Gas-Phase Reactions

Kondratiev, Victor N.; Nikitin, E. E.

doi:10.1007/978-3-642-67608-6

Cited by 67 publications

(16 citation statements)

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“…To date, the growth theory of CVD is complex and controversial. 26 Chloromethylsilane containing Si and C is commonly used to produce SiC, as described in eq 1. In detail, the Si crystallites are first pyrolyzed from chloromethylsilane at high temperatures (eq 2), and subsequently, the C crystallites are generated from CH 3 (eq 3).…”

Section: Resultsmentioning

confidence: 99%

Large-Scale Production of a Silicon Nanowire/Graphite Composites Anode via the CVD Method for High-Performance Lithium-Ion Batteries

et al. 2021

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Aiming at preparing a cheap and high-performance anode material, a novel carbon-coated silicon nanowire on a surface of graphite microsphere composites was fabricated by employing a new silicon precursor via the chemical vapor deposition method. The chemical vapor deposition method could further reduce the cost and realize the large-scale preparation of silicon/graphite composites and simultaneously enhance the bonding strength between silicon and graphite. Due to the lower cost and lower requirement on equipment compared with silane, chloromethylsilane was selected to produce pure silicon as the content of carrier gas is 25 vol %. Deposited with silicon and carbon for 15 and 30 min, respectively, the carbon/silicon nanowire/graphite microsphere composites display outstanding electrochemical performance with a specific capacity of 580 mA h g–1 at a current density of 0.2 C after 100 cycles and high-rate performance of 300 mA h g–1 at 5 C. Besides, the adsorption and deposition mechanisms of silicon on a graphite surface are expounded. This new preparation process is an alternative route for promoting the practical application of silicon/graphite composites.

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Section: Resultsmentioning

confidence: 99%

Large-Scale Production of a Silicon Nanowire/Graphite Composites Anode via the CVD Method for High-Performance Lithium-Ion Batteries

et al. 2021

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“…The paper in a certain sense is the continuation of our previous works [2] [16]. In terms of the proposed model, the chain branching H + O 2 → O + OH and inhibiting H + O 2 + M → HO 2 + M formal reactions are considered as the set of elementary processes of forming, intramolecular energy redistribution between modes [16], relaxation, and monomolecular decay of the comparatively long-lived (see [18]- [21]) 4 vibrationally excited HO 2 (v) radical which moreover is capable to react and to exchange an energy with other components of the mixture. This significantly changes the physical understanding of the chemical mechanism in the reacting hydrogen-oxygen system.…”

Section: Introductionmentioning

confidence: 94%

“…(It is these circumstances that are the 1 The use of the formal kinetic description was and remains relevant in terms of its use in macro-kinetic applications, i.e., when it is enough to quantitatively correctly simulate the density and "heat release function" in the specific conditions of composition, temperature, and pressure. 2 According to existing concepts (see, for example, [4]), if molecules or radicals AB are 2-atomics (O2, H2, OH, •••), such a reaction proceeds in two the following elementary steps: forming vibrationally excited AB(v) and its subsequent relaxation to equilibrium distribution on vibrational states (in this case, deactivation in collisions). If the AB are 3(or more)-atomics (HO2, H2O, H2O2, •••) such a reaction proceeds in three following elementary steps: forming vibrationally excited AB(v), intramolecular energy redistribution, and relaxation.…”

Section: Introductionmentioning

confidence: 99%

“…The inability of the equilibrium kinetics concept to predict efficiencies of different third bodies, M, in recombination-dissociation reactions; the possibility of formation of electronically excited states O2( 1 ∆), O( 1 D), OH( 2 Σ + ), reactions with their participation, the complex multichannel character of quenching processes, including the chemical quenching processes (see[2]). 4 i.e., there is an overlap of the HO2(v) lifetime and collision time statistical distributions.…”

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Vibrational Nonequilibrium in the Hydrogen-Oxygen Reaction at Different Temperatures

Skrebkov¹

2014

JMP

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A theoretical model of chemical and vibrational kinetics of hydrogen oxidation is suggested based on the consistent account for the vibrational nonequilibrium of HO2 radical which forms in result of bimolecular recombination H + O2 = HO2 in the vibrationally excited state. The chain branching H + O2 = O + OH and inhibiting H + O2 + M = HO2 + M formal reactions are considered (in the terms of elementary processes) as a general multi-channel process of forming, intramolecular energy redistribution between modes, relaxation, and monomolecular decay of the comparatively long-lived vibrationally excited HO2 radical which is capable to react and exchange of energy with another components of the mixture. The model takes into account the vibrational nonequilibrium for the starting (primary) H2 and O2 molecules, as well as the most important molecular intermediates HO2, OH, O2(1 ∆), and the main reaction product H2O. The calculated results are compared with the shock tube experimental data for strongly diluted H2-O2 mixtures at 1000 < T < 2500 K, 0.5 < p < 4 atm. It is demonstrated that this approach is promising from the standpoint of reconciling the predictions of the theoretical model with experimental data obtained by different authors for various compositions and conditions using different methods. It is shown that the hydrogen-oxygen reaction proceeds in absence of vibrational equilibrium, and the vibrationally excited HO2 radical acts as a key intermediate in the principally important chain branching process. For T < 1500 K, the nature of hydrogen-oxygen reaction is especially nonequilibrium, and the vibrational nonequilibrium of HO2 radical is the essence of this process.

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“…There are two major problems with the Krasnopolsky and Parshev model. First, the equilibrium constant for clcO in the compilation from which they drew their laboratory data [Kondratiev, 1971] was incorrect due to a typographical error and implied clcO was two orders of magnitude more stable than laboratory studies had found. Second, independent laboratory studies [Yung and DeMore, 1982] found the mechanism postulated for reaction (28) was incorrect.…”

Section: Chlorine Chemistrymentioning

confidence: 99%