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Journal articles on the topic 'Reduction (Chemistry) Electrolytic reduction'

Author: Grafiati

Published: 4 June 2021

Last updated: 13 February 2022

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1

Knittel, Dierk, and V. Suryanarayana Rao. "Electrolytic reduction of azidochalcones." Monatshefte für Chemie - Chemical Monthly 117, no. 10 (October 1986): 1185–93. http://dx.doi.org/10.1007/bf00811331.

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2

Merica, Simona G., Wojceich Jedral, Susan Lait, Peter Keech, and Nigel J. Bunce. "Electrochemical reduction and oxidation of DDT." Canadian Journal of Chemistry 77, no. 7 (July 1, 1999): 1281–87. http://dx.doi.org/10.1139/v99-113.

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Electrolysis has been studied as a possible method to treat DDT wastes. In methanol, the major process was dehydrochlorination to DDE followed by further reduction. In an aqueous emulsion containing 1% heptane and 0.1% Triton SP-175®, DDT was reduced at a deposited lead electrode with sodium sulphate as the supporting electrolyte by sequential hydrodechlorination of the aliphatic chlorine atoms. An excellent material balance was achieved, but the current efficiency was poor, even at low current densities. Electrooxidation of DDT was also investigated; in aqueous solutions or emulsion, little oxidation occurred because of competing oxidation of water at the highly positive potentials needed to oxidize DDT. In acetonitrile, electrooxidation occurred with high current efficiency by way of "electrochemical combustion" of DDT and its intermediate oxidation products to CO2. We conclude that development of an electrolytic technology for destroying DDT wastes is unlikely.Key words: electroreduction, electrooxidation, voltammetry, surfactant media.

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3

Li, Tengfei, Yang Cao, Jingfu He, and Curtis P. Berlinguette. "Electrolytic CO2 Reduction in Tandem with Oxidative Organic Chemistry." ACS Central Science 3, no. 7 (June 28, 2017): 778–83. http://dx.doi.org/10.1021/acscentsci.7b00207.

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4

Ouyang, Yixin, Yehui Zhang, Peter S. Rice, Li Shi, Jinlan Wang, and P. Hu. "Electrochemical CO2 reduction: water/catalyst interface versus polymer/catalyst interface." Journal of Materials Chemistry A 9, no. 32 (2021): 17474–80. http://dx.doi.org/10.1039/d1ta04867h.

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Alkaline polymer electrolyte electrolytic cells (APEECs) have the potential to replace aqueous-phase CO2 electrolyzer. Full reaction kinetics at polymer/copper interface is obtained to present a fundamental understanding of the superiority of APEECs.

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5

Weekes, David M., Danielle A. Salvatore, Angelica Reyes, Aoxue Huang, and Curtis P. Berlinguette. "Electrolytic CO2 Reduction in a Flow Cell." Accounts of Chemical Research 51, no. 4 (March 23, 2018): 910–18. http://dx.doi.org/10.1021/acs.accounts.8b00010.

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6

Hlavatý, Jaromír. "Electrolytic reduction of o-nitrobenzyl thiocyanate in buffered solutions on mercury." Collection of Czechoslovak Chemical Communications 50, no. 1 (1985): 33–41. http://dx.doi.org/10.1135/cccc19850033.

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The o-nitrobenzyl thiocyanate (I) behaves differently on the DME and on a large mercury pool electrode. Polarography did not give a sufficiently clear explanation of the reaction mechanism, only the preparative experiments yielded useful results. Whereas polarographic curves in solutions of Britton-Robinson buffer system with 50% by vol. ethanol exhibit two cathodic waves within the pH region 1-12, corresponding according to their height ratio to an uptake of 4 e and 2 e respectively, the controlled potential preparation electrolysis (CPE) and coulometry results indicate a more complicated reaction path. In the CPE carried out at the concentration of I 1 . 10 -2 mol/l the electroreductive splitting of CH2-SCN occurs as the first step. Nitrobenzyl radicals so formed react in the follow-up dimerization resulting in dibenzyl or toluene structures. Simultaneously or at a later stage the completion of the electrolytic reduction of the nitro group proceeds to the hydroxylamino group. In solution of 9 > pH > 1 the CPE of nitro compound I takes place by an ECEC mechanism yielding dibenzodiazocine III, its N-oxide IV and 2,2'-dimethylazoxybenzene (V). In course of preparative electrolysis in strongly acidic medium 2-amino-benzo(l,3)-thiazine-l-oxide (II) is formed by an EC mechanism.

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7

Moore, William, Wade Henke, Davide Lionetti, Victor Day, and James Blakemore. "Single-Electron Redox Chemistry on the [Cp*Rh] Platform Enabled by a Nitrated Bipyridyl Ligand." Molecules 23, no. 11 (November 2, 2018): 2857. http://dx.doi.org/10.3390/molecules23112857.

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[Cp*Rh] complexes (Cp* = pentamethylcyclopentadienyl) are attracting renewed interest in coordination chemistry and catalysis, but these useful compounds often undergo net two-electron redox cycling that precludes observation of individual one-electron reduction events. Here, we show that a [Cp*Rh] complex bearing the 4,4′-dinitro-2,2′-bipyridyl ligand (dnbpy) (3) can access a distinctive manifold of five oxidation states in organic electrolytes, contrasting with prior work that found no accessible reductions in aqueous electrolyte. These states are readily generated from a newly isolated and fully characterized rhodium(III) precursor complex 3, formulated as [Cp*Rh(dnbpy)Cl]PF6. Single-crystal X-ray diffraction (XRD) data, previously unavailable for the dnbpy ligand bound to the [Cp*Rh] platform, confirm the presence of both [η5-Cp*] and [κ2-dnbpy]. Four individual one-electron reductions of 3 are observed, contrasting sharply with the single two-electron reductions of other [Cp*Rh] complexes. Chemical preparation and the study of the singly reduced species with electronic absorption and electron paramagnetic resonance spectroscopies indicate that the first reduction is predominantly centered on the dnbpy ligand. Comparative cyclic voltammetry studies with [NBu4][PF6] and [NBu4][Cl] as supporting electrolytes indicate that the chloride ligand can be lost from 3 by ligand exchange upon reduction. Spectroelectrochemical studies with ultraviolet (UV)-visible detection reveal isosbestic behavior, confirming the clean interconversion of the reduced forms of 3 inferred from the voltammetry with [NBu4][PF6] as supporting electrolyte. Electrochemical reduction in the presence of triethylammonium results in an irreversible response, but does not give rise to catalytic H2 evolution, contrasting with the reactivity patterns observed in [Cp*Rh] complexes bearing bipyridyl ligands with less electron-withdrawing substituents.

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8

Gilbert, David M., and Tom C. Sale. "Sequential Electrolytic Oxidation and Reduction of Aqueous Phase Energetic Compounds." Environmental Science & Technology 39, no. 23 (December 2005): 9270–77. http://dx.doi.org/10.1021/es051452k.

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9

Yan, Xiao Y., and Derek J. Fray. "Direct electrolytic reduction of solid alumina using molten calcium chloride-alkali chloride electrolytes." Journal of Applied Electrochemistry 39, no. 8 (February 11, 2009): 1349–60. http://dx.doi.org/10.1007/s10800-009-9808-3.

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10

Xie, Kaiyu, and Ali Reza Kamali. "Electro-reduction of hematite using water as the redox mediator." Green Chemistry 21, no. 2 (2019): 198–204. http://dx.doi.org/10.1039/c8gc02756k.

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11

Qiu, Guohong, Kai Jiang, Meng Ma, Dihua Wang, Xianbo Jin, and George Z. Chen. "Roles of Cationic and Elemental Calcium in the Electro-Reduction of Solid Metal Oxides in Molten Calcium Chloride." Zeitschrift für Naturforschung A 62, no. 5-6 (June 1, 2007): 292–302. http://dx.doi.org/10.1515/zna-2007-5-610.

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Previous work, mainly from this research group, is re-visited on electrochemical reduction of solid metal oxides, in the form of compacted powder, in molten CaCl2, aiming at further understanding of the roles of cationic and elemental calcium. The discussion focuses on six aspects: 1.) debate on two mechanisms proposed in the literature, i. e. electro-metallothermic reduction and electro-reduction (or electro-deoxidation), for the electrolytic removal of oxygen from solid metals or metal oxides in molten CaCl2; 2.) novel metallic cavity working electrodes for electrochemical investigations of compacted metal oxide powders in high temperature molten salts assisted by a quartz sealed Ag/AgCl reference electrode (650 ºC- 950 ºC); 3.) influence of elemental calcium on the background current observed during electrolysis of solid metal oxides in molten CaCl2; 4.) electrochemical insertion/ inclusion of cationic calcium into solid metal oxides; 5.) typical features of cyclic voltammetry and chronoamperometry (potentiostatic electrolysis) of metal oxide powders in molten CaCl2; and 6.) some kinetic considerations on the electrolytic removal of oxygen.

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12

Gao, Y. M., B. Wang, S. B. Wang, and S. Peng. "Study on electrolytic reduction with controlled oxygen flow for iron from molten oxide slag containing FeO." Journal of Mining and Metallurgy, Section B: Metallurgy 49, no. 1 (2013): 49–55. http://dx.doi.org/10.2298/jmmb120112036g.

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A ZrO2-based solid membrane electrolytic cell with controlled oxygen flow was constructed: graphite rod /[O]Fe+C saturated / ZrO2(MgO)/(FeO) slag/iron crucible. The feasibility of extraction of iron from molten oxide slag containing FeO at an applied voltage was investigated by means of the electrolytic cell. The effects of some important process factors on the FeO electrolytic reduction with the controlled oxygen flow were discussed. The results show that: solid iron can be extracted from molten oxide slag containing FeO at 1450?C and an applied potential of 4V. These factors, such as precipitation and growth of solid iron dendrites, change of the cathode active area on the inner wall of the iron crucible and ion diffusion flux in the molten slag may affect the electrochemical reaction rate. The reduction for Fe2+ ions mainly appears on new iron dendrites of the iron crucible cathode, and a very small amount of iron are also formed on the MSZ (2.18% MgO partially stabilized zirconia) tube/slag interface due to electronic conductance of MSZ tube. Internal electronic current through MSZ tube may change direction at earlier and later electrolytic reduction stage. It has a role of promoting electrolytic reduction for FeO in the molten slag at the earlier stage, but will lower the current efficiency at the later stage. The final reduction ratio of FeO in the molten slag can achieve 99%. A novel electrolytic method with controlled oxygen flow for iron from the molten oxide slag containing FeO was proposed. The theory of electrolytic reduction with the controlled oxygen flow was developed.

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13

Xu, Yun, Kevin Wood, Jaclyn Coyle, Chaiwat Engtrakul, Glenn Teeter, Conrad Stoldt, Anthony Burrell, and Andriy Zakutayev. "Chemistry of Electrolyte Reduction on Lithium Silicide." Journal of Physical Chemistry C 123, no. 21 (May 7, 2019): 13219–24. http://dx.doi.org/10.1021/acs.jpcc.9b02611.

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14

Snook, Graeme A., Katherine McGregor, Andrew J. Urban, Marshall R. Lanyon, R. Donelson, and Mark I. Pownceby. "Development of a niobium-doped titania inert anode for titanium electrowinning in molten chloride salts." Faraday Discussions 190 (2016): 35–52. http://dx.doi.org/10.1039/c5fd00235d.

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The direct electrochemical reduction of solid titanium dioxide in a chloride melt is an attractive method for the production of titanium metal. It has been estimated that this type of electrolytic approach may reduce the costs of producing titanium sponge by more than half, with the additional benefit of a smaller environmental footprint. The process utilises a consumable carbon anode which releases a mixture of CO₂and CO gas during electrolysis, but suffers from low current efficiency due to the occurrence of parasitic side reactions involving carbon. The replacement of the carbon anode with a cheap, robust inert anode offers numerous benefits that include: elimination of carbon dioxide emissions, more efficient cell operation, opportunity for three-dimensional electrode configurations and reduced electrode costs. This paper reports a study of Nb-doped titania anode materials for inert anodes in a titanium electrolytic reduction cell. The study examines the effect of niobium content and sintering conditions on the performance of Nb-doped TiO₂anodes in laboratory-scale electrolysis tests. Experimental findings, including performance in a 100 h laboratory electrolysis test, are described.

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15

Vieira, Kenneth L., and Dennis G. Peters. "Electrolytic reduction of tert-butyl bromide at mercury cathodes in dimethylformamide." Journal of Organic Chemistry 51, no. 8 (April 1986): 1231–39. http://dx.doi.org/10.1021/jo00358a013.

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16

Clark II, Clayton J. "Reduction of a field generated waste microemulsion by electrolytic addition." Journal of Environmental Engineering and Science 4, no. 1 (January 2005): 83–87. http://dx.doi.org/10.1139/s04-057.

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17

Kipouros, Georges J., and Ram A. Sharma. "Electrolytic Regeneration of the Neodymium Oxide Reduction‐Spent Salt." Journal of The Electrochemical Society 137, no. 11 (November 1, 1990): 3333–38. http://dx.doi.org/10.1149/1.2086218.

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18

Wang, Xun, Jing Yang, Manohar Salla, Shibo Xi, Yi Yang, Mengsha Li, Feifei Zhang, et al. "Redox‐Mediated Ambient Electrolytic Nitrogen Reduction for Hydrazine and Ammonia Generation." Angewandte Chemie International Edition 60, no. 34 (July 16, 2021): 18721–27. http://dx.doi.org/10.1002/anie.202105536.

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19

Satyawali, Yamini, Tom Van de Wiele, Hans Saveyn, Paul Van der Meeren, and Willy Verstraete. "Electrolytic reduction improves treatability of humic acids containing water streams." Journal of Chemical Technology & Biotechnology 82, no. 8 (2007): 730–37. http://dx.doi.org/10.1002/jctb.1715.

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20

Awakura, Yasuhiro, Hiroshi Hiai, Hiroshi Majima, and Shuichiro Hirono. "Fundamental studies on the continuous electrolytic reduction of uranyl sulfate." Metallurgical and Materials Transactions B 20, no. 3 (June 1989): 337–43. http://dx.doi.org/10.1007/bf02696986.

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21

Shu, Jiancheng, Renlong Liu, Zuohua Liu, Hongliang Chen, and Changyuan Tao. "Leaching of manganese from electrolytic manganese residue by electro-reduction." Environmental Technology 38, no. 16 (October 21, 2016): 2077–84. http://dx.doi.org/10.1080/09593330.2016.1245789.

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22

Sa, Young Jin, Chan Woo Lee, Si Young Lee, Jonggeol Na, Ung Lee, and Yun Jeong Hwang. "Catalyst–electrolyte interface chemistry for electrochemical CO2 reduction." Chemical Society Reviews 49, no. 18 (2020): 6632–65. http://dx.doi.org/10.1039/d0cs00030b.

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23

Kunugi, Akira, Norimasa Takahashi, Kyo Abe, and Taketsugu Hirai. "The Electrolytic Reduction ofp-Substituted α-(Methylsulfinyl)-α-(methylthio)acetophenones in Acetonitrile." Bulletin of the Chemical Society of Japan 62, no. 6 (June 1989): 2055–57. http://dx.doi.org/10.1246/bcsj.62.2055.

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24

Toyoshima, Atsushi, Zijie Li, Masato Asai, Nozomi Sato, Tetsuya K. Sato, Takahiro Kikuchi, Yusuke Kaneya, et al. "Measurement of the Md3+/Md2+ Reduction Potential Studied with Flow Electrolytic Chromatography." Inorganic Chemistry 52, no. 21 (October 11, 2013): 12311–13. http://dx.doi.org/10.1021/ic401571h.

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25

Ramus, Terry L., and Lawrence C. Thomas. "Temperature selection for chlorinated hydrocarbon reduction for the hall electrolytic conductivity detector." Journal of Chromatography A 328 (January 1985): 342–46. http://dx.doi.org/10.1016/s0021-9673(01)87406-9.

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26

Kadowaki, Haruna, Yumi Katasho, Kouji Yasuda, and Toshiyuki Nohira. "Electrolytic Reduction of Solid Al2O3to Liquid Al in Molten CaCl2." Journal of The Electrochemical Society 165, no. 2 (2018): D83—D89. http://dx.doi.org/10.1149/2.1191802jes.

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27

Okubayashi, S., A. Yamazaki, Y. Koide, and H. Shosenji. "Effects of cyclodextrin on the electrolytic reduction of an anthraquinone dye." Coloration Technology 115, no. 10 (October 1999): 312–17. http://dx.doi.org/10.1111/j.1478-4408.1999.tb00385.x.

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28

Li, Liang, Yafeng Yun, Yuezhi Zhang, Yuanxing Huang, and Zhihua Xu. "Electrolytic reduction of nitrate on copper and its binary composite electrodes." Journal of Alloys and Compounds 766 (October 2018): 157–60. http://dx.doi.org/10.1016/j.jallcom.2018.07.004.

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29

Chen, Chaoyi, Xiaqiong Yang, Junqi Li, Xionggang Lu, and Shufeng Yang. "Direct Electrolytic Reduction of Solid Ta2O5 to Ta with SOM Process." Metallurgical and Materials Transactions B 47, no. 3 (March 10, 2016): 1727–35. http://dx.doi.org/10.1007/s11663-016-0633-x.

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30

Park, B. H., I. W. Lee, and C. S. Seo. "Electrolytic reduction behavior of U3O8 in a molten LiCl–Li2O salt." Chemical Engineering Science 63, no. 13 (July 2008): 3485–92. http://dx.doi.org/10.1016/j.ces.2008.04.021.

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31

Wang, Bo, Chao-yi Chen, Jun-qi Li, Lin-zhu Wang, Yuan-pei Lan, and Shi-yu Wang. "Solid oxide membrane-assisted electrolytic reduction of Cr2O3 in molten CaCl2." International Journal of Minerals, Metallurgy and Materials 27, no. 12 (December 2020): 1626–34. http://dx.doi.org/10.1007/s12613-020-2141-x.

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32

OYAMA, Munetaka, Mikio OKADA, and Satoshi OKAZAKI. "Electrochemical Reduction of Cytochrome c by Using a Column-Electrolytic Continuous-Flow Method." Denki Kagaku oyobi Kogyo Butsuri Kagaku 61, no. 7 (July 5, 1993): 778–79. http://dx.doi.org/10.5796/electrochemistry.61.778.

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33

Majima, Hiroshi, Yasuhiro Awakura, Koji Sato, and Shuichiro Hirono. "Laboratory reduction rate and current efficiency studies of batch type electrolytic reduction of U(VI) in a sulfate system." Metallurgical Transactions B 17, no. 1 (January 1986): 69–76. http://dx.doi.org/10.1007/bf02670820.

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34

Li, Changzhen, Rui Xiong, Di Yin, Zheng Tang, Junfeng Wang, Dahua Li, Zuxing Yu, and Jing Shi. "Single crystal Tl0.3MoO3 growth by electrolytic reduction method of a Tl2CO3–MoO3 melts." Journal of Crystal Growth 285, no. 1-2 (November 2005): 81–87. http://dx.doi.org/10.1016/j.jcrysgro.2005.07.051.

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35

Ji, Nan, Tiejian Zhu, Hao Peng, Feng Jiang, Wei Huang, and Yu Gong. "The Electrolytic Reduction of Gd2O3 in LiCl-KCl-Li2O Molten Salt." Journal of The Electrochemical Society 168, no. 8 (August 1, 2021): 082512. http://dx.doi.org/10.1149/1945-7111/ac1f59.

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36

Ogawa, Kazuya, Yuria Umetsu, and Kenji Kamimura. "Changes in the absorption spectra and colour of tetraphenylporphyrins after redox reactions." Journal of Chemical Research 44, no. 9-10 (March 12, 2020): 613–17. http://dx.doi.org/10.1177/1747519820910915.

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In this study, we have investigated the electrochromic properties including the change in absorption spectra and colour after oxidation and reduction reactions of tetraphenylporphyrin and its metal complexes in dichloromethane. The first oxidation potential is determined from CV measurements, and the reduction potential is estimated from comparison with literature values. Electrolytic reactions are carried out by applying the oxidation potential and reduction potential to each sample solution. The metals used are Ag(II), Cu(II), Fe(III), Mg(II), Mn(III), Ni(II) and Zn(II). Various colours can be expressed after the redox reactions by changing the central metal.

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37

Li, Liang, Yuemei Zhou, Yuezhi Zhang, Yuanxing Huang, and Ramesh Goel. "Enhanced Electrolytic Nitrate Reduction Utilizing a Three-Dimensional Electrolysis Reactor Packed with Activated Carbon and Foamed Copper." Environmental Engineering Science 33, no. 8 (August 2016): 525–35. http://dx.doi.org/10.1089/ees.2016.0075.

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38

Hlavatý, Jaromír, and Jiří Volke. "Use of Nafion membranes in laboratory organic electrosynthesis." Collection of Czechoslovak Chemical Communications 53, no. 12 (1988): 3164–70. http://dx.doi.org/10.1135/cccc19883164.

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Electrolysis of quaternary ammonium bromides and iodides in a divided cell with a Nafion membrane yields quaternary polyhalogenides at a carbon anode in water-ethanolic anolytes. The electrodialysis of tetrabutylammonium iodide in a cell with a Nafion membrane enables generation of tetrabutylammonium hydroxide. In electrolytic reduction of nitrobenzene in presence of 1,3-dibromopropane, N-phenylisooxazolidine results in an approx. 60% yield. This electrosynthesis takes place in dimethylformamide with tetrabutylammonium bromide at a glassy-carbon cathode in a divided cell. In the electroreduction of lobelanine hydrogensulfate in a divided cell in acid water-ethanolic media at a lead cathode prevalently lobelanidine has been obtained.

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39

Wu, Fangfang, Zhu Xiao, Bin Zeng, Long Chen, Hui Liu, Min Liang, Peng Yu, and Baobin Mi. "Experimental and reduction leaching kinetics simulation of iron-rich manganese oxide ore using tobacco stem concrete as reducing agent." Metallurgical Research & Technology 116, no. 4 (2019): 422. http://dx.doi.org/10.1051/metal/2019017.

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Reduction leaching behaviors of Fe and Mn from an iron-rich manganese oxide ore using waste tobacco stem concrete as reducing agent were investigated in this paper with a view to determining the feasibility of tobacco stem concrete used in reduction leaching of Mn from iron-rich manganese oxide ore. Results indicated that the leaching processes of Fe and Mn were both dominated by internal diffusion, but the effects of leaching parameters on leaching ratios of Fe and Mn were different based on established leaching kinetic equations. The leaching ratio of Mn reached up to 96.18% while that of Fe kept a lower concentration (17.66%) under optimal leaching conditions, which achieved high selectivity recovery of Mn from iron-rich manganese oxide ore. In addition, the leached solution can be used as electrolytic stock solution in the production of electrolytic manganese. Characterization of the obtained electrolytic manganese product indicated that the quality of electrolytic manganese fully met the standards of YB/T 051-2003, which disclosing a novel recycling approach of utilizing the resource coming from the tobacco industry.

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40

Delima, Roxanna S., Rebecca S. Sherbo, David J. Dvorak, Aiko Kurimoto, and Curtis P. Berlinguette. "Supported palladium membrane reactor architecture for electrocatalytic hydrogenation." Journal of Materials Chemistry A 7, no. 46 (2019): 26586–95. http://dx.doi.org/10.1039/c9ta07957b.

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41

Fujimoto, Kotaro, Yuji Ueda, Tomoya Ishida, Yasuhiro Fujii, and Masaharu Nakayama. "Heat-Treated Electrolytic Manganese Dioxide as an Efficient Catalyst for Oxygen Reduction Reaction in Alkaline Electrolyte." Journal of The Electrochemical Society 168, no. 8 (August 1, 2021): 086510. http://dx.doi.org/10.1149/1945-7111/ac1fb0.

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42

Kim, Seo Ju, Ja Yang Koo, Taeeun Mun, Mingi Choi, and Wonyoung Lee. "Tailoring defect chemistry at interfaces for promoted oxygen reduction reaction kinetics." Journal of Materials Chemistry A 8, no. 44 (2020): 23313–22. http://dx.doi.org/10.1039/d0ta06581a.

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Engineering the defect chemistry at the interface between the electrolyte and the electrode is crucial to facilitate oxygen reduction reaction, thereby improve the electrochemical performance of intermediate temperature solid oxide fuel cells.

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43

Kuntyi, Orest, Oleg Bilan, Viktor Yavorskyi, and Yevhen Okhremchuk. "Cadmium electrochemical reduction in CdCl2 solutions in dimethylsulfoxide and morphology of cathode deposit." Chemistry & Chemical Technology 1, no. 1 (March 15, 2007): 23–26. http://dx.doi.org/10.23939/chcht01.01.023.

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Cadmium reduction in solutions at steady-state and pulse electrolysis has been studied. It was established that polarization results in cadmium formation at potentials 1 V larger than equilibrium one. In 0.25-1.0 molar solutions of CdCl2 concentrated depolarization leads to removement of the beginning of cadmium reduction by 0.3 V. Photographs of SEM are presented and effect of electrolysis characteristics on the morphology of cathode deposit is shown.

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44

Kim, Sung-Wook, Sang-Kwon Lee, Hyun Woo Kang, Eun-Young Choi, Wooshin Park, Sun-Seok Hong, Seung-Chul Oh, and Jin-Mok Hur. "Electrochemical properties of noble metal anodes for electrolytic reduction of uranium oxide." Journal of Radioanalytical and Nuclear Chemistry 311, no. 1 (November 16, 2016): 809–14. http://dx.doi.org/10.1007/s10967-016-5107-8.

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45

Park, B. H., S. B. Park, S. M. Jeong, C. S. Seo, and S. W. Park. "Electrolytic reduction of spent oxide fuel in a molten LiCl-Li2O system." Journal of Radioanalytical and Nuclear Chemistry 270, no. 3 (December 2006): 575–83. http://dx.doi.org/10.1007/s10967-006-0464-3.

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46

Gard, J. C., Y. Mugnier, Y. Huang, and J. Lessard. "Reduction mechanism of 4-nitrobenzophenone in tetrahydrofuran. Influence of added proton donors." Canadian Journal of Chemistry 71, no. 3 (March 1, 1993): 325–30. http://dx.doi.org/10.1139/v93-048.

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In tetrahydrofuran, with tetrabutylammonium hexafluorophosphate as supporting electrolyte, 4-nitrobenzophenone is reduced to the radical anion and, at a more negative potential, to the dianion. These two species are stable even on the time scale of electrolysis. In the presence of proton donors of increasing strength, the dianion is protonated to ArNO2H− but the radical anion is protonated to ArNO2H• only with the strongest acids. These species react further and the different mechanisms are discussed.

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47

Kumar, Ritesh, and Abhishek K. Singh. "Electronic Structure Based Intuitive Design Principle of Single‐Atom Catalysts for Efficient Electrolytic Nitrogen Reduction." ChemCatChem 12, no. 21 (September 4, 2020): 5456–64. http://dx.doi.org/10.1002/cctc.202000902.

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48

Kunugi, Akira, Kyo Abe, Toshio Hagi, and Taketsugu Hirai. "Electrolytic Reduction of 1-Methylsulfinyl-1-methylthio-1-alkenes at Mercury Electrode in Nonaqueous Media." Bulletin of the Chemical Society of Japan 59, no. 6 (June 1986): 2009–10. http://dx.doi.org/10.1246/bcsj.59.2009.

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49

Petrova, G. N., O. N. Efimov, and O. A. Tutochkina. "Electrolytic reduction of acetylene catalyzed by complexes of Ti(III) and Mo(III) with pyrocatechol." Bulletin of the Academy of Sciences of the USSR Division of Chemical Science 37, no. 1 (January 1988): 28–32. http://dx.doi.org/10.1007/bf00962651.

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Myren, Tessa H. T., Taylor A. Stinson, Zachary J. Mast, Chloe G. Huntzinger, and Oana R. Luca. "Chemical and Electrochemical Recycling of End-Use Poly(ethylene terephthalate) (PET) Plastics in Batch, Microwave and Electrochemical Reactors." Molecules 25, no. 12 (June 13, 2020): 2742. http://dx.doi.org/10.3390/molecules25122742.

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Abstract:

This work describes new methods for the chemical recycling of end-use poly(ethylene terephthalate) (PET) in batch, microwave and electrochemical reactors. The reactions are based on basic hydrolysis of the ester moieties in the polymer framework and occur under mild reaction conditions with low-cost reagents. We report end-use PET depolymerization in refluxing methanol with added NaOH with 75% yield of terephthalic acid in batch after 12 h, while yields up to 65% can be observed after only 40 min under microwave irradiation at 85 °C. Using basic conditions produced in the electrochemical reduction of protic solvents, electrolytic experiments have been shown to produce 17% terephthalic acid after 1 h of electrolysis at −2.2 V vs. Ag/AgCl in 50% water/methanol mixtures with NaCl as a supporting electrolyte. The latter method avoids the use of caustic solutions containing high-concentration NaOH at the outset, thus proving the concept for a novel, environmentally benign method for the electrochemical recycling of end-use PET based on low-cost solvents (water and methanol) and reagents (NaCl and electricity).

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