Nitrous oxide, thermal decomposition

Johnston H S 1951 Interpretation of the data on the thermal decomposition of nitrous oxide J. Chem. Phys. 19 663-7... 

Nitrous oxide may also be obtained by the controlled reduction of nitrates or nitrites, decomposition of hyponitrites, or thermal decomposition of hydroxylamine. 

Nitrous oxide can be made by the careful thermal decomposition of molten NH4NO3 at about 250°C ... 

PCSs obtained by dehydrochlorination of poly(2-dilorovinyl methyl ketones) catalyze the processes of oxidation and dehydrogenation of alcohols, and the toluene oxidation207. The products of the thermal transformation of PAN are also catalysts for the decomposition of nitrous oxide, for the dehydrogenation of alcohols and cyclohexene274, and for the cis-tnms isomerization of olefins275. Catalytic activity in the decomposition reactions of hydrazine, formic acid, and hydrogen peroxide is also manifested by the products of FVC dehydrochlorination... 

Thermal Decomposition. The therm decompn was studied betw 380 and 430° and found to be homogeneous and apparently 1st order. The products were complex and included nitric oxide, methane, carbon monoxide, and w plus small amts of ethane, ethylene, and nitrous oxide (Ref 23)... 

Hinshelwood and Burk [Proc. Roy. Soc., 106A (284), 1924] have studied the thermal decomposition of nitrous oxide. Consider the following adjusted data at 1030 °K. 

Data for the thermal decomposition of nitrous oxide on gold at 900°C and an initial pressure of 200 Torr are tabulated. Check the order of the reaction. 

Find the rate equation for the thermal decomposition of nitrous oxide in... 

Nitrous Oxide Nitrous oxide (1.1.11) is synthesized either by the thermal decomposition of ammonium nitrate, or by the oxidation of sulfamic acid by nitric acid [9-11]. 

Thermal decomposition occurs at 170°C producing nitrous oxide and water ... 

Nitric oxide is commercially produced by the catalytic oxidation of ammonia using a platinum catalyst 4NH3(g) + 50 —> 4NO(g) + 6H20(g). Nitrous oxide is produced by the thermal decomposition of ammonium nitrate at approximately 240°C NH4N03(g) —> N O + 2H . ... 

In the metal-catalyzed decomposition of nitrous oxide—corresponding to this conception—not the liberated 0 atom [C. Wagner (10)], but the N2O molecule receives electrons on adsorption (8,9,58). As the metal surface thereby loses electrons, it is to be expected that an increase of the work function will occur upon adsorption of N2O molecules, e.g., on platinum, even at such low temperatures that the thermal decomposition of N2O does not occur. 

According to this work the catalytic decomposition of nitrous oxide molecules proceeds in the following way a N2O molecule adsorbed by the catalyst binds metal electrons, and thus the bond between the 0 atom and N2 in the molecule is loosened, and N2 is thermally dissociated from O at sufficiently high temperature. The 0 atom is held to the surface through the influence of the metal electrons. It can combine with a neighboring... 

The use of ethyl nitrate as a component of rocket fuel involves the problem of thermal decomposition. Levy [16] has studied the decomposition of ethyl nitrate in the gaseous phase, in the temperature range 161 and 201°C under a pressure of a few centimeters of mercury. He found that ethyl nitrite is the main decomposition product. By-products include methyl nitrite, nitromethane, nitrogen dioxide and nitrous oxide. 

Spinel oxides with a general formula AB2O4 (i.e. the so-called normal spinels) are important materials in industrial catalysis. They are thermally stable and maintain enhanced and sustained activities for a variety of industrially important reactions including decomposition of nitrous oxide [1], oxidation and dehydrogenation of hydrocarbons [2], low temperature methanol synthesis [3], oxidation of carbon monoxide and hydrocarbon [4], and oxidative dehydrogenation of butanes [5]. A major problem in the applications of this class of compound as catalyst, however, lies in their usually low specific surface area [6]. 

Arsenic is oxidised, mainly to arsenious oxide, when heated in nitrous oxide 8 the reaction becomes appreciable at 250° to 270° C. and ignition occurs at 400° to 450° C. This reaction takes place specifically between arsenic and the nitrous oxide and is not due to reaction with oxygen after thermal decomposition of the nitrous oxide, as such decomposition does not occur below 400° C. and is very slight at 460° C. Nor does the reaction resemble that which occurs in oxygen, except that, like the reaction in the dark with the latter gas (see p. 47), it is a surface reaction. No chemi-luminescence is observed, however, and there is no upper critical oxidation pressure. At 360° C. the product contains at least 99 per cent, of pure arsenious oxide, and at 420° C. it contains about 5-8 per cent, of arsenic pentoxide. 

Vanpee (62) has studied the explosion of formaldehyde-oxygen mixtures. The dependence of explosion pressure upon temperature, vessel diameter, and the addition of inert diluent is in agreement with the thermal theory and consistent with studies of the slow reactions (54, 61). Typical of other reactions which have been reported to exhibit thermal explosion limits are the decomposition of nitrous oxide (75), the reaction between nitrous oxide and hydrogen (38), and cyanogen-air (32). 

For the sake of comparison, let us briefly consider the commonly known method of nitrous oxide synthesis [169] by thermal decomposition of ammonia nitrate at 523-533 K by the following reaction ... 

When the rate equation does not correspond stoichiometrically, the reaction is called a nonelementary reaction. Consider the thermal decomposition of nitrous oxide to nitrogen and oxygen as follows ... 

The primary commercial method for producing nitrous oxide is by thermal decomposition of ammonium nitrate, with nitrous oxide and water in the primary reaction ... 

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