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Relevant bibliographies by topics / Hydrogen peroxide ; Chemical reactions

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Journal articles

Academic literature on the topic 'Hydrogen peroxide ; Chemical reactions'

Author: Grafiati

Published: 4 June 2021

Last updated: 11 February 2022

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Journal articles on the topic "Hydrogen peroxide ; Chemical reactions"

1

Jacob, Peter, Bernhard Wehling, Wieland Hill, and Dieter Klockow. "Feasibility Study of Raman Spectroscopy as a Tool to Investigate the Liquid-Phase Chemistry of Aliphatic Organic Peroxides." Applied Spectroscopy 51, no. 1 (1997): 74–80. http://dx.doi.org/10.1366/0003702971938795.

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The described investigations are focused on peroxides occurring as products in atmospheric chemical processes, namely, hydrogen peroxide, methylhydroperoxide, hydroxymethylhydroperoxide, bis-(hydroxymethyl)peroxide, 1-hydroxyethylhydroperoxide, bis-(hydroxyethyl)peroxide, and hydroxymethylmethylperoxide. The compounds are identified and determined through the position and intensity of their characteristic O–O stretching bands in the range between 767 and 878 cm−1. Time-resolved Raman spectroscopy of peroxide solutions permits the in situ investigation of pathways and kinetics of reactions betw

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2

Di Menno Di Bucchianico, Daniele, Wander Y. Perez-Sena, Valeria Casson Moreno, Tapio Salmi та Sébastien Leveneur. "Model Discrimination for Hydrogen Peroxide Consumption towards γ-Alumina in Homogeneous Liquid and Heterogeneous Liquid-Liquid Systems". Processes 9, № 8 (2021): 1476. http://dx.doi.org/10.3390/pr9081476.

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The use of hydrogen peroxide as an oxidizing agent becomes increasingly important in chemistry. The example of vegetable oil epoxidation is an excellent illustration of the potential of such an agent. This reaction is traditionally performed by Prileschajew oxidation, i.e., by the in situ production of percarboxylic acids. Drawbacks of this approach are side reactions of ring-opening and thermal runaway reactions due to percarboxylic acid instability. One way to overcome this issue is the direct epoxidation by hydrogen peroxide by using γ-alumina. However, the reaction mechanism is not elucida

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3

Pędziwiatr, Paulina, Filip Mikołajczyk, Dawid Zawadzki, Kinga Mikołajczyk, and Agnieszka Bedka. "Decomposition of hydrogen peroxide - kinetics and review of chosen catalysts." Acta Innovations, no. 26 (January 1, 2018): 45–52. http://dx.doi.org/10.32933/actainnovations.26.5.

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Hydrogen peroxide is a chemical used in oxidation reactions, treatment of various inorganic and organic pollutants, bleaching processes in pulp, paper and textile industries and for various disinfection applications. It is a monopropellant, which, when purified, is self-decomposing at high temperatures or when a catalyst is present. Decomposing to yield only oxygen and water(disproportionation), hydrogen peroxide is one of the cleanest, most versatile chemicals available. The catalytic decomposition of hydrogen peroxide allows the use of various catalysts that will increase the rate of decompo

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4

Øiestad, Elisabeth Leere, Jeremy N. Harvey, and Einar Uggerud. "Unimolecular Reactions of Protonated Hydrogen Peroxide: A Quantum Chemical Survey." Journal of Physical Chemistry A 104, no. 36 (2000): 8382–88. http://dx.doi.org/10.1021/jp000480g.

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5

Ibragimova, D. A., O. M. Kamil, T. V. Yankova, N. A. Yashtulov, and N. K. Zaitsev. "THE EFFECT OF SURFACTANTS ON THE CHEMILUMINESCENT REACTION OF LUMINOL WITH HYDROGEN PEROXIDE." Fine Chemical Technologies 12, no. 6 (2017): 71–76. http://dx.doi.org/10.32362/2410-6593-2017-12-6-71-76.

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The luminol-hydrogen peroxide chemiluminescent system is widely used for the creation of diagnostic systems, for chemical analysis, for studying the kinetics and mechanisms of chemical reactions, for the creation of special and emergency light sources, and for monitoring living systems. However, the use of the luminol-hydrogen peroxide chemiluminescent system is limited by the fact that there are almost no ways of managing the reaction. The introduction of organized molecular systems into the luminol-hydrogen peroxide chemiluminescent system can create an additional channel for controlling che

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6

Sun, Yujun, Michael Fenster, Annie Yu, Richard M. Berry, and Dimitris S. Argyropoulos. "The effect of metal ions on the reaction of hydrogen peroxide with Kraft lignin model compounds." Canadian Journal of Chemistry 77, no. 5-6 (1999): 667–75. http://dx.doi.org/10.1139/v99-036.

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Peroxide bleaching is significantly affected by transition and alkaline earth metals. Isolating the effects of different transition and alkaline earth metals on the reactions of peroxide with different representative lignin structures allows the separation of the positive from the negative contributions of these metal ions. In this work, five monomeric or dimeric phenolic lignin model compounds were treated with alkaline hydrogen peroxide in the absence or presence of Mn2+, Cu2+, Fe3+, and Mg2+. We followed the disappearance of the starting material and the progress of demethylation, radical c

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7

Cooper, William J., and Richard G. Zepp. "Hydrogen Peroxide Decay in Waters with Suspended Soils: Evidence for Biologically Mediated Processes." Canadian Journal of Fisheries and Aquatic Sciences 47, no. 5 (1990): 888–93. http://dx.doi.org/10.1139/f90-102.

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Hydrogen peroxide decay studies have been conducted in suspensions of several well-characterized soils and in natural water samples. Kinetic and product studies indicated that the decay was biologically-mediated, and could be described by pseudo first-order rate expressions. At an initial H2O2 concentration of 0.5 μM, the hydrogen peroxide half-life varied from 1 to 8 h. The decay was inhibited by thermal and chemical sterilization of the soils. Peroxidase activity was inferred in several natural water samples, where the suspended particles catalyzed the oxidation of p-anisidine by hydrogen pe

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8

zamansky, Vladimir M., Loc Ho, Peter M. Maly, and W. Randall Seeker. "Gas phase reactions of hydrogen peroxide and hydrogen peroxide/methanol mixtures with air pollutants." Symposium (International) on Combustion 26, no. 2 (1996): 2125–32. http://dx.doi.org/10.1016/s0082-0784(96)80037-3.

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9

Groele, Joseph, and John Foster. "Hydrogen Peroxide Interference in Chemical Oxygen Demand Assessments of Plasma Treated Waters." Plasma 2, no. 3 (2019): 294–302. http://dx.doi.org/10.3390/plasma2030021.

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Plasma-driven advanced oxidation represents a potential technology to safely re-use waters polluted with recalcitrant contaminants by mineralizing organics via reactions with hydroxyl radicals, thus relieving freshwater stress. The process results in some residual hydrogen peroxide, which can interfere with the standard method for assessing contaminant removal. In this work, methylene blue is used as a model contaminant to present a case in which this interference can impact the measured chemical oxygen demand of samples. Next, the magnitude of this interference is investigated by dosing de-io

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10

Apak, Resat. "Life detection experiments of the Viking Mission on Mars can be best interpreted with a Fenton oxidation reaction composed of H2O2 and Fe2+ and iron-catalysed decomposition of H2O2." International Journal of Astrobiology 7, no. 3-4 (2008): 187–92. http://dx.doi.org/10.1017/s1473550408004126.

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AbstractThe findings of the life detection experiments carried out during the Viking mission to Mars were reinterpreted with a chemical hypothesis. The labelled release (LR), pyrolytic release (PR) and gas exchange (GEx) experiments were interpreted with Fenton chemistry. Oxygen and carbon dioxide evolution from Martian soil upon wetting and nutrient addition could be attributed to competition reactions between the Fenton-type oxidation of organic nutrients with the aqueous (hydrogen peroxide+Fe(II)) combination and the iron-catalysed decomposition of hydrogen peroxide. A substantial evolution

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