Nitrogen tetroxide decomposition

Figure 1.11 Standard heat of reaction and equilibrium constant for nitrogen tetroxide decomposition. [After S.I. Sandler, Chemical and Engineering Thermodynamics, reprinted by permission of John Wiley and Sons, New York, NY (1989).]...

Nitrogen tetroxide also causes rapid racemization of sulfoxides however, the reaction takes place without decomposition (279,280). This process is initiated by the formation of a sulfonium salt, which then undergoes partial ionization to form a dication intermediate. 

A study of the kinetics of the decomposition of ammonium perchlorate has been made by Bircumshaw and Newman [5]. The gaseous products, up to a temperature of 300°C, were found to be oxygen, chlorine, chlorine dioxide, nitrous oxide, nitrogen tetroxide, chlorine dioxide, hydrochloric acid, perchloric acid and water. The total volume of oxygen and nitrogen produced by unit weight of the solid showed practically no variation up to about 300°C. 

Other processes for making chlorine include sodium manufacture, caustic potash manufacture, hydrogen chloride decomposition, the nitro-syl chloride (NOC1) process, and a process where salt is treated with nitric acid to form sodium nitrate and chlorine with nitrosyl chloride (containing 4 to 10% nitrogen tetroxide) as a by-product. The nitrosyl chloride vapor is placed in contact with oxygen to produce nitrogen tetroxide and chlorine ... 

Greater than equilibrium concentrations of intermediate species have been observed in the combustion products of several reactant systems. Examples are the concentrations of ammonia in the products of the decomposition of hydrazine (32), the concentration of CH4 in ethylene oxide decomposition (33), nitric oxide and ammonia in the products of the reaction of hydrazine and nitrogen tetroxide (34), and chlorine monofluoride in the products of the reaction of hydrazine and chlorine pentafluorlde (35). 

In liquid nitrogen tetroxide the decomposition is about twice as rapid as in the gas phase where vacuum may be considered as the solvent. In nitromethane the decomposition is slightly slower than in the gas phase. Other solvents, as widely different as liquid bromine and carbon tetrachloride, give values which are only slightly greater than those in the gas phase. 

The interpretation of Fig. 28 is now apparent. At 4,050 A N20 and N2O5 do not absorb, and the molecules of nitrogen dioxide decomposed per photon absorbed is practically independent of the amount of decomposition products. But at the other two lines, 3,660 and 3,130 A, nitrogen tetroxide absorbs light as well as nitrogen dioxide however the light which it absorbs does not produce any permanent chemical change. 

Explosive reaction with sodium -I-methanol or sodium methoxide + methanol. Mixtures with sodium or potassium are impact-sensitive explosives. Reacts violently with acetone + alkah (e.g., sodium hydroxide, potassium hydroxide, or calcium hydroxide), Al, disilane, Li, Mg, methanol + alkah, nitrogen tetroxide, perchloric acid + phosphorus pentoxide, potassium-tert-butoxide, sodium methylate, NaK. Incompatible with dinitrogen tetraoxide, fluorine, metals, or trhsopropylphosphine. Nonflammable. When heated to decomposition it emits toxic fumes of CT. 

Incompatible with dinitrogen tetraoxide, 2,4-dinitrophenyl disulfide, potassium, potassium hydroxide, nitrogen tetroxide, sodium, sodium potassium alloy. Mutation data reported. When heated to decomposition it emits very toxic fumes of... 

P3-14b Reconsider the decomposition of nitrogen tetroxide discussed in Example 3-8. The reaction is to be Carried out in PER and aiso in a constant-volume batch reactor at 2 atm and 340 K. Only Nj04 and an inert I are to be fed to the reactors, Plot the equilibrium conversion as a function of inert mole fraction in the feed for both a constant-volume batch reactor and a plug Sow reactor, Why is the equilibrium conve ton lower for the batch system than the flow system in Example 3-87 Will this lower equilibrium conversion result always be the case for batch systems ... 

The reversible gas-phase decomposition of nitrogen tetroxide, N2O4, to nitrogen dioxide, NO,... 

Calculate the equilibrium mole fractions for the decomposition of nitrogen tetroxide as a result of the reaction N2O4 (g) = 2 NO2 (g) at 25°C and 1 bar. Assume the components form an ideal-gas mixture. Initially there is only 1 mol of N2O4. 

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