Publication

Role of adsorbed NO in N2O decomposition over iron containing ZSM-5 catalysts at low temperatures

Albert Renken, Lioubov Kiwi
2006
Journal Articles

Abstract

Transient response and temperature-programmed desorption/reaction (TPD/TPR) methods were used to study the formation of adsorbed NOx from N2O and its effect during N2O decomposition to O2 and N2 over FeZSM-5 catalysts at temperatures below 653 K. The reaction proceeds via the atomic oxygen (O)Fe loading from N2O on extraframework active Fe(II) sites followed by its recombination/desorption as the rate-limiting step. The slow formation of surface NOx,ads species was observed from N2O catalyzing the N2O decomposition. This autocatalytic effect was assigned to the formation of NO2,ads species from NOads and (O)Fe leading to facilitation of (O)Fe recombination/desorption. Mononitrosyl Fe2+(NO) and nitro (NO2,ads) species were found by diffuse reflectance infrared fourier transform spectroscopy (DRIFTS) in situ at 603 K when N2O was introduced into NO-containing flow passing through the catalyst. The presence of NOx,ads does not inhibit the surface oxygen loading from N2O at 523 K as observed by transient response. However, the reactivity of (O)Fe toward CO oxidation at low temperatures (

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Albert Renken, Lioubov Kiwi
2006
Journal Articles

Abstract

Official source

https://infoscience.epfl.ch/entities/publication/9a7590cf-bdf6-4ff4-a23f-5dc38a13b521

About this result

Related concepts (32)

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Oxygen is the chemical element with the symbol O and atomic number 8. It is a member of the chalcogen group in the periodic table, a highly reactive nonmetal, and an oxidizing agent that readily forms oxides with most elements as well as with other compounds. Oxygen is Earth's most abundant element, and after hydrogen and helium, it is the third-most abundant element in the universe. At standard temperature and pressure, two atoms of the element bind to form dioxygen, a colorless and odorless diatomic gas with the formula O2.

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In chemical kinetics, the overall rate of a reaction is often approximately determined by the slowest step, known as the rate-determining step (RDS or RD-step or r/d step) or rate-limiting step. For a given reaction mechanism, the prediction of the corresponding rate equation (for comparison with the experimental rate law) is often simplified by using this approximation of the rate-determining step. In principle, the time evolution of the reactant and product concentrations can be determined from the set of simultaneous rate equations for the individual steps of the mechanism, one for each step.

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