Butane reaction profile

Table 17.9 The reaction profile of butane over solid acids mixed with Pt/Zr02...

Well head pressures increased when injection was stopped at Well No. 1 for more than 24 h, apparently caused by a combination of precipitation reactions and backflow of sand. Injecting a slug of brine after every period of interrupted flow solved this problem. Movement of the main organic constituents (n-hexylamine, butanal, butanol, and phenol) was assumed to be slowed by adsorption. This conclusion was based on laboratory adsorption experiments by involving a different geologic formation (Cottage Grove sandstone) no direct observations were made of the injected waste. For current hazardous waste injection wells in Texas, the reader can refer to Texas Environmental Profiles web site for on-line resources for the State of Texas.185... 

In the rhodium- and platinum-catalysed reactions [167], it is of significant interest that the 7V-profiles calculated from the distributions of deuterium in the n-butane (Table 30) appear to bear no clear relationship to the 7V-profiles of the n-butenes formed simultaneously. This observation has been interpreted as indicating that either the butene which undergoes further hydrogenation never desorbs as butene, or that the sites responsi-... 

Figure 3 shows a profile of the potential surface of the consecutive stages of (I). Let k be the rate constant of the reaction. Then, in conformity with the results obtained, km. It is clear, however, that the level 4 of the adsorbed butylene in the process of dehydrogenation of butane is the same as the level 6 of the butylene in the dehydrogenation of the latter. Hence, km = ka and consequently km km. Thus, in dehydrogenation the desorption rate constant of the initial substance is considerably larger than that of its dehydrogenation. 

Air and n-butane are introduced into a fluid-bed, catalytic reactor (1). The fluid-bed reactor provides a uniform temperature profile for optimum catalyst performance. Reaction gases are cooled and filtered to remove small entrained catalyst particles and then routed to the recovery section. Reactor effluent is contacted with water in a scrubber (2), where essentially 100% of the reactor-made maleic anhydride is recovered as maleic acid. The process has the capability of co-producing maleic anhydride (MAH) with the addition of the appropriate purification equipment. Scrubber overhead gases are sent to an incinerator for safe disposal. 

Air and n-butane are introduced into a fluid-bed, catalytic reactor (1). The fluid-bed reactor provides a uniform temperature profile for optimum catalyst performance. Reaction gases are cooled and fil-... 

The reactors for the basic propane and n-butane pyrolysis were of monolithic annular quartz construction (Type I reactor). The reaction space was kept virtually isothermal by a surrounding bath of Ottawa sand fluidized vigorously by a stream of nitrogen. Temperature profiles were measured by calibrated Pt-Rh couples in a central thermowell. A description of this type of reactor has been given elsewhere (6). 

Following this study, Wilk et al. [230] simulated the composition-time profiles for selected alkenes and oxygenated products that were formed from n-butane and i-butane combustion, and also mixtures of these fuels, in a motored engine. An engine cycle was simulated within a spatially uniform zone of varying volume. The volume history was specified in such a way that the predicted pressure history matched the measured polytropic pressure history in non-reactive conditions. Composition profiles were compared with those measured experimentally. Some of the kinetic features that distinguish the reactivities of the two fuels and their modes of reaction involving alkylperoxy and dialkylperoxy radicals were elucidated in this work. The n-butane oxidation model had also been applied to the... 

In order to compare the nature of the carbon deposits on Pc and Pt-Sn catalysts, carbon deposition on three catalysts with different Sn/Pt ratio was carried out in the in situ reaction and TPO system for n-butane dehydrogenation and successive temperature programmed oxidation. The areas of Peaks 1 and 2 of the TPO profiles of the three catalysts after carbon deposition were resolved and detemnined by an integraph. The ratios of areas of Peak 1 to Peak 2 of the TPO profiles were calculated and ploued against the Sn/Pt ratio in Fig. 4. Becanse the addition of Sn can inhibit the cart)on deposition on metallic surfaces, the proportion of Peak 1 to Peak 2 decreases with the increasing of Sn/Pt ratio These results imply that the ratio of carbon deposits on metal surfaces to total carbon deposits decreases with the incorporation of tin. 

Reaction time influenced the odorant profile. The SPME-GC-MS data revealed significant differences for some compounds previously described as ham odorants (Figure 2) The largest values appeared in the 14-days group, and after that a significant decrease was found. This tendency was also found in other odorants (heptanal, oct-(E)-2-enal, butane-2,3-dione) but was not significant. 

Abstract This chapter emphasises on the important aspects of steric and stereo-electronic effects and their control on the conformational and reactivity profiles. The conformational effects in ethane, butane, cyclohexane, variously substituted cyclohexanes, and cis- and tra/ ,v-decalin systems allow a thorough understanding. Application of these effects to E2 and ElcB reactions followed by anomeric effect and mutarotation is discussed. The conformational effects in acetal-forming processes and their reactivity profile, carbonyl oxygen exchange in esters, and hydrolysis of orthoesters have been discussed. The application of anomeric effect in 1,4-elimination reactions, including the preservation of the geometry of the newly created double bond, is elaborated. Finally, a brief discussion on the conformational profile of thioacetals and azaacetals is presented. 

Here Lc and Me value are combination of constants. Adsorption constants represent adsorption of crotonaldehyde via the olefinic bond (Kab), via the carbonyl bond (Kac) and via both bonds (Kabc)> while kc, ks and kco rate constants of crotonaldehyde hydrogenation to crotyl alcohol and butanal and of cro-tyl alcohol to butanol. Analysis of the equation (3) reveals that the initial selectivity (at low conversions) depends on the Lc value. Selectivity profile as a function of conversion depends more on the Me value. For parallel-consecutive reactions the lower value of Me, the less pronounced is the crotyl alcohol selectivity dependence on the conversion. 

In conclusion the dehydrogenation of butane has been studied over a Pt/alumina catalyst under continuous flow conditions. The system is operating at equilibrium in terms of total butene yield, however the 1-butene is does not undergo fast equilibration with the 2-butenes. The 2-butenes are usually in thermodynamic equilibrium. Analysis of the deactivation profiles of the butenes confirms that the carbon deposition reaction takes place on different sites for 1-butene and the 2-butenes. 

Kinetic studies of the reaction between the a-nucleophile, butane-2-3-dione oximate (Ox ), and p-nitrophenyl thionobenzoate (18) in DMSO-H2O mixtures of varying compositions at 298,308, and 318 K revealed that, based on a comparison of rates of reaction with a normal nucleophile, p-chlorophenoxide, the a-effect showed a bell-shaped profile, the maximum value occurring at 50% DMSO at all temperatures, but decreasing as the temperature increased. Dissection of the activation parameters, A7/ and revealed that the bell-shaped a-effect behaviour is due to entropy of activation differences rather than enthalpy terms, although the enthalpy term controls almost entirely the solvent-dependent dramatic increase in reaction rate (about 2000-fold greater in 80% DMSO than in H2O). Differences in the TS structures for the reactions with Ox ... 

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