Mechanism of gas-phase oxidation of hydrogen sulfide at high temperatures

Chernysheva, A. V.; Basevich, V. Ya.; Vedeneev, V. I.; Arutyunov, V. S.

doi:10.1007/bf00958236

Cited by 9 publications

(8 citation statements)

References 38 publications

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“…The authors noted that their value for this rate coefficient was smaller than other experimental expressions and cautioned that using a larger one would require changes in their Arrhenius expressions for reactions 14a and 14b. Chernysheva et al (1990) developed an elaborate mechanism for the H2S-02 system by estimating many of the needed rate coefficients. 2 S reactions, It was used to interpret a number of previous experimental studies, including the ignition delay experiments of Frenklach et al (1981), data on H2S-02 explosion limits, and conversion of H2S to sulfur in the Claus process (Tesner et al 1984).…”

Section: Sulfur Reaction Studies In Shock Tubesmentioning

confidence: 99%

Kinetics and Mechanisms of the Oxidation of Gaseous Sulfur Compounds

Hynes

Wine

2000

Gas-Phase Combustion Chemistry

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Section: Sulfur Reaction Studies In Shock Tubesmentioning

confidence: 99%

Kinetics and Mechanisms of the Oxidation of Gaseous Sulfur Compounds

Hynes

Wine

2000

Gas-Phase Combustion Chemistry

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“…Early modeling efforts for H 2 S oxidation largely had to rely on estimated rate constants for the sulfur subset. More recently, Haynes and coworkers investigated the chemistry of H 2 S pyrolysis and oxidation in a series of modeling studies , supported by ab initio calculations for key reactions .…”

Section: Introductionmentioning

confidence: 99%

An Exploratory Flow Reactor Study of H₂S Oxidation at 30–100 Bar

Song

Hashemi

Christensen

et al. 2016

Int J of Chemical Kinetics

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Hydrogen sulfide oxidation experiments were conducted in O2/N2 at high pressure (30 and 100 bar) under oxidizing and stoichiometric conditions. Temperatures ranged from 450 to 925 K, with residence times of 3–20 s. Under stoichiometric conditions, the oxidation of H2S was initiated at 600 K and almost completed at 900 K. Under oxidizing conditions, the onset temperature for reaction was 500–550 K, depending on pressure and residence time, with full oxidization to SO2 at 550–600 K. Similar results were obtained in quartz and alumina tubes, indicating little influence of surface chemistry. The data were interpreted in terms of a detailed chemical kinetic model. The rate constants for selected reactions, including SH + O2 ⇄ SO2 + H, were determined from ab initio calculations. Modeling predictions generally overpredicted the temperature for onset of reaction. Calculations were sensitive to reactions of the comparatively unreactive SH radical. Under stoichiometric conditions, the oxidation rate was mostly controlled by the SH + SH branching ratio to form H2S + S (promoting reaction) and HSSH (terminating). Further work is desirable on the SH + SH recombination and on subsequent reactions in the S2 subset of the mechanism. Under oxidizing conditions, a high O2 concentration (augmented by the high pressure) causes the termolecular reaction SH + O2 + O2 → HSO + O3 to become the major consumption step for SH, according to the model. Consequently, calculations become very sensitive to the rate constant and product channels for the H2S + O3 reaction, which are currently not well established.

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“…It includes 22 reactions of which 15 are reversible. The initial kinetic parameters are essentially from Basevitch et al., Chnerysheva et al, and the NIST database, and the thermochemical data used are from Burcat and McBride's database …”

Section: Kinetic Modelingmentioning

confidence: 99%

Kinetic Study of the Pyrolysis of H₂S

Binoist¹,

Labegorre²,

Monnet³

et al. 2003

Ind. Eng. Chem. Res.

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The pyrolysis of hydrogen sulfide has been studied at residence times between 0.4 and 1.6 s and in the temperature range of 800−1100 °C. A continuous perfectly mixed quartz reactor was used to acquire kinetic data on the thermal dissociation of hydrogen sulfide and elemental sulfur mixtures diluted in argon (95 vol %). The kinetic auto-acceleration effect of sulfur is demonstrated. A detailed radical mechanism is written to account for the experimental results, in particular for the auto-acceleration effect, and validated against experimental results. This pyrolysis kinetic scheme is the first step and core of a complete detailed mechanism capable of modeling the various oxidation reactions encountered in an industrial Claus furnace.

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Mechanism of gas-phase oxidation of hydrogen sulfide at high temperatures

Cited by 9 publications

References 38 publications

Kinetics and Mechanisms of the Oxidation of Gaseous Sulfur Compounds

Kinetics and Mechanisms of the Oxidation of Gaseous Sulfur Compounds

An Exploratory Flow Reactor Study of H₂S Oxidation at 30–100 Bar

Kinetic Study of the Pyrolysis of H₂S

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Mechanism of gas-phase oxidation of hydrogen sulfide at high temperatures

Cited by 9 publications

References 38 publications

Kinetics and Mechanisms of the Oxidation of Gaseous Sulfur Compounds

Kinetics and Mechanisms of the Oxidation of Gaseous Sulfur Compounds

An Exploratory Flow Reactor Study of H2S Oxidation at 30–100 Bar

Kinetic Study of the Pyrolysis of H2S

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Product

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An Exploratory Flow Reactor Study of H₂S Oxidation at 30–100 Bar

Kinetic Study of the Pyrolysis of H₂S