decker determined from kinetic data on the thermal decomposition of nitric oxide in the presence of excess O2. For the temperature range 1500-1700 °K they obtained the expression... 

S. Pancharatnam, R.A. Huggins, and D.M. Mason, Catalytic decomposition of nitric oxide on zirconia by electrolytic removal of oxygen, J. Electrochem. Soc. 722 869 (1975). 

PllC-1 The decomposition of nitric oxide on a heated platinum wire is discussed in Chem. Eng. ScL, 30, 781 (1975). After making some assumptions about the density and the temperatures of the wire and atmosphere, and using a correlation for convective heat transfer, determine if mass transfer limitations are a problem in this reaction. 

If special conditions are required for a reaction to take place, such as the presence of a catalyst, the conditions or the catalyst can be written above or below the arrow. Platinum metal catalyzes (speeds up) the decomposition of nitric oxide to its constituent elements in catalytic converters. 

Catalytic activity of perovskite-type oxides for the direct decomposition of nitric oxide b... 

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