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  • 101
    Electronic Resource
    Electronic Resource
    Chichester : Wiley-Blackwell
    Journal of Physical Organic Chemistry 4 (1991), S. 225-232 
    ISSN: 0894-3230
    Keywords: Organic Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology , Physics
    Notes: Equilibrium displacements within the enol-enthiolic tautomeric systems of β-thioxoketones caused by long-range isotope effects were monitored by 1H and 13C NMR spectroscopy. Thioacetylacetone and 1,3-diphenyl-3-thioxopropanone deuteriated at various positions were investigated. Both compounds are in fast (Z)-enol-(Z)-enethiol equilibrium on the NMR time scale. The investigations showed that CD3 and C6D5 groups changes the equilibrium so that the tautomer having a C = X bond next to the CD3 or C6D5 groups decreases. Deuteriation at the methine position pushes the equilibrium towards the (Z)-enol form. The study further showed that deuteriation at the phenyl ring next to the C = O group causes the largest effect if the deuterium is at the ortho position and the smallest if it is at the para position. Long-range effects on equilibrium are discussed in general in order to establish a common pattern. Deuterium scrambling is observed both during the coupling reaction of ethyl thionoacetate with hexadeuterioacetone and during preparation of specifically labelled acetophenone. The latter compounds are synthesized by acetylation of specifically labelled benzenes. The scrambling reaction is suggested to be a transdeuteriation of the deuteriated benzenes rather than involving the acetophenones.
    Additional Material: 2 Ill.
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  • 102
    Electronic Resource
    Electronic Resource
    Chichester : Wiley-Blackwell
    Journal of Physical Organic Chemistry 4 (1991), S. 260-262 
    ISSN: 0894-3230
    Keywords: Organic Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology , Physics
    Notes: Oxygen-17 NMR spectra of some N-nitrosamines are discussed in terms of steric and conjugative effects. Relationships have been observed between rotational barriers, conformations and 17O chemical shifts. A tentative linear correlation has been determined between repulsive Van der Waals interactions and some N-nitrosopiperidines.
    Additional Material: 2 Tab.
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  • 103
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    Electronic Resource
    Chichester : Wiley-Blackwell
    Journal of Physical Organic Chemistry 4 (1991), S. 277-284 
    ISSN: 0894-3230
    Keywords: Organic Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology , Physics
    Notes: The reversible interaction of N-(1-ethylpropyl)-3, 4-dimethyl-2, 6-dinitroaniline (1) with HO- is characterized by several kinetic processes. The relaxation times of two of them were measured. It is suggested that the faster one is related to the protonation-deprotonation of the 3-methyl group and the value of the protonation rate is 0.19 s-1. The slowest process leads to the dianionic species with maximum absorption at 340 nm where one HO- group adds to the unsubstituted ring position of an anion derived from 1 by deprotonation of either the NH or the 3-methyl group. The rate and equilibrium constants for the formation of this species are reported.
    Additional Material: 4 Ill.
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  • 104
    Electronic Resource
    Electronic Resource
    Chichester : Wiley-Blackwell
    Journal of Physical Organic Chemistry 4 (1991), S. 310-314 
    ISSN: 0894-3230
    Keywords: Organic Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology , Physics
    Notes: The behaviour of cis-dicyanodi-1-10-phenanthrolinoiron(II) and acetylacetonato-N, N,N′,N′-tetramethylethylene-diaminocopper(II) perchlorate as solvatochromic indicators for the ability of solvents to donate a hydrogen atom or a pair of electrons, respectively, towards the formation of a hydrogen bond is examined by multivariable linear regressions and principal component analysis.
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  • 105
    Electronic Resource
    Electronic Resource
    Chichester : Wiley-Blackwell
    Journal of Physical Organic Chemistry 4 (1991), S. 463-466 
    ISSN: 0894-3230
    Keywords: Organic Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology , Physics
    Notes: A new Y scale for the correlation of solvolytic reactivities for benzylic ρ-nitrobenzoates was established based on rate data for 2-phenyl-2-adamantyl ρ-nitrobenzoate, and from which the solvent assistance in the solvolysis of tert-cumyl ρ-nitrobenzoate is suggested.
    Additional Material: 3 Ill.
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  • 106
    Electronic Resource
    Electronic Resource
    Chichester : Wiley-Blackwell
    Journal of Physical Organic Chemistry 4 (1991), S. 479-484 
    ISSN: 0894-3230
    Keywords: Organic Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology , Physics
    Notes: Theoretical calculations with the ab initio molecular orbital STO-3G basis set on the effect of trihydration on the relative acidities of 3- and 4-substituted phenols, 4-substituted quinuclidinium ions and 4-substituted bicyclo [2.2.2]octylammonium ions are reported. These results are contrasted with calculations on non-hydrated species and compared with results in aqueous solution and in the gas phase. Unlike results for smaller molecules such as substituted acetic acids and methylammonium ions, the solvation effects of three molecules of water are far short of that observed in going from the gas phase to aqueous solution. Reasons for this are discussed in the context of solvent attenuation factors for various molecules.
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  • 107
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    Chichester : Wiley-Blackwell
    Journal of Physical Organic Chemistry 4 (1991), S. 492-500 
    ISSN: 0894-3230
    Keywords: Organic Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology , Physics
    Notes: The preparation and characterization of 10-methyl- and 10-ethyl-9-decalyl cations is described. Both cations undergo a rapid, degenerate 10, 9-alkyl shift, but the ethyl group migration is about 700 times slower at -120°C than that of the methyl group. This preference is opposite to that usually found for alkyl migration rates and, on the basis of MO calculations, it is suggested that a conformational interchange may be the rate-determining step. Both cations irreversibly rearrange at about -100°C, giving in the methyl case the rearrangement cascade 10-methyl-9-decalyl → cis-1-methyldecalyl → trans-1-methyldecalyl → trans-2-methyldecalyl. Each of these rearrangement ions was independently prepared and characterized by NMR spectroscopy. One can rationalize the initial formation of the less stable cis ring junction on the basis of suprafacial hydride and methyl shifts. Attempts to add molecular hydrogen to the 10-methyl-9-decalyl cation were unsuccessful.
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  • 108
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    Chichester : Wiley-Blackwell
    Journal of Physical Organic Chemistry 4 (1991), S. 501-515 
    ISSN: 0894-3230
    Keywords: Organic Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology , Physics
    Notes: The mechanism of the Grignard reactions of substituted benzophenones with two kinds of alkyl Grignard reagent, n-C3H7MgBr, and i-C3H7MgBr, was investigated. In these reactions, both addition and reduction products were also generated. Based on the results of product analysis and stopped-flow, ESR and association measurements, it was confirmed that the product distribution was governed by several factors: the oxidizing ability of benzophenones, the association ability of Grignard reagents and the structure of alkyl groups of Grignard reagents. In particular, the strength of C—Mg and β-C—H bonds of Grignard reagents could strongly affect the product distribution.
    Additional Material: 8 Ill.
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  • 109
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 607-622 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The reaction pathways of n-butoxy and s-butoxy radicals have been investigated by TLC and HPLC analysis of end products, particularly peroxides and carbonyl compounds. The butoxy radicals were produced by the pyrolysis of very low concentrations of the corresponding dibutylperoxide in an atmosphere of oxygen and nitrogen, at atmospheric pressure. The decomposition reaction (3) s-BuO → C2H5 + CH3CHO and the reaction (2) s-BuO + O2 → HO2 + CH3COC2H5 have been studied, and the ratio k3/k2 has been determined in the temperature range 363-503 K by kinetic modeling of the formation of the observed acetaldehyde and methylethylketone. The rate constant k3 obtained was: \documentclass{article}\pagestyle{empty}\begin{document}$$ \log _{10} k_3 /{\rm s}^{ - 1} = \left({13.8 \pm _{0.3}^{0.2} } \right) - \left({15.0 \pm 0.9} \right){\rm kcal\,mol}^{ - 1} /2.303\,RT. $$\end{document} A good agreement was observed between experimental data and RRKM theory. The implications of the results for atmospheric chemistry and combustion are discussed. At room temperature, the reaction with O2, yielding HO2 radicals and methylethylketone is, by far, the main channel for s-BuO radicals. In the field of low temperature combustion, the decomposition of s-BuO radicals producing C2H5 and CH3CHO is the main pathway; the route s-BuO + O2 decreases tremendously in importance as the temperature is raised above 393 K.
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  • 110
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 639-654 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The rate of hydrolysis of title schiff bases was studied in the pH range 4-13 in 10% dioxanewater system, CTAB, NaLS micellar solutions. The hydrolysis was found to be due to ‘water’ and ‘hydroxide’ reactions and hence the rate constants in different pH were computed and analyzed with an intermediate involving a water molecule being positioned with the help of 2-OH group and the thiazolyl C-N pi bond. The ‘hydroxide’ reaction was due to a direct nucleophilic attack of hydroxide ion at the aldimine linkage of the reactant. The influence of cationic and anionic micelles supports the mechanistic picture in the entire pH range.
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  • 111
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 623-632 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Ultrasonic relaxation spectra of LiClO4 plus the open chain polyether triglyme (TG) at CLiClO4 ≃ 0.8 M, molar ratio R = [TG]/[LiClO4] = 1, and at temperatures of 15, 25, 35, and 45°C in dry acetonitrile are reported. Corresponding spectra for LiClO4 plus the macrocycle 12-crown-4 (12C4) at R = [12C4]/[LiClO4] = 1, at 10, 15, 20, 25, 30, and 40°C, and CLiClO4 = 0.32 M in acetonitrile are also reported.Both relaxation envelopes, for the two systems, have been fitted by two Debye relaxation processes and interpreted by the Eigen-Winkler reaction scheme: \documentclass{article}\pagestyle{empty}\begin{document}$$ {\rm Li}^ + \cdots {\rm PE} \mathop{\rightleftharpoons}\limits^{k_1}_{k_-1}{\rm LiPE}^ + \mathop{\rightleftharpoons}\limits^{k_2}_{k_-2} ({\rm LiPE})^ + $$\end{document} where “PE” symbolizes the polyether, Li+ … PE is a solvent separated species and LiPE+ and (LiPE)+ are two complex species. The temperature dependence of the relaxation spectra permits the calculation of the activation parameters for the forward and reverse processes for the system LiClO4 + TG and for one of the two processes for the LiClO4 + 12C4 system.Comparisons between the two sets of data lead to the conclusion that the much slower second relaxation process, in the case of the macrocycle, is attributable to a combination of an enthalpic and an entropic effect on the energy barrier for the present systems.
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  • 112
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 633-637 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The photolysis of azomethane in the near UV has been studied at room temperature and pressures from 10 mtorr to 10 torr. The main products, C2H6 and N2, accounted for more than 99% of the reaction. Minor hydrocarbon products observed were (with quantum yields) C3H8 (3.5 × 10-3), C2H4 (3.2 × 10-4), CH4 (3 × 10-3), and n-C4H10 (trace). Quantum yields of H2 of 4 × 10-5 and 2 × 10-5 were measured at azomethane pressures of 0.1 and 1.0 torr, respectively.The minor hydrocarbon products can be accounted for by reactions of CH3 and C2H5 radicals following hydrogen abstraction from azomethane by CH3. The H2 product observed represents an upper limit for the H2 elimination from vibrationally excited C2H6 formed by CH3 combination in the system, corresponding to a rate of elimination ca. 5 × 10-5 times the competing rate of dissociation to 2CH3. Assuming a frequency factor of 1013 s-1 for the H2 elimination, a lower limit of about 90 kcal mol-1 was estimated for the energy barrier.
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  • 113
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 1035-1050 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The rate coefficients of the reactions and were determined in a series of shock tube experiments from CN time histories recorded using a narrow-linewidth cw laser absorption technique. The ring dye laser source generated 388.44 nm radiation corresponding to the CN B2Σ+(v = 0) ← X2Σ+(v = 0) P-branch bandhead, enabling 0.1 ppm detection sensitivity.Reaction (1) was measured in shock-heated gas mixtures of typically 200 ppm N2O and 10 ppm C2N2 in argon in the temperature range 3000 to 4500 K and at pressures between 0.45 and 0.90 atm. k1 was determined using pseudo-first order kinetics and was found to be 7.7 × 1013 (±20%) [cm3 mol-1 s-1]. This value is significantly higher than reported by earlier workers. Reaction (2) was measured in two regimes. In the first, nominal gas mixtures of 500 ppm O2 and 10 ppm C2N2 in argon were shock heated in the temperature range 2700 K to 3800 K and at pressures between 0.62 and 1.05 atm. k2 was determined by fitting the measured CN profiles with a detailed mechanism. In the second regime, gas mixtures of 500 ppm O2 and 1000 ppm C2N2 in argon were shock heated in the temperature range 1550 to 1950 K and at pressures between 1.19 and 1.57 atm. Using pulsed radiation from an ArF excimer laser at 193 nm, a fraction of the C2N2 was photolyzed to produce CN. Pseudo-first order kinetics were used to determine k2. Combining the results from both regimes, k2 was found to be 1.0 × 1013 (±20%) [cm3 mol-1 s-1].
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  • 114
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 1075-1094 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Reactions of the hydroxyl radical, OH, with several organic species of interest in combustion chemistry have been studied near 1200 K and 1 atm in shock tube experiments in which UV absorption was used to monitor the OH concentration. Rate coefficients were measured for the reactions of OH with 2,3-dimethylbutane, isooctane, neooctane, ethylene, propylene, acetylene, formaldehyde, methanol, and ethanol. The values were found to be (in units of 1012 cm3/mol-s): 21, 22, 18, 2.6, 9.6, 0.28, 12, 5.2, and 5.3. These measured values are compared with previous experimental results and, where appropriate, transition-state theory calculations.
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  • 115
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    International Journal of Chemical Kinetics 23 (1991), S. 1051-1074 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The oxidative pyrolysis of methylene chloride, chloroform, and carbon tetrachloride has been investigated using a micro-bore, fused silica, tubular flow reactor operating under laminar flow conditions coupled to in-line GC-MS detection. Data were obtained over the temperature range 573-1273 K for the following conditions: chlorocarbon/oxygen equivalence ratios of 3.0, chlorocarbon concentrations of 2.7 ± 0.1 × 10-5 mols/L, gas-phase residence times of 2.0 s, and reactor pressures of 1.15 ± 0.05 atm. The parent stability (defined by the temperature required for 99% destruction) was evaluated as: \documentclass{article}\pagestyle{empty}\begin{document}$$ {\rm CH}_2 {\rm Cl}_2 :1028{\rm\, K, CHCl}_3 :873{\rm\, K,}\,{\rm CCl}_{\rm 4} :1153{\rm\, K} $$\end{document} Chemically activated recombination of chlorinated C1 radicals are proposed as important pathways to chlorinated ethane and olefin products. The most significant finding from analysis of product distributions containing ≥2 carbon atoms was the observation of ca. 1 mol% yields of higher-molecular-weight perchlorinated aromatic species from the decomposition of chloroform and carbon tetrachloride. Implications with respect to the controlled high-temperature incineration of these chlorinated methanes are briefly discussed.
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  • 116
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 1095-1109 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Rate constants for the reactions of OH radicals and Cl atoms with CH3ONO, C2H5ONO, n-C3H7ONO, n-C4H9ONO, and n-C5H11ONO have been determined at 298 ± 2 K and a total pressure of approximately 1 atm. The OH rate data were obtained using both the absolute rate technique of pulse radiolysis combined with kinetic spectroscopy and a relative rate method involving simultaneous measurement of the loss of the nitrite and the reference compound. The Cl rate constants were measured using the relative rate method. Values of the rate constants in units of 10-13 cm3 molecule-1 s-1 are: TextRelative ClRelative OHAbsolute OHCH3ONO94.4 ± 7.43.0 ± 1.02.6 ± 0.5C2H5ONO295 ± 137.0 ± 1.57.0 -1.1n-C3H7ONO646 ± 5811.0 ± 1.512.0 ± 0.5n-C4H9ONO1370 ± 5822.7 ± 0.827.2 ± 6.0n-C5H11ONO2464 ± 44437.4 ± 5.042.5 ± 8.0When compared to rate data for the corresponding alkanes the results show that the -ONO group decreases the rate constant for H atom abstraction by the OH radical from groups bonded to the -ONO group and also decreases that for groups in the β position. Similar results were found for the reaction of Cl atoms with these compounds. The results are discussed in terms of reactivity trends.
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  • 117
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    International Journal of Chemical Kinetics 23 (1991), S. 761-766 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Tert-butoxyl radicals react with indole and methyl substituted derivatives by hydrogen abstraction. For those compounds which are unsubstituted at the N-atom, hydrogen abstraction takes place almost exclusively at the N—H bond. The reactivity of these compounds correlates with their donor electron capacity, pointing to significant contribution of charge transfer to the transition state stability. Substitution at the N atom considerably decreases the reactivity.
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  • 118
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    International Journal of Chemical Kinetics 23 (1991), S. 733-760 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics of pyrolysis of pyrrole dilute in argon have been studied in a single pulse shock tube, using capillary column GC, together with GC/MS and FTIR for product identification, over the temperature range 1200-1700 K, total pressures of 7.5-13.5 atm and nominal mixture compositions of pyrrole of 5000 and 700 ppm (nominal concentrations of 5 × 10-7 and 7 × 10-8 mol cm-3). Time-resolved measurements of the rate of disappearance of pyrrole behind reflected shock waves have been made by absorption spectroscopy at 230 nm, corresponding to the lowest 1π* ← 1π transition of pyrrole at pressures of 20 atm and mixture compositions between 1000-2000 ppm pyrrole (1.7-3.0 × 10-7 mol cm-3) over the temperature range of 1300 to 1700 K. At the lower end of the studied temperature range, the isomers of pyrrole, allyl cyanide and cis- and trans-crotononitrile, were the principal products, together with hydrogen cyanide and propyne/allene. At elevated temperatures, acetylene, acetonitrile, cyanoacetylene, and hydrogen became important products.The rate of overall disappearance of pyrrole, as measured by absorption spectrometry, was found to be first order in pyrrole concentration, with a rate constant kdis(pyrrole) = 1014.1±0.7 exp(-74.1 ± 3.0 kcal mol-1/RT) s-1 between 1350-1600 K and at a pressure of 20 atm. First order dependence of pyrrole decomposition and major product formation was also observed in the single pulse experiments over the range of mixture compositions studied.A 75-step reaction model is presented and shown to substantially fit the observed temperature profiles of the major product species and the reactant profile. In the model the initiation reaction is postulated to be the reversible formation of pyrrolenine, (2H-pyrrole). Pyrrolenine can undergo ring scission at the C2—N bond forming a biradical which can rearrange to form allyl cyanide and crotononitrile or undergo decomposition to form HCN and C3H4 or acetylene and a precursor of acetonitrile. The model predicts an overall rate of disappearance of pyrrole in agreement with the experimental measurements.
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  • 119
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    International Journal of Chemical Kinetics 23 (1991), S. 779-783 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics of the gas phase pyrolyses of methyl 2-bromopropionate and 2-bromopropionic acid were studied in a seasoned, static reaction vessel and under maximum inhibition of the free radical suppressor toluene. The working temperature and pressure range was 310-430°C and 26.5-201.5 torr, respectively. The reactions proved to be homogeneous, unimolecular, and obeys a first-order rate law. The rate coefficients are expressible by the following equations: for methyl 2-bromopropionate, log k1(s-1) = (13.10 ± 0.34) - (211.4 ± 4.4)kJ mol-1(2.303RT)-1; for 2-bromopropionic acid, log k1(s-1) = (12.41 ± 0.29) - (180.3 ± 3.4)kJ mol-1(2.303RT)-1. The bromoacid yields acetaldehyde, CO and HBr. Because of this result, the mechanism is believed to proceed via a polar five-membered cyclic transition state.
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  • 120
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    International Journal of Chemical Kinetics 23 (1991), S. 767-778 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: We have developed a computer code for an IBM PC/XT/AT or compatible which can be used to estimate, edit, or enter thermodynamic property data for gas phase radicals and molecules using Benson's group additivity method. The computer code is called THERM (THermo Estimation for Radicals and Molecules). All group contributions considered for a species are recorded and thermodynamic properties are generated in old NASA polynomial format for compatibility with the CHEMKIN reaction modeling code. In addition, listings are created in a format more convenient for thermodynamic, kinetic, and equilibrium calculations. Polynomial coefficients are valid from 300-5000 K using extrapolation methods based upon the harmonic oscillator model, an exponential function, or the Wilhoit polynomials. Properties for radical and biradical species are calculated by applying bond dissociation increments to a stable parent molecule to reflect loss of H atom. THERM contains a chemical reaction interpreter to calculate thermodynamic property changes for chemical reactions as functions of temperature. These include equilibrium constant, heat release (required heat, ΔHr), entropy change (ΔSr), Gibbs free energy change (ΔGr), and the ratio of forward to reverse Arrhenius A-factors (for elementary reactions). This interpreter can also process CHEMKIN input files. A recalculation procedure is incorporated for rapid updating of a database of chemical species to reflect changes in estimated bond dissociation energies, heats of formation, or other group values. All input and output files are in ASCII so that they can be easily edited, expanded, or updated.
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  • 121
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    International Journal of Chemical Kinetics 23 (1991), S. 785-798 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The ultraviolet absorption spectra of the peroxy radicals derived from hydrochlorofluorocarbons 141b and 142b, (CFCl2CH2O2 and CF2ClCH2O2, respectively), and the kinetics of their self reactions have been studied in the gas phase at 298 K using a pulse radiolysis technique. Absorption cross sections were quantified over the wavelength range 220-300 nm. Measured absorption cross sections at 250 nm were indistinguishable within the experimental uncertainties (≈10%) and yield; \documentclass{article}\pagestyle{empty}\begin{document}$$ \sigma _{{\rm CFCl2CH2O2}} (250{\rm\, nm) =\,}\sigma _{{\rm CF2ClCH2O2}} (250{\rm\, nm) = (3}{\rm .38}\, \pm\, {\rm 0}{\rm .68)}\, \times\, {\rm 10}^{- 18}\, {\rm cm}^{\rm 2}\, {\rm molecule}^{- 1} $$\end{document} Errors represent the sum of statistical uncertainty and our estimate of potential systematic errors. Our absorption cross section data were then used to derive the observed self reaction rate constants for reactions (1) and (2), defined as -d[RO2]/dt = 2k[RO2]2 (R = CFCl2CH2 or CF2ClCH2), of k1obs = (4.36 ± 0.64) × 10-12 and k2obs = (4.13 ± 0.58) × 10-12 cm3 molecule-1 s-1, quoted errors represent 2σ. These results are discussed with respect to previous studies of the absorption spectra and kinetics of peroxy radicals.
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  • 122
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    International Journal of Chemical Kinetics 23 (1991), S. 799-805 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: A kinetic study of base-catalyzed hydrolysis of Cu(II)-malonamide complex has been performed in sodium hydroxide solution (0.2-1.25M). The reaction follows an irreversible first-order consecutive path: \documentclass{article}\pagestyle{empty}\begin{document}$$ {\rm Cu}\left({{\rm II}} \right) - {\rm Malonamide\,Complex}\mathop {\longrightarrow}\limits_{ - {\rm NH}_3 }^{k_{1obs} } {\rm Malonamic\,Acid}\mathop {\longrightarrow}\limits_{ - {\rm NH}_3 }^{k_{2obs} } {\rm Malonic\,Acid} $$\end{document} The variation of k1obs and k2obs with alkali concentration was found to be in good agreement with the equations: \documentclass{article}\pagestyle{empty}\begin{document}$$ \begin{array}{*{20}c} {1/k_{{\rm 1obs}} = B_1 + B_2 /[{\rm \bar OH]}} & {{\rm and}} \\ \end{array} $$\end{document} \documentclass{article}\pagestyle{empty}\begin{document}$$ 1/k_{{\rm 2obs}} = C_1 + C_2 /[{\rm \bar OH]} $$\end{document} where B1, B2, C1, and C2 are empirical constants. The mechanism of hydrolysis of Cu(II)-malonamide complex has been discussed and rate equations have been derived. Retardation of rate of hydrolysis due to coordination of Cu(II) with malonamide, in alkaline medium, has been explained in terms of comparatively slow breakdown of the C—N bond of the tetrahedral intermediate (TI). Thermodynamic parameters have also been evaluated.
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  • 123
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics of oxidation of triethanolamine (TEA) by diperiodatoargenate(III) anion, [Ag(HIO6)2]5-, has been studied in aqueous alkaline medium by conventional spectrophotometry. The reaction is pseudo-first-order in [Ag(III)] disappearance with kobs = (k1 + k2[OH-]) K1K2[TEA]/{[H2IO63-]e + K1 + K1K2[TEA]}, where k1 = 8.05 × 10-3 S-1, k2 = 0.46 M-1 S-1, K1 = 6.15 × 10-4 M, and K2 = 537 M-1 at 25°C, and μ = 0.30 M. Based on the inference that an inner-sphere complex is formed by indirect replacement of a ligand of [Ag(HIO6)2]5- by a TEA molecule, a reaction mechanism has been proposed. The complex undergoes redox by two modes, both internal and one hydroxide ion assisted.
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  • 124
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    International Journal of Chemical Kinetics 23 (1991), S. 807-814 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The bridged dimer of molybdenum(V), Mo2O42+ (aq) is oxidized to Mo(VI) by carboxylato-bound chromium(V). Reaction of bis(chelated) Cr(V) with excess (MoV)2 yields a chelated Cr(III) complex, but this conversion proceeds through a pink Cr(IV) intermediate, indicating that the oxidation of (MoV)2 entails a series of le- steps, passing through a reactive transient, the mixed valence complex, MoVMoVI. When experiments are carried out in buffers of the ligating acid, 2-ethyl-2-hydroxybutanoic acid, two stages of ligation of (MoV)2 by the ligand anion, characterized by rate constants near 104 and 0.14 M-1 s-1 (19°C; pH 3.0; μ = 0.6 M) must be considered. In quick mixing experiments, the first, but not the second, of these proceeds before the redox reaction gets under way, and autocatalytic redox profiles are observed. If the slower ligation is allowed to reach completion before Cr(V) is added, reduction to Cr(IV) is greatly accelerated and conforms to the superposition of two processes, whereas the reduction of Cr(IV) to Cr(III) is slow and exhibits a rate independent of [CrIV]. A proposed sequence applicable to the latter conditions includes reductions of Cr(V) at two ligation levels, slow unimolecular conversion of (MoV)2 to an activated form, and rapid reduction of the latter with Cr(IV). Here Cr(IV) has assumed the role of a scavenger for the reactive form of (MoV)2.
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  • 125
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    International Journal of Chemical Kinetics 23 (1991), S. 825-835 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The classical mechanism of chemically activated unimolecular reactions is extended to interpret experimental results in systems olefin/hydrogen atoms. In the case of a large excess of the latter, one has to take into consideration a second chemical activation of the primarily formed radicals by their recombination with H-atoms to yield chemically activated alkane molecules. The radicals as well as the alkane molecules may decompose, and a method based on the coupling of two steady-state master equations is developed to evaluate the contribution of either of the two reaction paths to the ratio decomposition to stabilization. The treatment proposed is demonstrated for the example cis but-2-ene/excess of thermal hydrogen atoms in the presence of molecular hydrogen as a bath gas at 298 K. It turns out that the step via activated butane is not negligible under these conditions.
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  • 126
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    International Journal of Chemical Kinetics 23 (1991) 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
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  • 127
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    International Journal of Chemical Kinetics 23 (1991), S. 1111-1128 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: This article describes a general kinetic formalism for treating the details of heterogeneous reactions at a gas-solid interface. We develop a nomenclature for treating reactions between the gas phase and surface species residing on any number of surface site types and bulk-phase species residing in bulk-phase mixtures or in pure bulk phases. The rate of progress of surface reactions follows the law of mass-action. We discuss the relationship between macroscopic conservation laws for mass and energy and the microscopic surface reaction rates as they might appear in boundary conditions for a chemically reacting flow. The formalism developed has been implemented in a general package of Fortran computer codes for the evaluation of complex surface-reaction kinetics called Surface Chemkin.
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  • 128
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    International Journal of Chemical Kinetics 23 (1991), S. 1129-1149 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The thermal reaction of HNCO has been studied in a static cell at temperatures between 873 and 1220 K and a constant pressure of 800 torr under highly diluted conditions. The reaction was measurable above 1000 K by FTIR spectrometry. The products detected include CO, CO2, HCN, NH3, and the unreacted HNCO. In this moderate temperature regime, the rates of product formation and HNCO decay cannot be accounted for by a previously established high-temperature mechanism, assuming HNCO → NH + CO (1) as the initiation process. Instead, a new bimolecular reaction, 2HNCO → CO2 + HNCNH (2), has been invoked to interpret the disappearance of HNCO as well as the formation of various products, most importantly CO2.The concentration profiles of all measured species can be quantitatively modeled, throughout the temperature range analyzed, by varying k2 using a modified mechanism. The kinetically modeled values of k2 can be effectively represented by \documentclass{article}\pagestyle{empty}\begin{document}$$ k_{\rm 2} = 10^{10.84 \pm 0.07} {\rm \,exp}(- 21,240 \pm 1,960/{\rm T}){\rm\, cm}^3 /{\rm mol\, s}{\rm .} $$\end{document}This result agrees closely with that computed with the conventional transition-state theory using the TST parameters predicted by the BAC-MP4 method: \documentclass{article}\pagestyle{empty}\begin{document}$$ k_2 ({\rm BAC} - {\rm MP}4) = 10^{11.13} {\rm \,exp(- 21,600/T) cm}^{\rm 3} /{\rm mol s}{\rm .} $$\end{document}The bimolecular reaction takes place via a stable 4-membered ring intermediate which is isoelectronic with diketene; viz.
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  • 129
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    International Journal of Chemical Kinetics 23 (1991) 
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    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
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  • 130
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    International Journal of Chemical Kinetics 23 (1991), S. 37-45 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The overall rate coefficient k of the self recombination of BrO radicals has been measured at 298 K with use of the discharge flow/mass spectrometry technique. The rate coefficient k2 for the reaction channel forming Br2 has been also determined. The results are: k = (3.2 ± 0.5) × 10-12 and k2 = (4.7 ± 1.5) × 10-13 (in cm3 molecule-1 s-1). These results are discussed with respect to previous literature data.
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  • 131
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    International Journal of Chemical Kinetics 23 (1991), S. 17-26 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Kinetics of the sulfuric acid catalyzed esterification of palmitic acid with isobutyl alcohol has been studied and reviewed critically. A theoretical rate equation is derived by the following reaction mechanism: (1) The reaction of sulfuric acid and isobutyl alcohol produces isobutyl sulfuric acid which acts as a catalyst; (2) Palmitic acid is protonated by the catalyst to form the reaction intermediate; and (3) The esterification proceeds reversibly. The experimental results are consistent with this rate equation.
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  • 132
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    International Journal of Chemical Kinetics 23 (1991), S. 27-35 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Kinetics of oxidation of indigo carmine (IC) by sodium hypohalites, NaOX (X = Cl or Br), in alkaline buffer of pH 9-11 has been studied spectrophotometrically at λ = 610 nm. The experimental rate law obtained is -d[IC]/dt = k[OX-][IC][OH-]x where x 〈1. Variation of ionic strength or dielectric constant of the medium had no effect on the reaction rate while the addition of halide ions slightly retarded the rate. A most plausible mechanism proposed on the basis of experimental results involves the formation of isatin sulphonate which undergoes further oxidation to anthranilate. Activation parameters have been evaluated.
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  • 133
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    International Journal of Chemical Kinetics 23 (1991), S. 1-15 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The thermal decomposition of CCl3O2NO2,CCl2FO2NO2, and CClF2O2NO2 was studied in a temperature-controlled 420 l reaction chamber using in situ detection of peroxynitrates by long-path IR absorption. The temperature dependence of the unimolecular dissociation rate constants was determined at total pressures of 10 and 800 mbar in nitrogen as buffer gas, and the pressure dependence was measured at 273 K between 10 and 800 mbar. In Troe's notation, the data are represented by the following values for the limiting low and high pressure rate constants k0/[N2] and k∞ and the fall-off curvature parameter Fc (in units of cm3 molecule-1 s-1, s-1): CCl3O2NO2,k0/[N2] = 6.3 × 10-3 exp(-85.1 kJ · mol-1/RT), k∞ = 4.8 × 1016 exp(-98.3 kJ · mol-1/RT), Fc = 0.22; CCl2FO2NO2, k0/[N2] = 1.01× 10-2 exp(-90.3 kJ · mol-1/RT), k∞ = 6.6 × 1016 exp(-101.8 kJ · mol-1/RT), Fc = 0.28; and CClF2O2NO2, k0/[N2] = 1.80 × 10-3 exp(-87.3 kJ · mol-1/RT), k∞ = 1.60 × 1016exp(-99.7 kJ · mol-1/RT), Fc = 0.30. From these dissociation rate constants and recently measured rate constants for the reverse reaction (see Caralp, Lesclaux, Rayez, Rayez, and Forst [19]), bond energies (=ΔHr,00) of 100, 103, and 104 kJ/mol were derived for the RO2-NO2 bonds in CCl3O2NO2, CCl2FO2NO2, and CClF2O2NO2, respectively. The kinetic and thermochemical parameters of these decomposition reactions are compared with those of the dissociation of other peroxynitrates. Atmospheric implications of the thermal stability of chlorofluoromethyl peroxynitrates are briefly discussed.
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  • 134
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    International Journal of Chemical Kinetics 23 (1991), S. 47-56 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The photolysis of C2F5I with CF3COOH in the temperature range 473-533 K was studied in the gas phase.Evidence is presented that supports a complex mechanism for the formation of C2F5H through the H-atom abstraction reaction from CF3COOH by C2F5 radicals as well as the participation of I(2P½).
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  • 135
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    International Journal of Chemical Kinetics 23 (1991), S. 99-101 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: It is reported and explained that the front-like reaction sustains, and its velocity is enhanced in frozen phase in the chlorite-thiosulphate system.
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  • 136
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    International Journal of Chemical Kinetics 23 (1991), S. 57-76 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: We have studied the effect of vibrational mode activation in the CF3 radical on the bromine abstraction reaction; CF3 + Br2 → CF3Br + Br. Excess vibrational energy resides in the symmetric modes of the radical after 248 nm photolysis of the parent molecule, CF3I. Our data indicate that the hot radicals react no faster than thermalized CF3, and may actually have a lower cross-section for reaction. Dynamical factors that result in poor coupling of the vibrational energy to the reaction coordinate, as well as other similar considerations, could be responsible for the experimental observations. In addition, we have made an independent determination of the rate for the bromine abstraction reaction of (1.08 ± .13) × 1012 s-1 cm3 mol-1.
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  • 137
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    International Journal of Chemical Kinetics 23 (1991), S. 77-97 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The ring-retaining products formed from the OH radical-initiated reactions of o-, m-, and p-xylene in the presence of NOx have been identified and their formation yields determined. Experiments were carried out at 298 ± 2 K and in the presence of 740 torr total pressure of air. The products observed, and their yields, were: from o-xylene, o-tolualdehyde, 0.0453; 2-methylbenzyl nitrate, (0.0135 + 5.5 × 10-17 [NO2]); 2,3-dimethylphenol, 0.097; 3,4-dimethyl-phenol, 0.064; 3-nitro-o-xylene, 0.0059; 4-nitro-o-xylene, (0.0111 + 9.9 × 10-17 [NO2]); from m-xylene, m-tolualdehyde, 0.0331; 3-methylbenzyl nitrate, 0.0061; 2,4-dimethylphenol, 0.099; 2,6-dimethylphenol, 0.111; 4-nitro-m-xylene, 0.0018; 5-nitro-m-xylene, (0.0032 + 1.6 × 10-17 [NO2]); from p-xylene, p-tolualdehyde, 0.0701; 4-methylbenzyl nitrate, 0.0082; 2,5-dimethylphenol, 0.188, 2-nitro-p-xylene, (0.0120 + 2.8 × 10-17 [NO2]), where the NO2 concentration is in molecule cm-3 units. The nitro-xylene data are consistent with our recent product study of the corresponding reactions of benzene and toluene and indicate that under the experimental conditions employed the dimethylhydroxycyclohexadienyl radicals reacted with NO2 and not with O2. When combined with literature ring-cleavage product yields, these data show that ca. 55-80% of the reaction pathways are accounted for.
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  • 138
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    International Journal of Chemical Kinetics 23 (1991), S. 103-103 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
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  • 139
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    Topics: Chemistry and Pharmacology
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  • 140
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    International Journal of Chemical Kinetics 23 (1991), S. 113-125 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics and mechanism of the oxidation of 3,3′-dimethoxybenzidine (oda, o-dianisidine) by potassium bromate in aqueous acidic medium were studied by monitoring the formation rate of the reaction product, 3,3′-dimethoxy 4,4′-diphenoquinone at 447 nm. The reaction is, first order with respect to both the substrate and oxidant, and second order with respect to H+. The oda: bromate stoichiometric ratio is 1:1. Plausible mechanism and rate laws are proposed accounting the experimental findings. Computer simulations were done using the proposed mechanism.
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  • 141
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    International Journal of Chemical Kinetics 23 (1991), S. 127-136 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Kinetics of oxidation of cinnamaldehyde (Cinn) by chloramine-T (CAT) has been studied in solutions containing HCl and H2SO4 at 313 K. The respective experimental rate laws obtained in HCl and H2SO4 media are as follows: and Here the value of x varies from 0.9 to zero while the values of y and z are 0.83 and 0.72, respectively. Effects, on the reaction rate, of ionic strength, reaction product (p-toluenesulfonamide), dielectric constant of the solvent medium, and the anions, Cl- and SO42-, have been investigated. Activation parameters have been computed, based on the rate constants determined at different temperatures. Mechanisms proposed and the rate laws derived are consistent with the observed kinetic data represented by the experimental rate laws.
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  • 142
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics of the reactions of manganese(III) complexes of trans-cyclohexane-1,2-diamine-NNN′N′-tetraacetic acid (H4cydta) and 2,2′-bipyridyl (bpy) have been investigated in the acid ranges [H+] = 1.00 ×10-5 - 3.16 × 10-3 M and [H+] = 0.10 - 1.00 M, respectively, at different temperatures and at a constant ionic strength. Both the molecular and mono-anionic forms of ascorbic acid have been found to be reactive in the experimental acid ranges. The monoanionic species has been found to be more reactive than the molecular form. Attempts have been made to correlate the kinetic results in terms of the Marcus relationship for outer-sphere electron transfer reaction. Differences between the calculated rates (k0.8) and experimental rates (k) by approximately four and seven orders of magnitude (k0.8≪ k) suggest an innersphere pathway for the reaction of Mn(cydta)(H2O)-. Inner-sphere reaction is also believed to be operative for the other reaction. The activation parameters have been evaluated and compared with other reported systems.
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  • 143
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    International Journal of Chemical Kinetics 23 (1991), S. 137-149 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: In the stirred batch experiment, the Mn(II)-catalyzed bromate-saccharide reaction in aqueous H2SO4 or HClO4 solution exhibits damped oscillations in the concentrations of bromide and Mn(II) ions. Peculiar multiple oscillations are observed in the system with arabinose or ribose. The apparent second-order rate constants of the Mn(III)-saccharide reactions at 25°C are (0.659, 1.03, 1.76, 2.32, and 6.95) M-1 s-1 in 1.00 M H2SO4 and (4.69, 7.51, 10.2, 13.5, and 36.2) M-1 s-1 in (2.00-4.00) M HClO4 for (glucose, galactose, xylose, arabinose, and ribose), respectively. At 25°C, the observed pseudo-first-order rate constant of the Mn(III)-Br- reaction is kobs = (0.2 ± 0.1) [Br-] + (130 ± 5)[Br-]2 + (2.6 ± 0.1) × 103[Br-]3 + (1.2 ± 0.2) × 104[Br-]4 s-1 and the rate constant of the Br2—Mn(II) reaction is less than 1 × 10-4 M-1 s-1. The second-order rate constants of the Br2-saccharide reactions are (3.65 ± 0.15, 11.0 ± 0.5, 4.05, 12.5 ± 0.7, and 2.62) × 10-4 M-1 s-1 at 25°C for glucose, galactose, xylose, arabinose, and ribose, respectively.
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  • 144
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    Keywords: Chemistry ; Physical Chemistry
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    Topics: Chemistry and Pharmacology
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  • 145
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    International Journal of Chemical Kinetics 23 (1991), S. 151-160 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The rate constants for the reaction of CN with N2O and CO2 have been measured by the laser dissociation/laser-induced fluorescence (two-laser pump-probe) technique at temperatures between 300 and 740 K. The rate of CN + N2O was measurable above 500 K, with a least-squares averaged rate constant, k = 10-11.8±0.4 exp(-3560 ± 181/T) cm3/s. The rate of CN + CO2, however, was not measurable even at the highest temperature reached in the present work, 743 K, with [CO2] ≤ 1.9 × 1018 molecules/cm3.In order to rationalize the observed kinetics, quantum mechanical calculations based on the BAC-MP4 method were performed. The results of these calculations reveal that the CN + N2O reaction takes place via a stable adduct NCNNO with a small barrier of 1.1 kcal/mol. The adduct, which is more stable than the reactants by 13 kcal/mol, decomposes into the NCN + NO products with an activation energy of 20.0 kcal/mol. This latter process is thus the rate-controlling step in the CN + N2O reaction. The CN + CO2 reaction, on the other hand, occurs with a large barrier of 27.4 kcal/mol, producing an unstable adduct NCOCO which fragments into NCO + CO with a small barrier of 4.5 kcal/mol. The large overall activation energy for this process explains the negligibly low reactivity of the CN radical toward CO2 below 1000 K.Least-squares analyses of the computed rate constants for these two CN reactions, which fit well with experimental data, give rise to \documentclass{article}\pagestyle{empty}\begin{document}$$ k_{{\rm N}_{\rm 2} {\rm O}} \, = \,6.4 \times 10^{- 21} {\rm T}^{{\rm 2}{\rm .6}} \exp (- 1860/{\rm T)cm}^{\rm 3} /{\rm s} $$\end{document} \documentclass{article}\pagestyle{empty}\begin{document}$$ k_{{\rm C} {\rm O}_{\rm 2}} \, = \,6.1 \times 10^{- 18} {\rm T}^{{\rm 2}{\rm .2}} \exp (- 13530/{\rm T)cm}^{\rm 3} /{\rm s} $$\end{document} for the temperature range 300-3000 K.
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    International Journal of Chemical Kinetics 23 (1991), S. 161-172 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Rates of solvolysis of complex ions [Co(3Rpy)4Cl2]+ with R = Me and Et have been determined in mixtures of water with the hydrophobic co-solvent propan-;2-ol for a range of temperatures. The variations of the enthalpies and entropies of activation with the solvent composition have been correlated with the physical properties of the solvent and it has been shown that the linear plot found for ΔH* against ΔS* in water + propan-2-ol is coincident with that found for water + methanol mixtures. A free energy cycle has been applied to the dissociative-type process of initial state (Cn+) going to the transition state (M(n+1)+…‥ Cl-) using values for the free energy of transfer of the chloride ion from water into the mixture, ΔGt∘(Cl-), derived from the solvent sorting technique or from the TATB/TPTB method. Irrespective of the source of ΔGt∘(Cl-), it is found that ΔGt∘(Co(3Rpy)4Cl2+*) ca. ΔGt∘(Co(3Rpy)4Cl2+) (where * indicates a species in the transition state) for mol fractions of propan-2-ol x2 ≳ 0.04-0.05 with ΔGt∘(Co(3Rpy)4Cl2+*) becoming increasingly more negative than ΔGt∘(Co(3Rpy)4Cl2+) as x2 increases above 0.05. These variations are compared with those for the solvolysis of the same ions in water + methanol mixtures and of a range of other ions in water + propan-2-ol mixtures. It is concluded that, using values for ΔGt∘(Cl-) from either source, the stabilizing influence of changes in solvent structure is greater on the cation in the transition state than on the cation in the initial state for the solvolyses of complexes [Co(Rpy)4Cl2+] and [Coen2LCl]n+.
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  • 147
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    International Journal of Chemical Kinetics 23 (1991), S. 173-196 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The reactions of NH(X3Σ-) with NO, O2, and O have been studied in reflected and incident shock wave experiments. The source of NH in all the experiments was the thermal dissociation of isocyanic acid, HNCO. Time-histories of the NH(X3Σ) and OH(X2Π) radicals were measured behind the shock waves using cw, narrow-linewidth laser absorption at 336 nm and 307 nm, respectively. The second-order rate coefficients of the reactions: were determined to be: \documentclass{article}\pagestyle{empty}\begin{document}$$ k_{\rm 3} \, = \,1.7 \times 10^{14} \exp (- 6400/{\rm T,K)}\,\,\,\,\,\,{\rm (}f\, = \,0.65,{\rm F}\,{\rm =}\,{\rm 1}{\rm .5)}\,\,\,\,\,\,{\rm T}\,{\rm =}\,{\rm 2220 - 3350\, K,} $$\end{document} \documentclass{article}\pagestyle{empty}\begin{document}$$ k_{\rm 4} \, = \,3.5 \times 10^{13} \exp (- 6800/{\rm T,K)}\,\,\,\,\,\,{\rm (}f\, = \,0.65,{\rm F}\,{\rm =}\,{\rm 1}{\rm .5)}\,\,\,\,\,\,{\rm T}\,{\rm =}\,{\rm 2220 - 3370\, K,} $$\end{document} and \documentclass{article}\pagestyle{empty}\begin{document}$$ k_{\rm 5} \, = \,9.2 \times 10^{13} \,\,\,\,\,\,\,\,\,\,\,\,{\rm (}f\, = \,0.60,{\rm F}\,{\rm =}\,{\rm 1}{\rm .6)}\,\,\,\,\,\,{\rm T}\,{\rm =}\,{\rm 2730 - 3380\, K,} $$\end{document} cm3 mol-1 s-1, where ƒ and F define the lower and upper uncertainty limits, respectively.The branching fraction of channel defined as k3b/k3total, was determined to be 0.19 ± 0.10 over the temperature range of 2940 K to 3040 K.
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  • 148
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    International Journal of Chemical Kinetics 23 (1991), S. 197-202 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: We have performed a product and kinetic study of the hydrolysis of 3,4-diphenyl-1,2,5-thiadiazole-1,1-dioxide in aqueous solution. Benzil and sulfamide are the only products of hydrolysis and are formed in equimolar yields.The kinetic results indicate that a first order law is followed up to 90% conversion. The observed rate constant is independent of substrate concentration.Ionic strength and buffer concentration do not affect the rate constant, but the reaction is acid-base catalyzed. The rate-pH profile has been determined and a mechanism that fits the experimental data satisfactorily is proposed. Corresponding rate constants and equilibrium constants for the protonation of the substrate are reported.
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  • 149
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    International Journal of Chemical Kinetics 23 (1991), S. 203-213 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The reaction of peroxomonophosphoric acid and hydrazinium ion in acid perchlorate solutions occurs as per stoichiometry (i), and the rate law (ii) at large [N2H5 +], where K′d is the first acid dissociation constant of H3PO5 and k 1 and k 2 are rate constants found to be 2.6 × 10-4 s-1 and 5.0 × 10-2 M-1 s-1, respectively, at 35°. The reaction is greatly catalyzed by iodide ions. The mechanism involves a redox cycle I-/I2 and the rate is independent of [N2H5 +] in the presence of iodide ions. K′d was found to be 0.55 M-1 and independent of temperature.
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  • 150
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    International Journal of Chemical Kinetics 23 (1991), S. 215-227 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Rate constants for the retro-Diels-Alder dissociation of 1,2,3,6-tetrahydropyridine, to 1,3-butadiene and methanimine, have been measured over 650-1450 K. To cover this range, three separate techniques were used at three laboratories: laser schlieren and single pulse shock tube methods, and a comparative rate flow system technique. The derived rate constants are extrapolated to the high-pressure limit with an RRKM model parameterized to fit the falloff observed in the laser-schlieren measurements. The resulting high-pressure rate constants show a reduction in activation energy of about 10 kcal/mol, comparing the isoelectronic cyclohexene, but little change in A-factor. There is an apparent increase in activation energy of 4 kcal/mol over the temperature range of these experiments, which is just outside probable error. Such a rise in activation energy is in marked contrast to the drop usually seen in simple bond fission, and may reflect a change from a concerted to a stepwise, biradical mechanism at high temperatures.
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  • 151
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    International Journal of Chemical Kinetics 23 (1991), S. 229-236 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Bromite, BrO2-, in aqueous carbonate or borate buffers (pH 9-11), reacts rapidly with H3AsO3, with the tartrate complex of Sb(III), and with the EDTA complexes of Sn(II) and U(IV). Each reaction yields Br-, even when BrO2- is taken in excess. Reaction rates with Sb(III) and Sn(II) are independent of pH, but the acidity pattern observed with As(III) points to competing bimolecular reductions by H2AsO3- and H3AsO3 having specific rates 3.4 and 1.2 M-1 s-1 (25°C, μ = 0.5M). Reduction by U(IV) is strongly inhibited by carbonate; data for carbonate buffers are in accord with the operation of two contributing reaction paths (specific rates 0.45 and 6.3 M-1 s-1) with the activated complex for the slower featuring one more carbonate than that for the rapid. Reactions of BrO2- with single electron reductants, or with reagents that can undergo both 1e and 2e changes, are generally complicated by variable induction periods, inhibition by O2, catalyzed decomposition of BrO2-, or combinations of these. The much smoother reductions by 2e- reagents must pass through OBr-, which reacts much more rapidly than BrO2- in each case. An inner-sphere path, operating through an oxygen-bridged transition state and culminating in oxygen atom transfer, is proposed for the 2e reductants. Hypophosphite, despite its highly negative formal potential, is not oxidized by BrO2- under our conditions. Here it is likely that the substitution-inert character of the coordinatively saturated P(I) center rules out formation of the precursor required for redox.
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  • 152
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    International Journal of Chemical Kinetics 23 (1991), S. 237-245 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The reactions of IO radicals with CH3SCH3, CH3SH, C2H4, and C3H6 have been studied using the discharge flow method with direct detection of IO radicals by mass spectrometry. The absolute rate constants obtained at 298 K are the following: IO + CH3SCH3 → products (1): k1 = (1.5 ± 0.2) × 10-14; IO + CH3SH → products (2): k2 = (6.6 ± 1.3) × 10-16; IO + C2H4 →products (3): k3 〈 2 × 10-16; IO + C3H6 → products (4): k4 〈 2 × 10-16 (units are cm3 molecule-1 s-1). CH3S(O)CH3 and HOI were found as products of reactions (1) and (2), respectively. The present lower value of k1 compared to our previous determination is discussed.
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  • 153
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    International Journal of Chemical Kinetics 23 (1991), S. 247-250 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The thermal decomposition of benzoylformic acid into carbon dioxide and benzaldehyde is a unimolecular first-order reaction which takes place according to the rate equation log k = 15.3-42,500/4.575 K. At 600 K the reaction takes place 18 times faster than the corresponding decomposition of pyruvic acid into carbon dioxide and acetaldehyde. This is consistent with the 4-center process proposed previously for pyruvic acid, in which a partial negative charge develops on the carbon of the α-carbonyl group in the transition state. Benzoylformic acid is considerably less reactive towards thermal elimination than is oxalic acid, which also accords with the proposed mechanism.
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  • 154
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    International Journal of Chemical Kinetics 23 (1991) 
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    Keywords: Chemistry ; Physical Chemistry
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    Topics: Chemistry and Pharmacology
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  • 155
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    International Journal of Chemical Kinetics 23 (1991), S. 251-278 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Stability and sensitivity analysis are used to examine the ignition/reaction characteristics of dilute hydrogen-oxygen mixtures. The analysis confirms the existence of two distinct regions of ignition and fast reaction previously labeled “weak” and “strong” ignition, both of which are located in the explosive pressure-temperature domain and separated by a region related to the “extended” classical second limit. The stability analysis is based on an eigenanalysis of the Green's function matrix of the governing kinetic equations. The magnitudes of the largest (and system controlling) eigenvalue allow the strengths of the two processes to be quantified, giving a clear definition to the terms “weak” and “strong.” The sensitivities of the largest eigenvalue to the reaction rate constants of the mechanism pinpoint the elementary steps controlling the two ignition processes and the subsequent reaction. The associated eigenvectors yield the direction of change in species concentrations and temperature during the course of reaction. These vectors are found to be nearly constant during the induction period of both “weak” and “strong.” ignition, thus producing constant overall stoichiometric reactions. The subsequent reaction of major reactants associated with “weak” ignition also has a constant overall reaction vector, although, different than that during the induction period. However, the vector describing the reaction of major reactants associated with “strong.” ignition is found never to be constant, but continuously changing beyond the induction period.
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  • 156
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    International Journal of Chemical Kinetics 23 (1991), S. 279-288 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics of reaction of amino alcohols viz. 2-aminoethanol, 3-aminopropanol, and triethanolamine with chloramine-T have been studied in perchloric acid medium with palladous chloride as catalyst. The formation of {Pd(II)-(aminoalcohol)} and {Pd(II)-(aminoalcohol)2} complexes and resistance of {Pd(II)-(aminoalcohol)2} complex to react with chloramine-T have been observed. A suitable mechanism consistent with the kinetic data is proposed and discussed.
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  • 157
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    International Journal of Chemical Kinetics 23 (1991), S. 289-313 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The RAPRENOx process for NO reduction in combustion products involves reaction of nitric oxide with isocyanic acid. We have developed a mechanism for the gas-phase reaction of isocyanic acid with nitric oxide in the presence of various amounts of O2, H2O, and CO. Kinetics calculations using the mechanism are compared with the experimental data of Siebers and Caton, and the model reproduces all trends of these data. Sensitivity and rate-of-production analyses show that the reactions of HNCO with OH, O, and H play a major role in the NO-removal process and that NO removal occurs primarily by reaction of NO with NCO to form N2O, which subsequently reacts slowly to form N2. The overall reaction is critically dependent on production of radicals. When O2, H2O, and CO are present, the radicals are supplied by the moist-CO chain branching sequence. When any of these species is absent, radicals must be supplied by other reactions, principally the N2O decomposition reaction and the reaction of the NH2 radical with NO.
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  • 158
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    International Journal of Chemical Kinetics 23 (1991), S. 315-329 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics and the equilibrium constant of the chlorine transfer reaction between monochloramine NH2Cl and the amines: C2H5NH2, (CH3)2CHNH2, (CH3)2NH, and (C2H5)2NH are investigated by spectrophotometry in aqueous medium at 25°C, in the pH range from 8 to 13 and for an ionic strength equal to 1.03 ± 0.05M. For a concentration of total ammonia equal to 1M, the observed rate constant is pH independent below 8 and above 12.8 and reaches a maximum located between the pKas of NH4+ and RR'NH2+. From these results and those obtained earlier for NH2Cl and CH3NH2, the reaction is shown to involve an interaction between neutral molecules NH2Cl and RR'NH, subject to general acid catalysis. The ability of an interaction corresponding to a specific catalysis and involving NH3Cl+ and RR'NH rather than NH2Cl and RR'NH2+ is also discussed. The activation parameters are given for each reaction.
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  • 159
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    International Journal of Chemical Kinetics 23 (1991), S. 331-343 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The mechanism of ozone formation has been studied using 16O and 18O2. High-resolution microwave spectroscopy was used to measure the amounts of the isotopomeric ozone species formed. The study is hampered by the very rapid exchange process between the reactants, that tends to scramble the isotopes and hence give a 2:1 statistical ratio between the two possible isotopomers. We have found a strategy to come around this difficulty and conclude that the mechanism is a simple end-on-addition.
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  • 160
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    International Journal of Chemical Kinetics 23 (1991) 
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    Keywords: Chemistry ; Physical Chemistry
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    Topics: Chemistry and Pharmacology
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  • 161
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    International Journal of Chemical Kinetics 23 (1991), S. 345-359 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Aliphatic amino acids are smoothly oxidized by peroxomonophosphoric acid (PMPA) in the pH region 6-10. Kinetic studies reveal second order dependence in the amino acid not observed hitherto in any of the PMPA oxidations. Dependence in PMPA is unity. Rate-pH profile yields a maximum around pH 8. The reaction path includes oxidation steps due to H2PO5- and HPO52-. Second order dependence in the amino acid has been attributed to participation of two Zwitter-ionic molecules of the amino acid to form a nucleophile.
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  • 162
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    International Journal of Chemical Kinetics 23 (1991), S. 369-375 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Vibrationally excited 1,1-difluorocyclopropane, generated by addition of singlet methylene to 1,1-difluoroethene, reacts according to four reaction channels by isomerization as well as by elimination of difluoromethylene. Identification of the products leads to a critical view on an early study dealing with this reaction system. The pressure dependence of the reaction is investigated. The apparent rate-constants of the reaction paths were determined.
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  • 163
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    International Journal of Chemical Kinetics 23 (1991), S. 361-367 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: CF3 radicals were generated by the photolysis of perfluoroacetic anhydride. In the presence of pentafluorobenzene, the CF3 radicals react according to the following mechanism: It was found that the addition reaction (3) becomes reversible above ca. 453 K. The addition rate parameters have been revised and they satisfactorily agree with those reported previously.At temperatures higher than 593 K, only true H-abstraction occurs. The rate constant kH for reaction (5) is given by: \documentclass{article}\pagestyle{empty}\begin{document}$$ \log [(k_{\rm H} /k_c^{1/2}){\rm mol}^{- 1/2} \,{\rm cm}^{{\rm 3/2}} \,{\rm s}^{{\rm - 1/2}}]\, = \,(4.34\, \pm \,0.43)\, - \,(59,00\, \pm \,2.62)/\theta $$\end{document} where θ = 2.303 RT kJmol-1 and kc is the rate constant for combination of CF3 radicals. The reactions of CF3 with benzene and pentafluorobenzene are compared.
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  • 164
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    International Journal of Chemical Kinetics 23 (1991), S. 377-388 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The stopped-flow measurements on the disappearance of alkaline osmium(VIII) at 402 nm indicated a first-order dependence each in [Os(VIII)] and [HCHO]. The pseudo first-order rate constant kobs ([HCHO] ≫ [Os(VIII)]) decreased with increasing [OH-]. The ionic strength, however, had no effect on kobs. The rapid scan spectra of the reaction mixture indicated the formation of an inert complex which absorbs at 319 nm. Therefore the rate determining step is considered to involve the bimolecular collision between OsO4(OH)22- and hydrated formaldehyde. The values of the rate limiting constant k and the equilibrium constant Kha for the formation of the alkoxide ion from the reaction of hydrated formaldehyde with OH- are evaluated. The equilibrium constant Kha, within the experimental limits, is independent of temperature. The pKa value, calculated from Kha, is 13.62 ± 0.05 which is in good agreement with the pKa value 13.27 for formaldehyde. The activation parameters, ΔH
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  • 165
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    International Journal of Chemical Kinetics 23 (1991), S. 389-395 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The rate of reaction of (Fe(DTPA)) with H2O2 was investigated at various temperatures. The observed rate law is given by the expression.\documentclass{article}\pagestyle{empty}\begin{document}$$ \frac{{- {\rm d[H}_{\rm 2} {\rm O}_{\rm 2} {\rm]}}}{{\rm dt}}\, = \,{\rm kK[FeY(H}_{\rm 2} {\rm O)]}^{{\rm 2 -}} [{\rm H}_{\rm 2} {\rm O}_{\rm 2}]\, + \,{\rm k}_3 {\rm K}_{\rm 1} {\rm K}_{\rm 2} \frac{{{\rm [FeY(OH)]}^{{\rm 3 -}} [{\rm OOH}^{\rm -}]}}{{{\rm [H}^{\rm+}]}} $$\end{document}The rate constants and the related thermodynamic parameters are calculated. Substitution controlled mechanisms are suggested to account for the formation of the violet peroxy intermediate. The results are compared with previously data for Fe EDTA complex.
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  • 166
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    International Journal of Chemical Kinetics 23 (1991), S. 419-429 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The oxidation of thiourea by chlorite within the pH range of 2 to 5.5 has been found to produce a single wave of chlorine dioxide in unstirred solutions. The wave has been studied in narrow tubes of varying diameters and in petri dishes. The wave appears after an induction period that depends on the acid concentration, the [ClO2-]/[CS(NH2)2] ratio, the temperature, and the diameter of the tube. The wave starts from the surface in a tube and from the edges in a petri dish. The rate of wave movement is proportional to the ratio and the acid concentration. Barium chloride and starch were used as indicators. The wave could be initiated electrochemically and by addition of a drop of solution containing chlorine dioxide. The chlorine dioxide is produced by the oxidation of chlorite by hypochlorous acid.
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  • 167
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    International Journal of Chemical Kinetics 23 (1991), S. 431-435 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Cross-disproportionation to combination ratios for CF2H and n-C3H7 radicals have been determined (the hydrogen acceptor radical is given first) to be Δ(n-C3H7, CF2H) = 0.30 ± 0.01 and Δ(CF2H, n-C3H7) = 0.057 ± 0.006.
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  • 168
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    International Journal of Chemical Kinetics 23 (1991), S. 397-417 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Recent shock tube measurements [1,2] of the reactions of OH radicals with various hydrocarbons provide the incentive for revising an earlier model [3] used to carry out thermochemical transition state theory calculations for the reaction rate coefficients of OH radicals with alkanes. In this article, details of the revised model are presented and calculations are described and compared with experiments. Of particular interest is the question of the reliability of an additive formulation for H atom abstraction rate coefficients; i.e., can we evaluate the total rate coefficient as the sum of site-specific rate coefficients, ktotal = ΣinHiki, where we sum either over primary, secondary, and tertiary H atoms or over some larger number of classes of atoms? It is argued that there are two major reasons for expecting different primary, secondary, or tertiary H atoms to have different rate parameters: (1) activation energies may depend on next-nearest neighbors and (2) activation entropies can be mass-dependent. In principle the first factor invalidates the common procedure of treating the total rate coefficient for OH + RH H abstraction processes as the sum of invariant primary, secondary, and tertiary rates multiplied by the respective number of such H atoms in the molecule. The second factor places limits on the accuracy of any additive formulation. A separate question is whether there is sufficient experimental evidence to justify these distinctions, or whether, given experimental and theoretical uncertainties, it is adequate to treat them all as equivalent. It is concluded that (1) mass-dependent variations are just barely discernible; and (2) there are measurable differences among various primary H atom abstractions, and possibly among secondary atoms, but the data base does not justify distinguishing among tertiary H atoms.
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  • 169
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  • 170
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    International Journal of Chemical Kinetics 23 (1991), S. 437-455 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Ethane oxidation in jet-stirred reactor has recently been investigated at high temperature (800-1200 K) in the pressure range 1-10 atm and molecular species (H2, CO, CO2, CH4, C2H2, C2H4, C2H6) concentration profiles were obtained by probe sampling and GC analysis. Ethane oxidation was modeled using a comprehensive kinetic reaction mechanism including the most recent findings concerning the kinetics of the reactions involved in the oxidation of C1—C4 hydrocarbons. The proposed mechanism is able to reproduce experimental data obtained in our high-pressure jet stirred reactor and ignition delay times measured in shock tube in the pressure range 1-13 atm, for temperatures extending from 800 to 2000 K and equivalence ratios of 0.1 to 2. It is also able to reproduce atoms concentrations (H,O) measured in shock tube at ≈2 atm. The same detailed kinetic mechanism can also be used to model the oxidation of methane, ethylene, propyne, and allene in similar conditions.
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    International Journal of Chemical Kinetics 23 (1991), S. 473-482 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: A kinetic study of the silver(I)-catalyzed oxidation of tris(1,10-phenanthroline)iron(II) with peroxodiphosphate was carried out by estimating tris-complex at 510 nm. The reaction is found to conform to the rate law (i). with K2 and K3 being the acid dissociation constants of H3P2O8- and H2P2O82-, respectively. The silver(I) catalysis in the reaction has been explained on the basis of complex formation between pdp and silver(I).
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  • 172
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    International Journal of Chemical Kinetics 23 (1991), S. 457-472 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The flash photolysis of the mono and di-thiocyanate complexes of μ-oxo bis(oxo-molybdenum(V)) (Mo2O4(NCS)x(H2O)6-x(2-x)+ where x = 1, 2) has been studied in the system composed of perchloric acid solutions of Mo2O4(H2O)62+ in the presence of excess thiocyanate.Irradiation with light in the wavelength range 250-340 nm induced the formation of three reaction intermediates identified as μ-oxo-bis (oxo-molybdenum(V)) species: Mo2O3(H2O)84+ (A), Mo2O3(NCS) (H2O)73+ (B), and Mo2O3(NCS)2(H2O)62+ (C). A rapid equilibria between the transient species is established before they decay following a first order kinetics. Intermediate A is the only species effective in promoting the observed decay leading to the end products Mo(VI) and H2.The relative absorption spectrum of species A, B, and C are reported, as well as the measured stability constants for the formation of B and C in the temperature range 20-45°C. An overall mechanism is proposed.
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  • 173
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    International Journal of Chemical Kinetics 23 (1991), S. 483-527 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics of elementary gas phase reactions involved in the oxidation of reduced sulfur species, H2S, CS2, OCS, CH3SH, CH3SCH3, and CH3SSCH3, to SO2 (or other products) are reviewed. The reactions with OH and NO3 which are the processes that initiate the degradation of the above compounds have been evaluated. Reactions of key intermediates, HS, HSO, CH3S, and CH3SO, are discussed. Whenever possible, recommendations for the rate coefficients are made and the need for further work indicated. The review has been carried out with the atmospheric chemistry in mind by looking at the laboratory based kinetics data. This review also provides information that will help model the Earth's sulfur cycle.
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  • 174
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    International Journal of Chemical Kinetics 23 (1991), S. 559-559 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
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  • 175
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    International Journal of Chemical Kinetics 23 (1991), S. 529-539 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The reaction of the (100) face of a gallium arsenide single crystal with atomic and molecular bromine has been studied in a discharge flow system at temperatures between 100 and 225°C and pressures between 0.1 and 40 torr. The reaction with Br2 was found to be first order in Br2 only at pressures below 1 torr. Temperature dependence studies in the linear range gave the activation energy and preexponential factor for the rate controlling reaction in the low pressure regime. The results are summarized in the following Arrhenius equation: \documentclass{article}\pagestyle{empty}\begin{document}$$ k_1 = 10^{\left({4.5 \pm 5} \right)} \mu {\rm m}\ {\rm min}^{- 1}\ {\rm torr}^{- 1} e^{- {{\left({26.6 \pm 4.2{{{\rm kJ}} \mathord{\left/ {\vphantom {{{\rm kJ}} {{\rm mol}}}} \right. \kern-\nulldelimiterspace} {{\rm mol}}}} \right)} \mathord{\left/ {\vphantom {{\left({26.6 \pm 4.2{{{\rm kJ}} \mathord{\left/ {\vphantom {{{\rm kJ}} {{\rm mol}}}} \right. \kern-\nulldelimiterspace} {{\rm mol}}}} \right)} {RT}}} \right. \kern-\nulldelimiterspace} {RT}}} $$\end{document} Deviations from linearity at high pressures are discussed in terms of two alternative mechanisms.The reaction of GaAs with atomic bromine was also studied as a function of temperature, and found to have a temperature dependence described by the following Arrhenius equation: \documentclass{article}\pagestyle{empty}\begin{document}$$ k_3 = \left({2.0 \pm 0.5} \right) \times 10^4 \mu {\rm m}\ {\rm min} ^{- 1}\ {\rm torr}^{- 1} e^{- {{\left({12.9 \pm 0.9} \right){\rm kJ}} \mathord{\left/ {\vphantom {{\left({12.9 \pm 0.9} \right){\rm kJ}} {{{{\rm mol}} \mathord{\left/ {\vphantom {{{\rm mol}} {RT}}} \right. \kern-\nulldelimiterspace} {RT}}}}} \right. \kern-\nulldelimiterspace} {{{{\rm mol}} \mathord{\left/ {\vphantom {{{\rm mol}} {RT}}} \right. \kern-\nulldelimiterspace} {RT}}}}} $$\end{document}
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  • 176
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    International Journal of Chemical Kinetics 23 (1991), S. 553-558 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The high temperature oxidation of ethyl tert-butyl ether (ETBE) with oxygen in argon diluent has been studied in reflected shock waves over the temperature range 1160 to 1830 K, with pressures of 3.5 bar and with varying equivalence ratios from 0.3 to 2.4. Measurements of the ignition delay times, characterized by chemiluminescence and pressure rise, show that the rate of oxidation is very similar to that of methyl tert-butyl ether.
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  • 177
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    International Journal of Chemical Kinetics 23 (1991), S. 541-552 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Rate constants have been measured by pulse radiolysis for the reactions of the carbonate radical, CO3·-, with a number of organic and inorganic reactants as a function of temperature, generally over the range 5 to 80°C. The reactants include the substitution-inert cyano complexes of FeII, MoIV, and WIV, the simple inorganic anions SO32-, ClO2-, NO2-, I-, and SCN-, several phenolates, ascorbate, tryptophan, cysteine, cystine, methionine, triethylamine, and allyl alcohol. The measured rate constants ranged from less than 105 to 3 × 109 M-1 s-1, the activation energies ranged from -11.4 to 18.8 kJ mol-1, and the pre-exponential factors ranged from log A = 6.4 to 10.7. The activation energies for the metal complexes and inorganic anions generally decrease with increasing driving force for the reaction, as expected for an outer sphere electron transfer. For highly exothermic reactions, however, the activation energy appears to increase, probably reflecting the temperature dependence of diffusion. For many of the organic reactants, the activation energies were low and independent of driving force, suggesting that the oxidation is via an inner sphere mechanism.
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  • 178
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    International Journal of Chemical Kinetics 23 (1991) 
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    Keywords: Chemistry ; Physical Chemistry
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    Topics: Chemistry and Pharmacology
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  • 179
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    International Journal of Chemical Kinetics 23 (1991), S. 561-566 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The effects of the concentrations of LiCl, NaCl, KCl, CsCl, Na2CO3, BaCl2, and Me4NCl on the rates of reactions of hydroxide ion with ionized N-hydroxyphthalimide (NHP) at 30°C and in a H2O-MeCN solvent containing 98%, v/v, H2O reveal a nonlinear increase in observed rate constants with increase in salt concentrations. The observed rate constants are highly sensitive to the valence state of cations and almost insensitive to the valence state of anions of the salts. These observations are explained in terms of ion-pair formation between cations and NHP-.
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  • 180
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    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The nucleophilic second-order rate constant (kOH) for the reaction of ŌH with ionized N-hydroxyphthalimide (S-) appears to follow a reaction mechanism similar to that for reactions of ŌH with neutral phthalimide and its N-substituted derivatives. Kinetically indistinguishable terms, k′w[H2O][S-] and kŌH[ŌH][SH] (SH represents nonionized N-hydroxyphthalimide), which constitute the pH-independent rate region of the pH-rate profile, are resolved qualitatively. It is shown that the term kŌH[ŌH][SH], rather than k′w[H2O][S-], is important in these reactions. The rates of ŌH-catalyzed cleavage of S- were studied at 32° in the presence of micelles of sodium dodecyl sulphate (SDS). At a constant [ŌH], the observed pseudo first-order rate constants (kobs) increase linearly with [SDS]T (total SDS concentration). These data are explained in terms of the pseudophase model of micellar effects on reactivity. The linear dependence of kobs with [SDS]T (within [SDS]T range of 0.0-0.2 or 0.3 M) is attributed to the occurrence of the reaction between the exterior boundary of Stern layer and Gouy-Chapman layer.
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  • 181
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    International Journal of Chemical Kinetics 23 (1991), S. 579-591 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics of the reactions of IO, BrO, and ClO with DMS have been investigated at 298 K and total pressures of 0.5-6.8 mbar He using the discharge flow-mass spectrometry technique to monitor the halogen oxide radicals. Rate coefficients of (8.8 ± 2.1) × 10-15, (2.7 - 0.5) × 10-13 and (9.5 ± 2.0) × 10-15 cm3 molecule-1 s-1 have been obtained for the reactions of IO, BrO, and ClO with DMS, respectively. The result for IO with DMS is in good agreement with two other recent studies on this reaction but is nearly three orders of magnitude slower than two earlier studies, one of which was from this laboratory. The earlier studies are now thought to be in error because of heterogeneous and secondary chemistry occurring in the systems investigated. The rate coefficient for BrO with DMS is in excellent agreement with a previously reported preliminary value from this laboratory. However, the rate coefficient for ClO with DMS is a factor of 4 lower than our previously determined value. The new data are considered more reliable in view of the much improved experimental technique in the present study. DMSO was detected as a product in all of these reactions. A semi-quantitative determination of the DMSO yield was only possible in the case of the reaction of IO with DMS where a yield of 84 ± 40% was found.
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  • 182
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    International Journal of Chemical Kinetics 23 (1991), S. 593-605 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The oxidation of L-Phenylalanine by permanganate ion in aqueous phosphate buffers is autocatalized by the inorganic reaction product, which is stabilized in solution by adsorption of phosphate ions on its surface. This product is a soluble form of colloidal manganese dioxide. The rate of the noncatalytic reaction pathway is first-order in both the oxidizing and reducing agent. It is not affected by potassium chloride addition to the solution, but by phosphate addition. The rate increases with the pH of the medium. The autocatalytic pathway is first-order in both permanganate ion and colloidal manganese dioxide, (the permanganate ion according to the Langmuir isotherm). The autocatalytic rate increases with reductant concentration (follows the Langmuir adsorption isotherm). It is not affected by potassium chloride addition to the solution, whereas an increase in the phosphate concentration results in an increase in the rate with the same pH of the medium. Mechanisms consistent with the experimental data are proposed.
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  • 183
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    Keywords: Chemistry ; Physical Chemistry
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    Topics: Chemistry and Pharmacology
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  • 184
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    International Journal of Chemical Kinetics 23 (1991), S. 669-681 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The oxidation of phosphinic, phenylphosphinic, and phosphorous acids by N-bromoacetamide (NBA) in acid solution, results in the formation of corresponding higher oxyacids of phosphorus. The reaction is first order with respect to NBA, second order in the oxyacid and inverse first in hydrogen ions. The oxidation of deuteriated phosphorus oxyacids showed the presence of a substantial primary kinetic isotope effect. The reaction failed to induce polymerization of acrylonitrile. Added acetamide has no effect on the reaction rate. It has been shown that the ‘inactive’ tautomer of the phosphorus oxyacids, RHP(O)OH, participates in the oxidation process. A rate-determining step involving transfer of a hydride ion from the P—H bond to the oxidant has been proposed.
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  • 185
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    International Journal of Chemical Kinetics 23 (1991), S. 683-700 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The thermochemical kinetics formulation of conventional transition state theory has been applied to metathesis reactions of H atoms with a series of alkanes in order to provide a sound framework for the intercomparison of experimental data, and also to extrapolate rate coefficients to temperature regimes that may lie beyond the range of experiments. The calculations require a value for the rate coefficient at some temperature, necessitating a discussion of the extant experimental data and their reliability. The procedures are described, the results of the calculations are presented, and their agreement with experimental data (for methane, ethane, propane, butane, pentane, isobutane, cyclopropane, cyclohexane, neopentane, neooctane, and 2,2,3-trimethylbutane) is discussed. A general expression for reactions of H with large (more than 4 carbons) alkanes is proposed: \documentclass{article}\pagestyle{empty}\begin{document}$$ \begin{array}{rcl} k({\rm T}) &=& 5.4\, \times\, 10^3 n_p {\rm T}^{{\rm 2.0}} \exp (- 3540/{\rm T)}\, +\, 4.7\, \times\, 10^3 n_s {\rm T}^{{\rm 2}{\rm .2}} \exp (- 2640/{\rm T)}\\ \,\,&+&\, 3.7\, \times\, 10^3 n_t {\rm T}^{{\rm 2}{\rm .0}} \exp (- 970/{\rm T),} \end{array} $$\end{document} where np, ns, and nt are the numbers of primary, secondary, and tertiary H atoms available for abstraction.
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  • 186
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    International Journal of Chemical Kinetics 23 (1991), S. 655-668 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The reaction of atomic hydrogen with isocyanic acid (HNCO) to produce the amidogen radical (NH2) and carbon monoxide, has been studied in shock-heated mixtures of HNCO dilute in argon. Time-histories of the ground-state NH2 radical were measured behind reflected shock waves using cw, narrowlinewidth laser absorption at 597 nm, and HNCO time-histories were measured using infrared emission from the fundamental v2-band of HNCO near 5 μm. The second-order rate coefficient of reaction (2(a)) was determined to be: \documentclass{article}\pagestyle{empty}\begin{document}$$ \begin{array}{*{20}c} {k_{2a} = 2.1 \times 10^{14}\, {\rm exp(- 8500/T,K)}} & {{\rm (f} = 0.5,{\rm F} = 1.75)} & {{\rm T = 2340} - {\rm 3270\,K,}} \\ \end{array} $$\end{document} cm3 mol-1 s-1, where f and F define the lower and upper uncertainty limits, respectively.An upper limit on the rate coefficient of was determined to be: \documentclass{article}\pagestyle{empty}\begin{document}$$ \begin{array}{*{20}c} {k_5 \le 5.0 \times 10^{11} {\rm cm}^{\rm 3}\, {\rm mol}^{{\rm - 1}} {\rm s}^{{\rm - 1}},} & {{\rm T} = 2340 - 2680\,{\rm K}{\rm .}} \\ \end{array} $$\end{document}
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  • 187
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    International Journal of Chemical Kinetics 23 (1991), S. 701-715 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Rate coefficients of the termolecular reaction \documentclass{article}\pagestyle{empty}\begin{document}$$ {\rm CF}_2 {\rm ClO}_2 + {\rm NO}_{\rm 2} + {\rm M} \longrightarrow {\rm CF}_2 {\rm ClO}_2 {\rm NO}_2 + {\rm M} $$\end{document} were determined over the temperature range of 248-324 K and at pressures from 1 to 10 torr by time resolved mass spectrometry. CF2ClO2 radicals were generated by flash photolysis of CF2ClBr in the presence of oxygen. Their rate of decay was measured by following (CF2O2)+ fragment ions formed in the ion source. With 2 to 40 mtorr of NO2 present the dominant removal pathway is addition to form the peroxynitrate. The third order rate coefficients are wholly within the falloff over the experimental pressure range, and have a negative temperature coefficient. Rate constants for the reverse reaction, the unimolecular dissociation of CF2ClO2NO2, D. Koppenkastrop and F. Zabel, Int. J. Chem. Kinet., 23, 1 (1991) were employed to calculate equilibrium constants, from which a 600 torr value of the combination rate coefficient was obtained at each temperature. From the temperature dependence of the equilibrium constants, the average enthalpy of reaction over the experimental temperature range was found to be 106.1 ± 0.3 kJ/mol. Extrapolation of the combination rate constants to lower and higher pressures, and estimates of low and high pressure limiting rate coefficients, k0 and k∞ were done by nonlinear least squares fit of the experimental data, using the empirical Fc equations developed by Troe.
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  • 188
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    Topics: Chemistry and Pharmacology
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  • 189
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    International Journal of Chemical Kinetics 23 (1991), S. 717-732 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The kinetics of the reaction between permanganate ion and triethylamine in aqueous phosphate buffers (pH 6-8) has been studied. The reaction is autocatalytic, a soluble form of colloidal manganese dioxide temporarily stabilized in solution by adsorption of phosphate ions on its surface having been identified as the autocatalyst. The reaction is also catalyzed by gum arabic. Mechanisms in agreement with the kinetic data are proposed for the reaction pathways taking place in the bulk solution (for both triethylamine and triethylammonium ion as reductants) and on both the gum arabic and manganese dioxide colloidal particles.
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  • 190
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    International Journal of Chemical Kinetics 23 (1991), S. 837-852 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The alkanolysis of ionized phenyl salicylate, PS-, has been studied in the presence and absence of micelles of sodium dodecyl sulphate, SDS, at 0.05 M NaOH, 30 or 32°C and within the alkanol, ROH, (ROH = HOCH2CH2OH and CH3OH) contents of 15-74 or 92%, v/v. The alkanolysis of PS- involves intramolecular general base catalysis. At a constant concentration of SDS, [SDS]T, the observed pseudo first-order rate constants, kobs, for the reactions of ROH with PS- obtained at different concentration of ROH, [ROH]T, obey the relationship: kobs = k[ROH]T/(1 + KA[ROH]T) where k is the apparent second-order rate constant and KA is the association constant for dimerization of ROH molecules. Both k and KA decrease with increase in [SDS]T. At a constant [ROH]T, the rate constants, kobs, show a decrease of nearly 2-fold with increase in [SDS]T from 0.0-0.3M. These results are explained in terms of pseudo-phase model of micelle. The rate constants for alkanolysis of PS- in micellar pseudophase are insignificant compared with the corresponding rate constants in aqueous-alkanol pseudophase. This is attributed largely to considerably low value of [ROH] in the specific micellar environment where micellar bound PS- molecules exist. The increase in [ROH]T decrease the value of the binding constant of PS- with SDS micelle. The effects of anionic micelles on the rates of alkanolysis of PS- are explained in terms of the porous cluster micellar structure.
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  • 191
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    International Journal of Chemical Kinetics 23 (1991), S. 853-860 
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    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Ring-opening radical polymerization has been followed by the flash photolysis method. As an initiator radical, the arylthiyl radical (ArS·) was used; the addition reaction rate constants of ArS· to vinyl monomer containing epoxy-ring such as vinyloxiranes have been determined at first. The rate constant of ring opening reaction of the adduct radical changing to ArSCH2CH = CROCH2· were determined in the form of the relative values, which were converted to the absolute values. The ring-opening reaction rate constants were ca. 106 s-1, which indicates that the ring-opening rates are faster than usual radical propagation rates. The rate constants for vinyl monomer with 5-member ring (1,4-epoxy-1,4-dihydronaphthalene) were similarly evaluated.
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  • 192
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    International Journal of Chemical Kinetics 23 (1991), S. 861-879 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: An experimental investigation in a conventional static apparatus of the oxidation of equimolecular mixtures 1,4-dioxane-O2 has shown that 1,4-dioxane reacts with oxygen more readily than most hydrocarbons. Cool flames and ignitions were observed above 200°C in a pressure range up to 300 torr.The products of the slow reaction and cool flame were analyzed by gas chromatography and GC-MS; the slow reaction gives only CO, CO2, H2CO, H2, C2H4, and H2O.A radical chain mechanism is suggested and discussed by using an evaluation of the rate constants of the possible elementary steps by the methods of thermochemical kinetics.
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  • 193
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    International Journal of Chemical Kinetics 23 (1991), S. 881-896 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Oscillatory change of pH occurs during the chromate-catalyzed decomposition of hydrogen peroxide in a weakly acidic medium at elevated temperature and at high initial concentration of hydrogen peroxide. In a closed system, there are only two or three periods, but sustained oscillation occurs in a CSTR. In a CSTR bistability is also found. In closed systems the temperature exhibits a great maximum (up to 15°C increase), in a CSTR sustained oscillation occurs at a constant stationary temperature.
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  • 194
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    International Journal of Chemical Kinetics 23 (1991), S. 897-906 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Rate constants for the gas-phase reactions of the biogenically emitted monoterpene β-phellandrene with OH and NO3 radicals and O3 have been measured at 297 ± 2 K and atmospheric pressure of air using relative rate methods. The rate constants obtained were (in cm3 molecule-1 s-1 units): for reaction with the OH radical, (1.68 ± 0.41) × 10-10; for reaction with the NO3 radical, (7.96 ± 2.82) × 10-12; and for reaction with O3, (4.77 ± 1.23) × 10-17, where the error limits include the estimated uncertainties in the reference reaction rate constants. Using these rate constants, the lifetime of β-phellandrene in the lower troposphere due to reaction with these species is calculated to be in the range of ca. 1-8 h, with the OH radical reaction being expected to dominate over the O3 reaction as a loss process for β-phellandrene during daylight hours.
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  • 195
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    International Journal of Chemical Kinetics 23 (1991), S. 925-939 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The chemical reaction of 2,5-dimethylpyrrole (C6H9N) with O2(1Δg) was studied in the gas phase in an isothermal flow reactor at room temperature and low pressures. The C6H9N concentration profiles were studied under pseudo-first order conditions [C6H9N]∘ ≪ [O2(1Δg)] with mass-spectrometric detection of C6H9N. O2(1Δg) was produced either in a microwave discharge or in a chemical reaction. The value for the rate constant: \documentclass{article}\pagestyle{empty}\begin{document}$$ k_{1c} (298{\rm K)} = (1.0 \pm 0.3)10^{11} {\rm cm}^{\rm 3} \cdot {\rm mol}^{ - {\rm 1}} \cdot {\rm s}^{ - {\rm 1}} $$\end{document} was measured.The rate constant is compared to the value obtained for the quenching process. The primary product C6H9NO2 was detected by mass spectrometry and the reaction mechanism is proposed. The possibility of using this reaction as a gas phase titration reaction for O2(1Δg) is discussed.
    Additional Material: 7 Ill.
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  • 196
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 907-924 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Methyl tertiary butyl ether (MTBE) has been proposed and is being used as an additive to increase the octane of gasoline without the use of tetraethyl lead and alkylbenzenes. The present experiments have been performed to examine the kinetics and mechanisms of the atmospheric removal of MTBE. The kinetics of the reaction of OH with MTBE was examined by using a relative rate technique in which photolysis of methyl nitrite was used as the source of OH. With n-butane as the reference compound a value of (2.99 ± 0.12) × 10-12 cm3 molecule-1 s-1 at a temperature of 298 K was obtained for the rate constant. The products (and product yields) for the OH reaction with MTBE in the presence of NOx were also determined and found to be t-butyl formate (0.68 ± 0.05), methyl acetate (0.14 ± 0.02), acetone (0.026 ± 0.003), t-butanol (0.062 ± 0.009), and formaldehyde (0.48 ± 0.05) in mols/mol MTBE converted. The OH rate constant for the major product formed, t-butyl formate was also measured and found to be (7.37 ± 0.05) × 10-13 cm3 molecule-1 s-1. Mechanisms to rationalize the formation of the products are presented.
    Additional Material: 5 Ill.
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  • 197
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    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 941-946 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Perfluorobutylperoxyl radicals were produced by radiolytic reduction of perfluorobutyl iodide in aerated methanol solutions. Rate constants for the reactions of this peroxyl radical with various organic compounds were determined by kinetic spectrophotometric pulse radiolysis. The rate constants for alkanes and alkenes were determined by competition kinetics using chlorpromazine as a reference. The results indicate that hydrogen abstraction from aliphatic compounds takes place with a rate constant that is too slow to measure in our system (〈105 M-1 s-1), and that abstraction of allylic and doubly allylic hydrogens is slow compared with addition. Addition to alkenes takes place with rate constants of the order of k = 106 - 108 M-1 s-1. Good correlation was obtained between log k and the Taft substituent constants σ* for the various substituents on the double bond. Perfluorobutylperoxyl radical is found to be more reactive than trichloromethylperoxyl and other peroxyl radicals.
    Additional Material: 1 Ill.
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  • 198
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991) 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Type of Medium: Electronic Resource
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  • 199
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    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 947-956 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The unimolecular decomposition of 1,3,5-trioxane into three formaldehyde molecules has been studied thermally at eight temperatures between 523 and 603 K using mixtures highly diluted with Ar. Under these conditions, the only decomposition product detected by means of FTIR analysis was formaldehyde. At 588 K, the effect of total pressure was examined between 25 and 800 torr; a noticeable decline in the first-order rate constant was observed only at pressures below 500 torr. A least-squares analysis of the measured high-pressure, first-order rate constants leads to \documentclass{article}\pagestyle{empty}\begin{document}$$ k_1 = 10^{15.78 \pm 0.19} \exp [(- 25,620 \pm 254)/{\rm T]s}^{ - {\rm 1}} . $$\end{document} This result differs significantly from earlier data on the reaction, but it compares closely with the theoretical value: \documentclass{article}\pagestyle{empty}\begin{document}$$ k_1 ({\rm BAC} - {\rm MP}4) = 10^{15.67 \pm 0.01} \exp [(- 25,760 \pm 20)/{\rm T]s}^{ - {\rm 1}} . $$\end{document} computed with the transition-state theory using the molecular and TST parameters predicted by the BAC-MP4 method.
    Additional Material: 5 Ill.
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  • 200
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    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 23 (1991), S. 957-970 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: As part of an ongoing program to model hydrocarbon assisted boron combustion, a kinetic model has been developed to describe gasification of the ubiquitous boron oxide coating that inhibits particulate boron ignition. This model includes homogeneous gas phase oxidation reactions, multi-component gas phase diffusion, heterogeneous surface reactions, and oxide vaporization. The kinetic processes are treated using a generalized kinetics code, with embeded sensitivity analysis, for the combustion of a one-dimensional (particle radius), spherical particle.This article presents the heterogeneous surface reactions used to describe oxide gasification and presents selected model results for a spherical boron oxide droplet which illustrate the dependence of the oxide gasification rates on the ambient temperature and particle diameter.
    Additional Material: 6 Ill.
    Type of Medium: Electronic Resource
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