Second-stage decomposition

This second-stage decomposition reaction (carbonate hydrolysis) proceeds to approximately 80% completion at 150 psig, producing hydroxide alkalinity and carbon dioxide and providing a further 0.35 ppm carbon dioxide (80% of 0.44 ppm). Consequently, the total production of carbon dioxide from 1 ppm of bicarbonate alkalinity is 0.79 ppm at 150 psig. 

The mass loss of the first-stage decomposition of the AP particles with 10% LiF is 56.7 %, and that of the second-stage decomposition is 28.5 %. The residue remaining above 790 K is 14.8%. As shown in Fig. 7.26, the two-stage decomposition process can be summarized as follows [i5]... 

The urea-product solution, leaving the first decomposition stage and still containing some unreacted carbamate and excess NH3, is let down in pressure and steam heated in the second-staged decomposition section, which operates at about 2 atm and 120°C. Practically all of the residual carbamate is decomposed and stripped from the urea-product solution together with the residual excess ammonia. The 74—75 wt % urea solution thus obtained is further processed to solid urea... 

The cases of pentamethylbenzene and anthracene reacting with nitronium tetrafluoroborate in sulpholan were mentioned above. Each compound forms a stable intermediate very rapidly, and the intermediate then decomposes slowly. It seems that here we have cases where the first stage of the two-step process is very rapid (reaction may even be occurring upon encounter), but the second stages are slow either because of steric factors or because of the feeble basicity of the solvent. The course of the subsequent slow decomposition of the intermediate from pentamethylbenzene is not yet fully understood, but it gives only a poor yield of pentamethylnitrobenzene. The intermediate from anthracene decomposes at a measurable speed to 9-nitroanthracene and the observations are compatible with a two-step mechanism in which k i k E and i[N02" ] > / i. There is a kinetic isotope effect (table 6.1), its value for the reaction in acetonitrile being near to the... 

At the second stage the decomposition of metal alkyl takes place. Metal alkyl is liable to decompose into metal alkyl and olefin causing the increased saturation of polyethylene macromolecules ... 

Tandem mass spectrometry (MS-MS) is a term which covers a number of techniqnes in which one stage of mass spectrometry, not necessarily the first, is used to isolate an ion of interest and a second stage is then nsed to probe the relationship of this ion with others from which it may have been generated or which it may generate on decomposition. The two stages of mass spectrometry are related in specific ways in order to provide the desired analytical information. There are a large nnmber of different MS-MS experiments that can be carried ont [9, 10] bnt the fonr most widely nsed are (i) the prodnct-ion scan, (ii) the precnrsor-ion scan, (iii) the constant-nentral-loss scan, and (iv) selected decomposition monitoring. 

The mechanoradical produced will react with the small amount of oxygen to form hydroperoxides these are subsequently utilised as radical generators in the second stage. The resulting hydroxyl radical (from hydroperoxide decomposition) abstracts a hydrogen from the substrate to form macroradical which, in turn, will react with more of the thiyl radical to form more bound antioxidant. The polymer bound antioxidant made in this way is very much more resistant to solvent leaching and volatilisation when compared to commercial additives (13). see Figure 2. 

Second stage ignition during oxidation/combustion of iodomethane in oxygen at 300-500°C was particularly violent, occasionally causing fracture of the apparatus, and was attributed to formation and decomposition of a periodic species. 

Basically, there are two different ways to decompose a 2S-MILP (see Figure 9.10). The scenario decomposition separates the 2S-MILP by the constraints associated to a scenario, whereas the stage decomposition separates the variables into first-stage and second-stage decisions. For both approaches, the resulting subproblems are MILPs which can be solved by standard optimization software. 

Surface catalysis affects the kinetics of the process as well. Saltzman et al. (1974) note that in the case of Ca -kaolinite, parathion decomposition proceeds in two stages with different first-order rates (Fig. 16.14). In the first stage, parathion molecules specifically adsorbed on the saturating cation are quickly hydrolyzed by contact with the dissociated hydration water molecules. In the second stage, parathion molecules that might have been initially bound to the clay surface by different mechanisms are very slowly hydrolyzed, as they reach active sites with a proper orientation. 

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