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Journal articles on the topic 'Photochemical water oxidation'

Author: Grafiati
Published: 4 June 2021
Last updated: 12 February 2022

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1

Hetterscheid, Dennis G. H., and Wilson A. Smith. "Electrochemical and photochemical water oxidation." Catalysis Today 290 (July 2017): 1. http://dx.doi.org/10.1016/j.cattod.2017.05.002.

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2

Yue, P. L., and O. Legrini. "Photochemical Degradation of Organics in Water." Water Quality Research Journal 27, no. 1 (February 1, 1992): 123–38. http://dx.doi.org/10.2166/wqrj.1992.007.

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Abstract Trichloroethylene, phenol, 4-cholorophenol, catechol and a pesticide were degraded by two advanced oxidation processes: photolytic oxidation with hydrogen peroxide, andphotolytic oxidation with ozone. The reactions were studied in a batch photoreactor with a low pressure mercury lamp as the radiation source. The variation of the concentration of total organic carbon with time was measured. For the organics studied, the reaction kinetics for the reduction of total organic carbon (TOC) were found to follow a power law. The exponent of the power law varies with the initial TOC concentration. Results show that TOC can be very effectively reduced provided the concentration of hydrogen peroxide used exceeds a certain threshold value. The UV/Ozone process yielded a more rapid rate of degradation and a greater degree of mineralisation.
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3

Sartorel, Andrea, Marcella Bonchio, Sebastiano Campagna, and Franco Scandola. "Tetrametallic molecular catalysts for photochemical water oxidation." Chem. Soc. Rev. 42, no. 6 (2013): 2262–80. http://dx.doi.org/10.1039/c2cs35287g.

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4

Kalisman, Philip, Yaron Kauffmann, and Lilac Amirav. "Photochemical oxidation on nanorod photocatalysts." Journal of Materials Chemistry A 3, no. 7 (2015): 3261–65. http://dx.doi.org/10.1039/c4ta06164k.

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5

Huang, Xiang, Juan-Pablo Aranguren, Johannes Ehrmaier, Jennifer A. Noble, Weiwei Xie, Andrzej L. Sobolewski, Claude Dedonder-Lardeux, Christophe Jouvet, and Wolfgang Domcke. "Photoinduced water oxidation in pyrimidine–water clusters: a combined experimental and theoretical study." Physical Chemistry Chemical Physics 22, no. 22 (2020): 12502–14. http://dx.doi.org/10.1039/d0cp01562h.

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6

Ressnig, Debora, Menny Shalom, Jörg Patscheider, René Moré, Fabio Evangelisti, Markus Antonietti, and Greta R. Patzke. "Photochemical and electrocatalytic water oxidation activity of cobalt carbodiimide." Journal of Materials Chemistry A 3, no. 9 (2015): 5072–82. http://dx.doi.org/10.1039/c5ta00369e.

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7

Tarasov, V. V., G. S. Barancova, N. K. Zaitsev, and Zhang Dongxiang. "Photochemical Kinetics of Organic Dye Oxidation in Water." Process Safety and Environmental Protection 81, no. 4 (July 2003): 243–49. http://dx.doi.org/10.1205/095758203322299761.

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8

Bofill, Roger, Jordi García-Antón, Lluís Escriche, and Xavier Sala. "Chemical, electrochemical and photochemical molecular water oxidation catalysts." Journal of Photochemistry and Photobiology B: Biology 152 (November 2015): 71–81. http://dx.doi.org/10.1016/j.jphotobiol.2014.10.022.

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9

Deng, Xiaohui, Hans-Josef Bongard, Candace K. Chan, and Harun Tüysüz. "Dual-Templated Cobalt Oxide for Photochemical Water Oxidation." ChemSusChem 9, no. 4 (September 25, 2015): 409–15. http://dx.doi.org/10.1002/cssc.201500872.

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10

Liu, Hongfei, René Moré, Henrik Grundmann, Chunhua Cui, Rolf Erni, and Greta R. Patzke. "Promoting Photochemical Water Oxidation with Metallic Band Structures." Journal of the American Chemical Society 138, no. 5 (January 28, 2016): 1527–35. http://dx.doi.org/10.1021/jacs.5b10215.

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11

Werner, Håkan A. F., and Rupert Bauer. "Some possibilities and problems regarding photochemical water oxidation." Journal of Molecular Catalysis 88, no. 2 (March 1994): 185–91. http://dx.doi.org/10.1016/0304-5102(93)e0265-i.

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12

Pfanner, Klaus, Niklaus Gfeller, and Gion Calzaferri. "Photochemical oxidation of water with thin AgCl layers." Journal of Photochemistry and Photobiology A: Chemistry 95, no. 2 (April 1996): 175–80. http://dx.doi.org/10.1016/1010-6030(95)04244-x.

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13

Das, Santu, and Soumyajit Roy. "Photochemical Water Oxidation Using {PMo12O40@Mo72Fe30}n Based Soft Oxometalate." Journal of Molecular and Engineering Materials 05, no. 01 (March 2017): 1750001. http://dx.doi.org/10.1142/s2251237317500010.

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Finding an alternative energy resource which can produce clean energy at a low cost is one of the major concerns of our times. The conversion of light energy into chemical energy is one key step forward in the direction. With that end in view photochemical water oxidation to produce oxygen plays a crucial role. In the present paper we have synthesized a soft oxometalate {PMo[Formula: see text]O[Formula: see text]@Mo[Formula: see text]Fe[Formula: see text]}n(1) from its well-known precursor polyoxometalate constituent [Muller et al., Chem. Commun. 1, 657 (2001)]. It is known that in the matter of catalysis, high surface area, possibility of heterogenization, recoverability makes soft oxometalates (SOMs) attractive as catalytic materials. Here we exploit such advantages of SOMs. The SOM based material acts as an active catalyst for photochemical water oxidation reaction with a maximum turnover number of 20256 and turnover frequency of 24.11[Formula: see text]min[Formula: see text]. The catalyst material is stable under photochemical reaction conditions and therefore can be reused for multiple photo catalytic water oxidation reaction cycles.
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14

Wentworth, Paul, and Daniel P. Witter. "Antibody-catalyzed water-oxidation pathway." Pure and Applied Chemistry 80, no. 8 (January 1, 2008): 1849–58. http://dx.doi.org/10.1351/pac200880081849.

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The intrinsic ability of all antibodies to generate hydrogen peroxide (H2O2) from singlet dioxygen (1O2*) via the antibody-catalyzed water-oxidation pathway (ACWOP) has triggered a rethink of the potential role of antibodies both in immune defense, inflammation, and disease. It has been shown that photochemical activation of this pathway is highly bactericidal. More recently, cholesterol oxidation by-products that may arise from the ACWOP have been discovered in vivo and are receiving a great deal of attention as possible key players in atherosclerosis and diseases of protein misfolding, such as Alzheimer's disease and Parkinson's disease.
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15

Gui-peng, Yang. "Photochemical oxidation of benzothiophene in seawater." Chinese Journal of Oceanology and Limnology 18, no. 1 (March 2000): 85–91. http://dx.doi.org/10.1007/bf02842547.

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16

Rao, C. N. R., S. R. Lingampalli, Sunita Dey, and Anand Roy. "Solar photochemical and thermochemical splitting of water." Philosophical Transactions of the Royal Society A: Mathematical, Physical and Engineering Sciences 374, no. 2061 (February 28, 2016): 20150088. http://dx.doi.org/10.1098/rsta.2015.0088.

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Artificial photosynthesis to carry out both the oxidation and the reduction of water has emerged to be an exciting area of research. It has been possible to photochemically generate oxygen by using a scheme similar to the Z -scheme, by using suitable catalysts in place of water-oxidation catalyst in the Z -scheme in natural photosynthesis. The best oxidation catalysts are found to be Co and Mn oxides with the e 1 g configuration. The more important aspects investigated pertain to the visible-light-induced generation of hydrogen by using semiconductor heterostructures of the type ZnO/Pt/Cd 1− x Zn x S and dye-sensitized semiconductors. In the case of heterostructures, good yields of H 2 have been obtained. Modifications of the heterostructures, wherein Pt is replaced by NiO, and the oxide is substituted with different anions are discussed. MoS 2 and MoSe 2 in the 1T form yield high quantities of H 2 when sensitized by Eosin Y. Two-step thermochemical splitting of H 2 O using metal oxide redox pairs provides a strategy to produce H 2 and CO. Performance of the Ln 0.5 A 0.5 MnO 3 (Ln = rare earth ion, A = Ca, Sr) family of perovskites is found to be promising in this context. The best results to date are found with Y 0.5 Sr 0.5 MnO 3 .
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17

Goussias, Charilaos, Alain Boussac, and A. William Rutherford. "Photosystem II and photosynthetic oxidation of water: an overview." Philosophical Transactions of the Royal Society of London. Series B: Biological Sciences 357, no. 1426 (October 29, 2002): 1369–81. http://dx.doi.org/10.1098/rstb.2002.1134.

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Conceptually, photosystem II, the oxygen–evolving enzyme, can be divided into two parts: the photochemical part and the catalytic part. The photochemical part contains the ultra–fast and ultra–efficient light–induced charge separation and stabilization steps that occur when light is absorbed by chlorophyll. The catalytic part, where water is oxidized, involves a cluster of Mn ions close to a redox–active tyrosine residue. Our current understanding of the catalytic mechanism is mainly based on spectroscopic studies. Here, we present an overview of the current state of knowledge of photosystem II, attempting to delineate the open questions and the directions of current research.
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18

Terao, Ryota, Takashi Nakazono, Alexander Rene Parent, and Ken Sakai. "Photochemical Water Oxidation Catalyzed by a Water-Soluble Copper Phthalocyanine Complex." ChemPlusChem 81, no. 10 (October 2016): 1064–67. http://dx.doi.org/10.1002/cplu.201600263.

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19

Mukhopadhyay, Sujay, Roop Shikha Singh, Arnab Biswas, and Daya Shankar Pandey. "Photochemical water oxidation by cyclometalated iridium(iii) complexes: a mechanistic insight." Chemical Communications 52, no. 19 (2016): 3840–43. http://dx.doi.org/10.1039/c5cc10520j.

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20

Voigt, Melanie, Indra Bartels, Anna Nickisch-Hartfiel, and Martin Jaeger. "Elimination of macrolides in water bodies using photochemical oxidation." AIMS Environmental Science 5, no. 5 (2018): 372–88. http://dx.doi.org/10.3934/environsci.2018.5.372.

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21

I. Litter, Marta, and Natalia Quici. "Photochemical Advanced Oxidation Processes for Water and Wastewater Treatment." Recent Patents on Engineering 4, no. 3 (November 1, 2010): 217–41. http://dx.doi.org/10.2174/187221210794578574.

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22

Sartorel, Andrea, Marcella Bonchio, Sebastiano Campagna, and Franco Scandola. "ChemInform Abstract: Tetrametallic Molecular Catalysts for Photochemical Water Oxidation." ChemInform 44, no. 22 (May 13, 2013): no. http://dx.doi.org/10.1002/chin.201322209.

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23

Braun, André M., and E. Oliveros. "How to evaluate photochemical methods for water treatment." Water Science and Technology 35, no. 4 (February 1, 1997): 17–23. http://dx.doi.org/10.2166/wst.1997.0076.

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Photochemical advanced oxidation processes (AOPs) generally imply generation of hydroxyl radicals which are initiating the oxidative degradation by well defined reactions (hydrogen abstraction, addition and electron transfer) with available organic substrates. This limitation of the scope of applications may be avoided in implementing combinations of different photochemical and/or thermal processes. A simple evaluation of photochemical AOPs is based on the absorption spectrum of the oxidant to be added and on the spectral distribution of the emission of commercially available light sources. Dominating light absorption, in particular in the UV-C spectral domain, by the solutes of the aqueous system to be treated may lead to exclude some of the degradation processes, as excitation of the oxidant and, consequently, production of the initiator become inefficient with increasing inner filter effects. The evaluation of photochemical AOPs in terms of volume independent rates is convenient and highly advocated, but such comparisons should only be made for processes applied to a restricted number of model substrates which are to be degraded in optimized equipment. Taking into account the volume independent rates determined in the range of realistic pollutant concentrations, the number of m3 of contaminated water of known pollutant nature and concentration to be treated per unit of time, the list of a commercially available light sources and their geometry, a final selection of the degradation process or of a combination of processes may be made, and the total electrical energy required and the number of photochemical reactors to be built may be calculated.
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24

Laine, Tanja M., Markus D. Kärkäs, Rong-Zhen Liao, Torbjörn Åkermark, Bao-Lin Lee, Erik A. Karlsson, Per E. M. Siegbahn, and Björn Åkermark. "Efficient photochemical water oxidation by a dinuclear molecular ruthenium complex." Chemical Communications 51, no. 10 (2015): 1862–65. http://dx.doi.org/10.1039/c4cc08606f.

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A dinuclear Ru complex housing an anionic ligand scaffold has been developed. The designed Ru complex was found to efficiently mediate the photochemical oxidation of H2O when using [Ru(bpy)3]2+-type photosensitizers.
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25

Gustafson, Karl P. J., Andrey Shatskiy, Oscar Verho, Markus D. Kärkäs, Bastian Schluschass, Cheuk-Wai Tai, Björn Åkermark, Jan-Erling Bäckvall, and Eric V. Johnston. "Water oxidation mediated by ruthenium oxide nanoparticles supported on siliceous mesocellular foam." Catalysis Science & Technology 7, no. 1 (2017): 293–99. http://dx.doi.org/10.1039/c6cy02121b.

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26

Nakazono, Takashi, and Ken Sakai. "Improving the robustness of cobalt porphyrin water oxidation catalysts by chlorination of aryl groups." Dalton Transactions 45, no. 32 (2016): 12649–52. http://dx.doi.org/10.1039/c6dt02535h.

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27

Mori, Naohisa, Yutori Tagoku, Hidenobu Shiroishi, Yoshinobu Saito, Morihiro Saito, and Jun Kuwano. "Basic Research of Water Photolysis Using Pyrochlore Oxides." Key Engineering Materials 388 (September 2008): 297–300. http://dx.doi.org/10.4028/www.scientific.net/kem.388.297.

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Photocatalytic proton reduction and water oxidation have been studied in a tris(2,2’-bipyridyl)ruthenium complex-catalyst system. Pyrochlore-type oxides have been used as proton reduction catalysts with a sacrificial electron donor (Na2EDTA) at pH 7 and as water oxidation catalysts with a sacrificial electron acceptor (K2S2O8) at pH 3. Rate constants for the proton reduction were estimated on the basis of photochemical processes. Yb2Ru2O7-δ was found to be the most active catalyst for proton reduction and water oxidation catalyst in this system.
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28

Braun, A. M., I. G. Pintori, H. P. Popp, Y. Wakahata, and M. Würner. "Technical development of UV-C- and VUV-photochemically induced oxidative degradation processes." Water Science and Technology 49, no. 4 (February 1, 2004): 235–40. http://dx.doi.org/10.2166/wst.2004.0272.

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Technical development work is presented, where the VUV photochemically induced oxidative degradation is used: (i) for analytic purposes, and (ii) for small to medium scale (<10 m2/d) waste water treatment processes or ultrapure water production. In the first case, small Xe-excimer radiation sources with an integrated reaction space designed for optimal conditions, as far as incident photon flux density, turbulence and concentration of dissolved molecular oxygen are concerned, have been built and tested. Under conditions of exhaustive oxidation and/or mineralization of pollutants in a continuous regime, they may be used for sample pre-treatment modules prior TOC, TOX and electrochemical trace metal analysis. Under conditions of partial oxidation or mineralization, the same lamp/reactor combination may be used for functionalization purposes prior to e.g. GC or HPLC analyses. In the second case, mass transfer limitations between the non-irradiated bulk volume and the irradiated volume are overcome by the electrochemical generation of molecular oxygen within or close to the irradiated volume and by the design of the photochemical part of the reactor.
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29

Shylin, Sergii I., Mariia V. Pavliuk, Luca D’Amario, Fikret Mamedov, Jacinto Sá, Gustav Berggren, and Igor O. Fritsky. "Efficient visible light-driven water oxidation catalysed by an iron(iv) clathrochelate complex." Chemical Communications 55, no. 23 (2019): 3335–38. http://dx.doi.org/10.1039/c9cc00229d.

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30

Talaat, Hala A., Montaser Y. Ghaly, Eman M. Kamel, Ahmed M. Awad, and Enas M. Ahmed. "Combined electro-photochemical oxidation for iron removal from ground water." Desalination and Water Treatment 28, no. 1-3 (April 2011): 265–69. http://dx.doi.org/10.5004/dwt.2011.1160.

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31

Kong, Li, and John L. Ferry. "Photochemical oxidation of chrysene at the silica gel–water interface." Journal of Photochemistry and Photobiology A: Chemistry 162, no. 2-3 (March 2004): 415–21. http://dx.doi.org/10.1016/s1010-6030(03)00385-x.

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32

Liu, Hongfei, Mauro Schilling, Maxim Yulikov, Sandra Luber, and Greta R. Patzke. "Homogeneous Photochemical Water Oxidation with Cobalt Chloride in Acidic Media." ACS Catalysis 5, no. 9 (July 30, 2015): 4994–99. http://dx.doi.org/10.1021/acscatal.5b01101.

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33

McGrail, Brendan T., Laura S. Pianowski, and Peter C. Burns. "Photochemical Water Oxidation and Origin of Nonaqueous Uranyl Peroxide Complexes." Journal of the American Chemical Society 136, no. 13 (March 20, 2014): 4797–800. http://dx.doi.org/10.1021/ja502425t.

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34

Shrestha, Sweta, and Prabir K. Dutta. "Photochemical Water Oxidation by Manganese Oxides Supported on Zeolite Surfaces." ChemistrySelect 1, no. 7 (May 16, 2016): 1431–40. http://dx.doi.org/10.1002/slct.201600208.

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35

Lingampalli, S. R., and C. N. R. Rao. "Solar Photochemical Reduction and Oxidation of Water and Related Aspects." Molecular Frontiers Journal 02, no. 01 (January 2018): 19–29. http://dx.doi.org/10.1142/s2529732518500013.

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Conversion of solar energy to useful chemicals has become necessary for finding solutions to energy and environmental issues. One of the means is to use of solar energy for the reduction of water to generate hydrogen or for the reduction of CO[Formula: see text] to useful chemicals. In spite of substantial effort, the discovery of stable and efficient photocatalysts remains a challenge, although some encouraging results have been reported. In this article, we provide a brief perspective of the current status of solar water splitting and reduction of CO[Formula: see text].
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36

Konhauser, Kurt O., Larry Amskold, Stefan V. Lalonde, Nicole R. Posth, Andreas Kappler, and Ariel Anbar. "Decoupling photochemical Fe(II) oxidation from shallow-water BIF deposition." Earth and Planetary Science Letters 258, no. 1-2 (June 2007): 87–100. http://dx.doi.org/10.1016/j.epsl.2007.03.026.

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37

Zhang, Mei, Yong-Liang Huang, Jia-Wei Wang, and Tong-Bu Lu. "A facile method for the synthesis of a porous cobalt oxide–carbon hybrid as a highly efficient water oxidation catalyst." Journal of Materials Chemistry A 4, no. 5 (2016): 1819–27. http://dx.doi.org/10.1039/c5ta07813j.

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38

Hamilton, J. W. J., J. A. Byrne, P. S. M. Dunlop, and N. M. D. Brown. "Photo-Oxidation of Water Using Nanocrystalline Tungsten Oxide under VisibleLight." International Journal of Photoenergy 2008 (2008): 1–5. http://dx.doi.org/10.1155/2008/185479.

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The photoelectrolysis of water to yield hydrogen and oxygen using visible light has enormous potential for solar energy harvesting if suitable photoelectrode materials can be developed. Few of the materials with a band gap suitable for visible light activation have the necessary band-edge potentials or photochemical stability to be suitable candidates. Tungsten oxide ( 2.8 eV) is a good candidate with absorption up to nm and known photochemical stability. Thin films of tungsten oxide were prepared using an electrolytic route from peroxo-tungsten precursors. The tungsten oxide thin films were characterised by FESEM, Auger electron spectroscopy, and photoelectrochemical methods. The magnitude of the photocurrent response of the films under solar simulated irradiation showed a dependence on precursor used in the film preparation, with a comparatively lower response for samples containing impurities. The photocurrent response spectrum of the tungsten oxide films was more favourable than that recorded for titanium dioxide () thin films. The photocurrent response was of equivalent magnitude but shifted into the visible region of the spectrum, as compared to that of the .
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39

Li, Ting-Ting, Wei-Liang Zhao, Yong Chen, Fu-Min Li, Chuan-Jun Wang, Yong-Hua Tian, and Wen-Fu Fu. "Photochemical, Electrochemical, and Photoelectrochemical Water Oxidation Catalyzed by Water-Soluble Mononuclear Ruthenium Complexes." Chemistry - A European Journal 20, no. 43 (September 9, 2014): 13957–64. http://dx.doi.org/10.1002/chem.201403872.

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40

Tsubonouchi, Yuta, Shu Lin, Alexander R. Parent, Gary W. Brudvig, and Ken Sakai. "Light-induced water oxidation catalyzed by an oxido-bridged triruthenium complex with a Ru–O–Ru–O–Ru motif." Chemical Communications 52, no. 51 (2016): 8018–21. http://dx.doi.org/10.1039/c6cc02816k.

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A μ-oxido-bridged triruthenium complex (RuT2+), formed by air oxidation of a previously reported monoruthenium water-oxidation catalyst (WOC), serves as an efficient photochemical WOC with the turnover frequency (TOF) and turnover number (TON) 0.90 s−1 and 610, respectively.
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41

Asraf, Md Ali, Chizoba I. Ezugwu, C. M. Zakaria, and Francis Verpoort. "Homogeneous photochemical water oxidation with metal salophen complexes in neutral media." Photochemical & Photobiological Sciences 18, no. 11 (2019): 2782–91. http://dx.doi.org/10.1039/c9pp00254e.

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42

Sougrati, Moulay T., Jeethu J. Arayamparambil, Xiaohui Liu, Markus Mann, Adam Slabon, Lorenzo Stievano, and Richard Dronskowski. "Carbodiimides as energy materials: which directions for a reasonable future?" Dalton Transactions 47, no. 32 (2018): 10827–32. http://dx.doi.org/10.1039/c8dt01846d.

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43

Salim, Márcia M. F. F., Aline Novack, Petrick A. Soares, Ângela Medeiros, Miguel A. Granato, Antonio A. U. Souza, Vítor J. P. Vilar, and Selene M. A. Guelli U. Souza. "Photochemical UVC/H2O2 oxidation system as an effective method for the decolourisation of bio-treated textile wastewaters: towards onsite water reuse." RSC Advances 6, no. 93 (2016): 90631–45. http://dx.doi.org/10.1039/c6ra15615k.

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A photochemical UVC/H2O2 oxidation system was applied for the decolourisation of two real textile wastewaters collected after biological oxidation from two different textile wastewater treatment plants.
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44

Lee, A. K. Y., K. L. Hayden, P. Herckes, W. R. Leaitch, J. Liggio, A. M. Macdonald, and J. P. D. Abbatt. "Characterization of aerosol and cloud water at a mountain site during WACS 2010: secondary organic aerosol formation through oxidative cloud processing." Atmospheric Chemistry and Physics Discussions 12, no. 2 (February 24, 2012): 6019–47. http://dx.doi.org/10.5194/acpd-12-6019-2012.

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Abstract. The water-soluble fractions of aerosol samples and cloud water collected during Whistler Aerosol and Cloud Study (WACS 2010) were analyzed using an Aerodyne aerosol mass spectrometer (AMS). This is the first study to report AMS organic spectra of re-aerosolized cloud water, and to make direct comparison between the AMS spectra of cloud water and aerosol samples collected at the same location. In general, the aerosol and cloud organic spectra were very similar, indicating that the cloud water organics likely originated from secondary organic aerosol (SOA) formed nearby. By using a photochemical reactor to oxidize both aerosol filter extracts and cloud water, we find evidence that fragmentation of aerosol water-soluble organics increases their volatility during oxidation. By contrast, enhancement of AMS-measurable organic mass by up to 30% was observed during aqueous-phase photochemical oxidation of cloud water organics. We propose that additional SOA material was produced by functionalizing dissolved organics via OH oxidation, where these dissolved organics are sufficiently volatile that they are not usually part of the aerosol. This work points out that water-soluble organic compounds of intermediate volatility (IVOC), such as cis-pinonic acid, produced via gas-phase oxidation of monoterpenes, can be important aqueous-phase SOA precursors in a biogenic-rich environment.
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45

Lee, A. K. Y., K. L. Hayden, P. Herckes, W. R. Leaitch, J. Liggio, A. M. Macdonald, and J. P. D. Abbatt. "Characterization of aerosol and cloud water at a mountain site during WACS 2010: secondary organic aerosol formation through oxidative cloud processing." Atmospheric Chemistry and Physics 12, no. 15 (August 6, 2012): 7103–16. http://dx.doi.org/10.5194/acp-12-7103-2012.

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Abstract. The water-soluble fractions of aerosol filter samples and cloud water collected during the Whistler Aerosol and Cloud Study (WACS 2010) were analyzed using an Aerodyne aerosol mass spectrometer (AMS). This is the first study to report AMS organic spectra of re-aerosolized cloud water, and to make direct comparison between the AMS spectra of cloud water and aerosol samples collected at the same location. In general, the mass spectra of aerosol were very similar to those of less volatile cloud organics. By using a photochemical reactor to oxidize both aerosol filter extracts and cloud water, we find evidence that fragmentation of water-soluble organics in aerosol increases their volatility during photochemical oxidation. By contrast, enhancement of AMS-measurable organic mass by up to 30% was observed during the initial stage of oxidation of cloud water organics, which was followed by a decline at the later stages of oxidation. These observations are in support of the general hypothesis that cloud water oxidation is a viable route for SOA formation. In particular, we propose that additional SOA material was produced by functionalizing dissolved organics via OH oxidation, where these dissolved organics are sufficiently volatile that they are not usually part of the aerosol. This work demonstrates that water-soluble organic compounds of intermediate volatility (IVOC), such as cis-pinonic acid, produced via gas-phase oxidation of monoterpenes, can be important aqueous-phase SOA precursors in a biogenic-rich environment.
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46

Sato, Yoichi, Shin-ya Takizawa, and Shigeru Murata. "Photochemical water oxidation system using ruthenium catalysts embedded into vesicle membranes." Journal of Photochemistry and Photobiology A: Chemistry 321 (May 2016): 151–60. http://dx.doi.org/10.1016/j.jphotochem.2016.02.003.

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47

He, Feng, Weirong Zhao, Liyuan Liang, and Baohua Gu. "Photochemical Oxidation of Dissolved Elemental Mercury by Carbonate Radicals in Water." Environmental Science & Technology Letters 1, no. 12 (November 12, 2014): 499–503. http://dx.doi.org/10.1021/ez500322f.

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48

Smith, R. D. L., S. Trudel, and C. P. Berlinguette. "Photochemical Route for the Preparation of Complex Amorphous Water Oxidation Catalyst." ECS Transactions 58, no. 45 (April 22, 2014): 67–76. http://dx.doi.org/10.1149/05845.0067ecst.

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49

Wee, Tse-Luen, Benjamin D. Sherman, Devens Gust, Ana L. Moore, Thomas A. Moore, Yun Liu, and Juan C. Scaiano. "Photochemical Synthesis of a Water Oxidation Catalyst Based on Cobalt Nanostructures." Journal of the American Chemical Society 133, no. 42 (October 26, 2011): 16742–45. http://dx.doi.org/10.1021/ja206280g.

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50

Shevchenko, Denys, Magnus F. Anderlund, Anders Thapper, and Stenbjörn Styring. "Photochemical water oxidation with visible light using a cobalt containing catalyst." Energy & Environmental Science 4, no. 4 (2011): 1284. http://dx.doi.org/10.1039/c0ee00585a.

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