Journal articles: 'Hydrogen peroxide decomposition'

1

TSUKADA, MASAO, AKIHIKO SEO, and TOMOAKI YOKOKURA. "The decomposition of hydrogen peroxide." Juntendo Medical Journal 50, no. 4 (2004): 515–22. http://dx.doi.org/10.14789/pjmj.50.515.

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2

Knotter, D. Martin, Stefan De Gendt, M. Baeyens, Paul W. Mertens, and Marc M. Heyns. "Hydrogen Peroxide Decomposition in Ammonia Solutions." Solid State Phenomena 65-66 (November 1998): 15–18. http://dx.doi.org/10.4028/www.scientific.net/ssp.65-66.15.

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3

Croiset, Eric, Steven F. Rice, and Russell G. Hanush. "Hydrogen peroxide decomposition in supercritical water." AIChE Journal 43, no. 9 (September 1997): 2343–52. http://dx.doi.org/10.1002/aic.690430919.

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4

Loeffler, M. J., and R. A. Baragiola. "Isothermal Decomposition of Hydrogen Peroxide Dihydrate." Journal of Physical Chemistry A 115, no. 21 (June 2, 2011): 5324–28. http://dx.doi.org/10.1021/jp200188b.

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Knotter, D. Martin, Stefan de Gendt, Martien Baeyens, Paul W. Mertens, and Marc M. Heyns. "Hydrogen Peroxide Decomposition in Ammonia Solutions." Journal of The Electrochemical Society 146, no. 9 (September 1, 1999): 3476–81. http://dx.doi.org/10.1149/1.1392499.

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Eberhardt, Manfred K., Angel A. Román-Franco, and Margarita R. Quiles. "Asbestos-induced decomposition of hydrogen peroxide." Environmental Research 37, no. 2 (August 1985): 287–92. http://dx.doi.org/10.1016/0013-9351(85)90108-2.

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Bourgeois, Marie-Josèphe, Marianne Vialemaringe, Monique Campagnole, and Evelyne Montaudon. "Réaction compétitive de la substitution homolytique intramoléculaire : décomposition de peroxydes allyliques dans le thioglycolate de méthyle." Canadian Journal of Chemistry 79, no. 3 (March 1, 2001): 257–62. http://dx.doi.org/10.1139/v01-024.

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The decomposition of allylic peroxides in methyl thioglycolate always leads to both epoxide and adduct peroxide. According to the nature of the allylic chain, either epoxide or peroxide is the predominant product, if not the only one. It is the first example where the hydrogen transfer is as fast as the intramolecular homolytic substitution. The influence of different factors upon the competition is studied.Key words: allylic peroxides, epoxides, intramolecular homolytic substitution, transfer.

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Watts, Richard J., Michael K. Foget, Sung-Ho Kong, and Amy L. Teel. "Hydrogen peroxide decomposition in model subsurface systems." Journal of Hazardous Materials 69, no. 2 (October 1999): 229–43. http://dx.doi.org/10.1016/s0304-3894(99)00114-4.

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Petigara, Bhakti R., Neil V. Blough, and Alice C. Mignerey. "Mechanisms of Hydrogen Peroxide Decomposition in Soils." Environmental Science & Technology 36, no. 4 (February 2002): 639–45. http://dx.doi.org/10.1021/es001726y.

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Hasegawa, Shinji, Kei Shimotani, Kentaro Kishi, and Hiroyuki Watanabe. "Electricity Generation from Decomposition of Hydrogen Peroxide." Electrochemical and Solid-State Letters 8, no. 2 (2005): A119. http://dx.doi.org/10.1149/1.1849112.

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11

Manthey, Michael K., Stephen G. Pyne, and Roger J. W. Truscott. "Decomposition of cinnabarinic acid by hydrogen peroxide." Journal of Heterocyclic Chemistry 29, no. 1 (January 1992): 263–64. http://dx.doi.org/10.1002/jhet.5570290150.

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12

Yoshimoto, Makoto, Yuya Miyazaki, Ayumi Umemoto, Peter Walde, Ryoichi Kuboi, and Katsumi Nakao. "Phosphatidylcholine Vesicle-Mediated Decomposition of Hydrogen Peroxide." Langmuir 23, no. 18 (August 2007): 9416–22. http://dx.doi.org/10.1021/la701277f.

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13

Sun, Bing, Hongwei Zhu, Yan Jin, Kun Qiao, Wei Xu, and Jie Jiang. "Rapid Hydrogen Peroxide Decomposition Using a Microreactor." Chemical Engineering & Technology 42, no. 1 (November 14, 2018): 252–56. http://dx.doi.org/10.1002/ceat.201800319.

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Arvin, Erik, and Lars-Flemming Pedersen. "Hydrogen peroxide decomposition kinetics in aquaculture water." Aquacultural Engineering 64 (January 2015): 1–7. http://dx.doi.org/10.1016/j.aquaeng.2014.12.004.

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15

El-Sheikh, M. Y., A. M. Habib, A. K. Abou-Seif, and A. B. Zaki. "Kinetics of heterogeneous decomposition of hydrogen peroxide." Journal of Inclusion Phenomena 4, no. 4 (December 1986): 359–67. http://dx.doi.org/10.1007/bf00656163.

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Tsuneda, Takao, and Tetsuya Taketsugu. "Theoretical investigations on hydrogen peroxide decomposition in aquo." Physical Chemistry Chemical Physics 20, no. 38 (2018): 24992–99. http://dx.doi.org/10.1039/c8cp04299c.

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Hydrogen peroxide (H₂O₂) decomposition mechanisms in the absence and presence of iron ions in aqueous solution, which contain no OH radical formation, are theoretically determined. H₂O₂ decomposition in the presence of iron ions is driven by electron transfer to the iron ion and proceeds by hydrogen transfers in the hydrogen bond network around H₂O₂.

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17

Kenna, N. Mac, and A. Morrin. "Inducing macroporosity in hydrogels using hydrogen peroxide as a blowing agent." Materials Chemistry Frontiers 1, no. 2 (2017): 394–401. http://dx.doi.org/10.1039/c6qm00052e.

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A new gas blowing method to induce a macroporous structure in pH-responsive hydrogel materials with basic functional groups is reported by a new technique that generates oxygen bubbles via hydrogen peroxide decomposition to template the polymer.

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18

Zun, Maria, Dorota Dwornicka, Katarzyna Wojciechowska, Katarzyna Swiader, Regina Kasperek, Marzena Rzadkowska, and Ewa Poleszak. "Kinetics of the decomposition and the estimation of the stability of 10% aqueous and non-aqueous hydrogen peroxide solutions." Current Issues in Pharmacy and Medical Sciences 27, no. 4 (December 1, 2014): 213–16. http://dx.doi.org/10.1515/cipms-2015-0017.

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Abstract In this study, the stability of 10% hydrogen peroxide aqueous and non-aqueous solutions with the addition of 6% (w/w) of urea was evaluated. The solutions were stored at 20°C, 30°C and 40°C, and the decomposition of hydrogen peroxide proceeded according to first-order kinetics. With the addition of the urea in the solutions, the decomposition rate constant increased and the activation energy decreased. The temperature of storage also affected the decomposition of substance, however, 10% hydrogen peroxide solutions prepared in PEG-300, and stabilized with the addition of 6% (w/w) of urea had the best constancy.

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19

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 decomposition. Comparison and description of the most commonly used catalysts were presented in this review.

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20

Gonopol'sky, A. M., S. G. Shashkovskiy, Y. A. Goldstein, S. G. Kireev, A. D. Volosatova, and A. I. Kulebyakina. "Pulse Рhotochemical Decomposition of Phenol in Wastewater." Ecology and Industry of Russia 24, no. 2 (February 26, 2020): 22–27. http://dx.doi.org/10.18412/1816-0395-2020-2-22-27.

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Photochemical decomposition of phenol with a concentration of 5 to 24 mg/L using hydrogen peroxide and ultraviolet irradiation (UV/H2O2) was studied. Xenon flash lamp was chosen as a radiation source. It emits high-intensity continuous-spectrum radiation in a wide wavelength range from 200 to 1000 nm. The effect of the initial concentration of hydrogen peroxide and the source average radiation power on the phenol destruction rate were studied. An extremum in the dependence of the phenol decomposition rate constant on the initial concentration of hydrogen peroxide was found. Kinetic model of the process based on the obtained data was developed. It was tested by predicting phenol destruction rate with the different process parameters and gave good accuracy.

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21

Luňák, Stanislav, Petr Sedlák, and Josef Vepřek-Šiška. "Photolysis of hydrogen peroxide, photocatalytic effects of Cu(II) and reaction kinetics." Collection of Czechoslovak Chemical Communications 51, no. 5 (1986): 973–81. http://dx.doi.org/10.1135/cccc19860973.

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The quantum yield of hydrogen peroxide photolysis has been measured as a function of the concentration of photocatalytically active Cu2+ ions, intensity of photolytic radiation, temperature, and hydrogen peroxide concentration. The results obtained are consistent with the concept that high quantum yields of hydrogen peroxide photolysis (Φ >> 1) are due to thermal decomposition of hydrogen peroxide catalyzed by photochemically generated copper ions in oxidation states which are catalytically active.

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22

Khan, Zainab, Nicholas F. Dummer, and Jennifer K. Edwards. "Silver–palladium catalysts for the direct synthesis of hydrogen peroxide." Philosophical Transactions of the Royal Society A: Mathematical, Physical and Engineering Sciences 376, no. 2110 (November 27, 2017): 20170058. http://dx.doi.org/10.1098/rsta.2017.0058.

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A series of bimetallic silver–palladium catalysts supported on titania were prepared by wet impregnation and assessed for the direct synthesis of hydrogen peroxide, and its subsequent side reactions. The addition of silver to a palladium catalyst was found to significantly decrease hydrogen peroxide productivity and hydrogenation, but crucially increase the rate of decomposition. The decomposition product, which is predominantly hydroxyl radicals, can be used to decrease bacterial colonies. The interaction between silver and palladium was characterized using scanning electron microscopy, X-ray diffraction, X-ray photoelectron spectroscopy (XPS) and temperature programmed reduction (TPR). The results of the TPR and XPS indicated the formation of a silver–palladium alloy. The optimal 1% Ag–4% Pd/TiO 2 bimetallic catalyst was able to produce approximately 200 ppm of H 2 O 2 in 30 min. The findings demonstrate that AgPd/TiO 2 catalysts are active for the synthesis of hydrogen peroxide and its subsequent decomposition to reactive oxygen species. The catalysts are promising for use in wastewater treatment as they combine the disinfectant properties of silver, hydrogen peroxide production and subsequent decomposition. This article is part of a discussion meeting issue ‘Providing sustainable catalytic solutions for a rapidly changing world’.

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23

Chumakov, Anton A., Valentina N. Batalova, Yuriy G. Slizhov, and Tamara S. Minakova. "VERIFICATION OF NON-CATALYTIC HYDROGEN PEROXIDE DISPROPORTIONATION MECHANISM BY THERMODYNAMIC ANALYSIS OF ONE-ELECTRON REDOX REACTIONS." IZVESTIYA VYSSHIKH UCHEBNYKH ZAVEDENIY KHIMIYA KHIMICHESKAYA TEKHNOLOGIYA 60, no. 6 (July 19, 2017): 40. http://dx.doi.org/10.6060/tcct.2017606.5529.

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There is two-electron transfer during the process of hydrogen peroxide decomposition into water and oxygen. The detailed mechanism of non-catalytic hydrogen peroxide disproportionation is not verified until now. We assumed that any poly-electron redox process is a complex and consists of one-electron redox reactions. We have formulated equations of possible one-electron transfers during hydrogen peroxide disproportionation. Based on known laws and equations of thermochemistry we calculated standard thermodynamic functions for a total reaction and each one-elect-ron redox reaction using reference values of standard thermodynamic functions of reagents and products of reactions. Results show that the total reaction leads to significant decrease in Gibbs free energy -246.0 kJ/mol in gas phase but there is increase +39.9 kJ/mol in Gibbs free energy during the first proposed step. It is substantiation for known dependence of hydrogen peroxide dismutation kinetics at thermal, photochemical or catalytic activation. The first proposed step of non-catalytic process is one-electron plus one-proton transfer in thermally or photochemically activated dimeric hydrogen peroxide associate (H2O2)2 with simultaneous generation of hydroperoxyl HO2• and hydroxyl HO• free radicals and water molecule. There is thermodynamic argumentation for radical chain mechanism of hydrogen peroxide disproportionation after the activation. We made the graphic illustration of thermodynamically supported scheme of non-catalytic hydrogen peroxide decomposition. There is a cyclic alternation of two radical-molecular interactions during the hydrogen peroxide chain decomposition. The hydroxyl radical generates the hydroperoxyl radi-cal from a hydrogen peroxide molecule and then the hydroperoxyl radical interacts with a next hydrogen peroxide molecule followed by the hydroxyl radical generation. Interactions between the homonymic or heteronymic free radicals are the reactions of chain breaking.Forcitation:Chumakov A.A., Batalova V.N., Slizhov Yu.G., Minakova T.S. Verification of non-catalytic hydrogen peroxide disproportionation mechanism by thermodynamic analysis of one-electron redox reactions. Izv. Vyssh. Uchebn. Zaved. Khim. Khim. Tekhnol. 2017. V. 60. N 6. P. 40-44.

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Siddiqui, S., M. Keswani, B. Brooks, A. Fuerst, and S. Raghavan. "A study of hydrogen peroxide decomposition in ammonia-peroxide mixtures (APM)." Microelectronic Engineering 102 (February 2013): 68–73. http://dx.doi.org/10.1016/j.mee.2012.04.003.

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25

Alvarez, J. D., W. Gernjak, S. Malato, M. Berenguel, M. Fuerhacker, and L. J. Yebra. "Dynamic Models for Hydrogen Peroxide Control in Solar Photo-Fenton Systems." Journal of Solar Energy Engineering 129, no. 1 (December 10, 2005): 37–44. http://dx.doi.org/10.1115/1.2391014.

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Simulations and real decomposition experiments with hydrogen peroxide induced by dissolved iron and solar illumination were performed in a solar pilot plant with compound parabolic collectors designed for photo-Fenton wastewater treatment. The structure of a gray-box linear model aimed at reproducing system dynamics with parameters dependent on operating conditions when operating around prescribed set-points is proposed. This simple model relates the changes in hydrogen peroxide concentration due to changes in hydrogen peroxide injection, dissolved iron, and solar illumination. Based on this model, control of the hydrogen peroxide concentration at set points between 200-900mg∕L±10mg∕L under dynamic conditions (simultaneous decomposition and addition of hydrogen peroxide by a dosage pump), was achieved. Different basic approaches for controller actuation upon the frequency of the dosage pump were tested, ranging from a simple PI controller to a PI controller plus antiwindup action and feedforward control. From these basic approaches, conclusions can be drawn about the process’s behavior under closed-loop control.

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26

Araminaitė, Rūta, Rasa Garjonytė, and Albertas Malinauskas. "Kinetic study of the decomposition of Prussian Blue electrocatalytic layer during cathodic reduction of hydrogen peroxide." Open Chemistry 6, no. 2 (June 1, 2008): 175–79. http://dx.doi.org/10.2478/s11532-008-0021-8.

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AbstractKinetic study on the decomposition of Prussian Blue electrocatalytic layer during electrochemical reduction of hydrogen peroxide has been studied in relation to biosensor application of this electrocatalyst. The decomposition has been shown to proceed as a nearly exponential decay process and the corresponding first-order rate coefficients were determined. It has been shown that the decomposition proceeds about 10 times faster in pH 7.3 buffer solution as compared to pH 5.5 buffer. A linear dependence of the decomposition rate on the concentration of hydrogen peroxide has been found.

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27

Glaze, William H., Fernando Beltran, Tuula Tuhkanen, and Joon-Wun Kang. "Chemical Models of Advanced Oxidation Processes." Water Quality Research Journal 27, no. 1 (February 1, 1992): 23–42. http://dx.doi.org/10.2166/wqrj.1992.002.

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Abstract Advanced oxidation processes (AOPs) have been defined as near-ambient temperature processes that involve the generation of highly reactive radical intermediates, especially the hydroxyl radical. These processes show promise for the destruction of hazardous organic substances in municipal and industrial wastes, in drinking water and in ultrapure water. Three types of AOPs are considered in this paper: catalyzed decomposition of ozone; ozone with hydrogen peroxide (Peroxone); and photolysis of hydrogen peroxide with ultraviolet radiation. Kinetic models for these processes are being developed based on known chemical and photochemical principles. The models take into account measured effects of radical scavengers such as bicarbonate; dose ratios of the oxidants or UV intensity; pH; and the presence of generic radical scavengers. The models are used to discuss two cases: oxidation of parts-per-million levels of nitrobenzene with ozone, Peroxone and peroxide/UV and oxidation of naphthalene and pentachlorophenol with peroxide/UV.

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28

Guo, Tian Xiang, Yi Zhao, Shuang Chen Ma, and Song Tao Liu. "Decomposition Characteristics of Hydrogen Peroxide in Sodium Hydroxide Solution." Advanced Materials Research 610-613 (December 2012): 359–62. http://dx.doi.org/10.4028/www.scientific.net/amr.610-613.359.

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In order to spread more applications, decomposition characteristics of hydrogen peroxide (H2O2) in sodium hydroxide (NaOH) solution were investigated in this paper. Research results indicate that the attack of charged particles such as OH- and HO2- leads to H2O2 decomposition. HO2¬- is vital reactive intermediate, which was mainly from neutral reaction of H2O2 with NaOH. The decomposition is considered as pseudo-two-order kinetics, and the reaction rate constant depended on decomposition temperature and solution pH. The apparent average activation energy is 51.92 kJ•mol-1 when the initial NaOH concentration is 1mol•L-1 and solution pH is 10.5.

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29

Vetter, Tiffany A., and D. Philip Colombo. "Kinetics of Platinum-Catalyzed Decomposition of Hydrogen Peroxide." Journal of Chemical Education 80, no. 7 (July 2003): 788. http://dx.doi.org/10.1021/ed080p788.

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30

Venkatachalapathy, R. "Catalytic decomposition of hydrogen peroxide in alkaline solutions." Electrochemistry Communications 1, no. 12 (December 1, 1999): 614–17. http://dx.doi.org/10.1016/s1388-2481(99)00126-5.

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31

Ball, Matthew C., and Steven Massey. "The thermal decomposition of solid urea hydrogen peroxide." Thermochimica Acta 261 (September 1995): 95–106. http://dx.doi.org/10.1016/0040-6031(95)02399-m.

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32

Wong, George T. F., William M. Dunstan, and Dong-Beom Kim. "The decomposition of hydrogen peroxide by marine phytoplankton." Oceanologica Acta 26, no. 2 (April 2003): 191–98. http://dx.doi.org/10.1016/s0399-1784(02)00006-3.

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33

Conklin, Alfred R., and Angela Kessinger. "Demonstration of the catalytic decomposition of hydrogen peroxide." Journal of Chemical Education 73, no. 9 (September 1996): 838. http://dx.doi.org/10.1021/ed073p838.

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34

Liao, Chih-Hsiang, and Mirat D. Gurol. "Chemical Oxidation by Photolytic Decomposition of Hydrogen Peroxide." Environmental Science & Technology 29, no. 12 (December 1995): 3007–14. http://dx.doi.org/10.1021/es00012a018.

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35

Ariafard, Alireza, Hamid Reza Aghabozorg, and Fathollah Salehirad. "Hydrogen peroxide decomposition over La0.9Sr0.1Ni1−Cr O3 perovskites." Catalysis Communications 4, no. 11 (November 2003): 561–66. http://dx.doi.org/10.1016/j.catcom.2003.08.010.

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36

Guseinov, Sh L., S. G. Fedorov, V. A. Kosykh, and P. A. Storozhenko. "Hydrogen Peroxide Decomposition Catalysts Used in Rocket Engines." Russian Journal of Applied Chemistry 93, no. 4 (April 2020): 467–87. http://dx.doi.org/10.1134/s1070427220040011.

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37

Ghiretti, F. "The decomposition of hydrogen peroxide by Octopus hemocyanin." Bulletin des Sociétés Chimiques Belges 65, no. 1-2 (September 1, 2010): 103–6. http://dx.doi.org/10.1002/bscb.19560650110.

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38

El-Sheikh, Mohamed Y. "Mixed resin base-catalyzed decomposition of hydrogen peroxide." Colloids and Surfaces 54 (January 1991): 83–88. http://dx.doi.org/10.1016/0166-6622(91)80051-o.

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39

Miletiev, Rosen, Ivaylo Simeonov, Vladislava Stefanova, and Mitko Georgiev. "Thermodynamic analysis of the hydrogen peroxide decomposition parameters." Journal of Thermal Analysis and Calorimetry 113, no. 2 (November 21, 2012): 985–89. http://dx.doi.org/10.1007/s10973-012-2769-5.

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40

Sorge, Annamaria Russo, Maria Turco, Giuseppe Pilone, and Giovanni Bagnasco. "Decomposition of Hydrogen Peroxide on MnO2/TiO2 Catalysts." Journal of Propulsion and Power 20, no. 6 (November 2004): 1069–75. http://dx.doi.org/10.2514/1.2490.

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41

Abbot, John, and Douglas G. Brown. "Stabilization of iron-catalysed hydrogen peroxide decomposition by magnesium." Canadian Journal of Chemistry 68, no. 9 (September 1, 1990): 1537–43. http://dx.doi.org/10.1139/v90-237.

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Catalytic decomposition of alkaline hydrogen peroxide by iron can be retarded by introduction of magnesium ions. This effect has been studied to evaluate the possibility of stabilization via formation of an iron–magnesium complex species. Under alkaline conditions, magnesium reacts with initial hydrolysis products of Fe3+ to produce a colourless complex species, in which the metal centres are probably linked through oxy or hydroxy bridges. This species is produced when the Mg:Fe molar ratio exceeds 6:1, and this ratio is also significant when magnesium is introduced during peroxide decomposition experiments. The evidence suggests that complex formation is an important factor in producing stabilization, and cannot be disregarded in favour of an alternative explanation where superoxide radicals combine with Mg2+ to produce magnesium dioxide. Keywords: hydrogen peroxide, kinetics, iron, magnesium, stabilization.

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Sanjay Vasanth., KB, G. Gokul Raj., and M. Venkatesan. "Numerical model for concentration measurement during decomposition of H2O2 over silver catalyst." MATEC Web of Conferences 172 (2018): 01008. http://dx.doi.org/10.1051/matecconf/201817201008.

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Minimal thrust of the order of few Newton is produced using micro thrusters, which are used for controlling the orientation and trajectory of the satellite or spacecraft. Controlled thrust production of the order of milli Newton is still a challenging task. Green propellants like Hydrogen peroxide are utilized in such applications. The products of this green fuel after decomposition are water in the form of steam and oxygen. The present work involves the simulation of hydrogen peroxide decomposition on silver catalyst which can be used in space propulsion. The simulations are done for flow of 30% hydrogen peroxide concentration when flowing inside a mini channel of size 3.4mm. Helical shaped silver catalyst is positioned inside the tube to enhance the decomposition. The model involves the concentration measurement of the reactants and products and after passing over the catalyst surface. The results will help in choosing the geometry and position of the catalyst to have effective decomposition of the monopropellant.

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43

Kim, Taegyu. "Hydrogen production from solid sodium borohydride with hydrogen peroxide decomposition reaction." International Journal of Hydrogen Energy 35, no. 23 (December 2010): 12870–77. http://dx.doi.org/10.1016/j.ijhydene.2010.08.102.

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44

Klaper, M., P. Wessig, and T. Linker. "Base catalysed decomposition of anthracene endoperoxide." Chemical Communications 52, no. 6 (2016): 1210–13. http://dx.doi.org/10.1039/c5cc08606j.

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45

Kutova, O. Yu, M. G. Dusheyko, B. O. Loboda, and T. Yu Obukhova. "Changing the conductivity of porous silicon with silver nanoparticles/silicon structures when detecting hydrogen peroxide." Технология и конструирование в электронной аппаратуре, no. 4 (2018): 28–32. http://dx.doi.org/10.15222/tkea2018.4.28.

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The authors investigate the influence of hydrogen peroxide concentration on the conductivity of the porous silicon with silver nanoparticles / crystalline silicon system. A simple resistive sensor with Ag nanoparticles was used as a catalyst in order to study processes occuring in porous silicon during hydrogen peroxide detection. Porous silicon was formed using a two-stage metal-assisted chemical etching with Ag nanoparticles. It was shown that two simultaneous processes are involved here: carrier extraction to porous silicon caused by interaction with hydrogen peroxide molecules and heating caused by hydrogen peroxide decomposition in presence of Ag nanoparticles. Dimensions of the investigated sensor structure were comparable with a drop of the solution, thus at 30‰ concentration heating could reach 10°C. As porous silicon/crystalline silicon system has a negative temperature coefficient, two above mentioned processes counteract which leads to a maximum, or saturation, on the graph of the dependence of resistivity on hydrogen peroxide concentration at 10—11‰. Sensitivity declines from 0.001—0.02 to 0.0001—0.0003%/‰. To prove these thesis resistivity-concentration dependences were adjusted taking into account calculated heating caused by hydrogen peroxide decomposition. It was shown that in this case the slope of the dependence curve remains stable up to 30 ‰ and sensitivity remains about 0.001—0.02%/‰.

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46

Das, N., SK Bose, and D. Biswas. "Effect of magnesium-salts on hydrogen peroxide bleaching of non-wood pulps." Bangladesh Journal of Scientific and Industrial Research 51, no. 4 (December 10, 2016): 291–96. http://dx.doi.org/10.3329/bjsir.v51i4.30449.

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Transition metal ions present in pulp, cause wasteful decomposition of hydrogen peroxide, a pulp brightener, and thus significantly affect the delignification selectivity of hydrogen peroxide bleaching. The metal ions also affect the brightness and optical properties of pulp. The free radicals generated during the decomposition degrade carbohydrates resulting in lower viscosity and yield. It is reported in the literature that magnesium sulfate successfully adsorbs transition metal ions and thus decrease their activity. This study dealt with the effect of Mg salts in hydrogen peroxide bleaching of jute caddies pulp. It was observed that prior bleaching treatments like chelation and acid washing of pulp were efficient in removing transition metal ions as indicated by lower consumption of hydrogen peroxide. However EDTA chelation seemed better compared to acid washing. The inclusion of Mg salts improved pulp brightness. The pulp viscosity was the highest with 0.3% Mg addition for both treated kraft and soda-AQ pulps. Considering both pulp viscosity and pulp brightness, it appeared that a 0.3% Mg dose on EDTA chelated pulp, was enough in hydrogen peroxide bleaching of pulps obtained from jute caddies. Bangladesh J. Sci. Ind. Res. 51(4), 291-296, 2016

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47

Špalek, Otomar. "Calculation of potential and concentration gradients in trickle-bed electrodes producing hydrogen peroxide." Collection of Czechoslovak Chemical Communications 51, no. 9 (1986): 1883–98. http://dx.doi.org/10.1135/cccc19861883.

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A mathematical model for describing the trickle-bed electrode has been developed and used to calculate the potential distribution along the current flow and the hydrogen peroxide concentration profile along the electrolyte flow (normal to the direction of current). Polarization curves and dependences of the current yield of hydrogen peroxide and the peroxide losses due to the processes occurring (reduction, decomposition, and transport into the anode chamber) on the current density have also been calculated. A comparison is made between calculated and measured dependences of the current yield of hydrogen peroxide on the current density.

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Tastanоva, L. K., and A. M. Muratkaliy. "Studу оf the activity оf irоn-cоntaining catalуsts fоr the оxidatiоn оf cуclоalkanes during the decоmpоsitiоn оf hуdrоgen perоxide." BULLETIN of the L.N. Gumilyov Eurasian National University. Chemistry. Geography. Ecology Series 130, no. 1 (2020): 62–67. http://dx.doi.org/10.32523/2616-6771-2020-130-1-62-67.

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Currently, the oxidation process, including the oxidation of cyclohexane with hydrogen peroxide, is widely used in the chemical industry. Today, polymer-metal catalysts are of great importance for the oxidation process. In this paper, ironcontaining catalysts were prepared and their activity was studied during the decomposition of hydrogen peroxide. Synthesis of catalysts were carried out by the impregnation method. The microstructure of iron-containing catalysts were determined using the scanning electron microscope PHENOM TM G2. The porous dimensions and characteristics were determined. Determination of the oxygen content formed during the decomposition of hydrogen peroxide was carried out using the gasometric method. As a result, it was found that the Fe-PVPD/ Al2O3 catalyst has a high activity in comparison with other iron-containing catalysts.

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Jacobi, Hans-Werner, Bright Kwakye-Awuah, and Otto Schrems. "Photochemical decomposition of hydrogen peroxide (H2O2) and formaldehyde (HCHO) in artificial snow." Annals of Glaciology 39 (2004): 29–33. http://dx.doi.org/10.3189/172756404781814357.

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AbstractLaboratory-made snow doped with either hydrogen peroxide (H2O2) or formaldehyde (HCHO) was exposed to radiation in the ultraviolet and visible range, resulting in a decomposition of both compounds. These experiments demonstrate that, besides the photolysis of nitrate, further photochemical reactions of atmospheric relevant compounds can take place in snow. Under similar conditions the decomposition of H2O2 is more efficient than that of HCHO. Since the decompositions in the experiments follow first-order reaction kinetics, we suggest that the same products as in photolysis reactions in the liquid phase are produced. If similar reactions also take place in natural snow covers, these reactions would have several important consequences. The reactions could represent pathways for the generation of highly reactive radicals in the condensed phase, enhancing the photochemical activity of surface snow and modifying the oxidation capacity of the atmospheric boundary layer. The photolysis could also constitute an additional sink for H2O2 and HCHO in surface snow, which should be taken into account for the reconstruction of atmospheric concentrations of both compounds from concentration profiles in surface snow and ice cores.

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Zuo, Guifu, Bingdong Li, Zhaoliang Guo, Liang Wang, Fan Yang, Weishu Hou, Songtao Zhang, et al. "Efficient Photocatalytic Hydrogen Peroxide Production over TiO2 Passivated by SnO2." Catalysts 9, no. 7 (July 21, 2019): 623. http://dx.doi.org/10.3390/catal9070623.

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Photocatalysis provides an attractive strategy for synthesizing H2O2 at ambient condition. However, the photocatalytic synthesis of H2O2 is still limited due to the inefficiency of photocatalysts and decomposition of H2O2 during formation. Here, we report SnO2-TiO2 heterojunction photocatalysts for synthesizing H2O2 directly in aqueous solution. The SnO2 passivation suppresses the complexation and decomposition of H2O2 on TiO2. In addition, loading of Au cocatalyst on SnO2-TiO2 heterojunction further improves the production of H2O2. The in situ electron spin resonance study revealed that the formation of H2O2 is a stepwise single electron oxygen reduction reaction (ORR) for Au and SnO2 modified TiO2 photocatalysts. We demonstrate that it is feasible to enhance H2O2 formation and suppress H2O2 decomposition by surface passivation of the H2O2-decomposition-sensitive photocatalysts.

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Journal articles on the topic 'Hydrogen peroxide decomposition'

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