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Relevant bibliographies by topics / Iron oxides

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Academic literature on the topic 'Iron oxides'

Author: Grafiati

Published: 4 June 2021

Last updated: 1 August 2024

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Journal articles on the topic "Iron oxides"

1

Pfretzschner, Hans-Ulrich. "Iron oxides in fossil bone." Neues Jahrbuch für Geologie und Paläontologie - Abhandlungen 220, no. 3 (June 11, 2001): 417–29. http://dx.doi.org/10.1127/njgpa/220/2001/417.

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Kim, I. H., W. S. Kim, and D. S. Rhee. "Photocatalytic Activity of Fe/Ti Mixed Oxide for Degrading Humic Acid in Water." Advanced Materials Research 717 (July 2013): 95–100. http://dx.doi.org/10.4028/www.scientific.net/amr.717.95.

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The comparative experiments for removing humic acid as environmental pollutant were conducted by adsorption on iron oxide, photooxidation in the presence of titanium dioxide catalyst and combined adsorption-photooxidation by iron-titanium mixed metal oxides, where all these active components were immobilized on polypropylene granules. The main purpose of the work was the combination of adsorption and photocatalytic oxidation processes to remove humic acid. The granules with iron-titanium mixed oxide for treating humic acid gave much better results with 1.2~3 times higher removal rates comparing to the other two single coated oxides at certain pH values. And the order of removal efficiency according to pH was the same as for single iron oxide-coated granules. The ratio 1:2 of iron oxide/titanium dioxide was found optimal for maximal decolorization of humic acid solution. The total organic carbon decrease of humic acid in each experiments, when it was pre-equilibrated with mixed oxides-coated granules in the dark for 30 min and without pre-equilibration, was very similar. The results suggested that the mechanism of humic acid removal may be not only a respectively combined adsorption and photooxidation by iron oxide and titanium oxides, but an enhanced photooxidation reaction as a result of concentrating humic acid on titanium oxide surface by iron oxide.

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Jeong, D., K. Kim, and W. Choi. "Accelerated dissolution of iron oxides in ice." Atmospheric Chemistry and Physics Discussions 12, no. 8 (August 13, 2012): 20113–34. http://dx.doi.org/10.5194/acpd-12-20113-2012.

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Abstract. Iron dissolution from mineral dusts and soil particles is vital as a source of bioavailable iron in various environmental media. In this work, the dissolution of iron oxide particles trapped in ice was investigated as a~new pathway of iron supply. The dissolution experiments were carried out in the absence and presence of various organic complexing ligands under dark condition. In acidic pH conditions (pH 2, 3, and 4), the dissolution of iron oxides was greatly enhanced in the ice phase compared to that in water. The dissolved iron was mainly in the ferric form, which indicates that the dissolution is not a reductive process. The extent of dissolved iron was greatly affected by the kind of organic complexing ligands and the type of iron oxides. The iron dissolution was most pronounced with high surface area iron oxides and in the presence of strong iron binding ligands. The enhanced dissolution of iron oxides in ice is mainly ascribed to the "freeze concentration effect", which concentrates iron oxide particles, organic ligands, and protons in the liquid-like ice grain boundary region and accelerates the dissolution of iron oxides. The ice-enhanced dissolution effect gradually decreased when decreasing the freezing temperature from −10 °C to −196 °C, which implies that the presence and formation of the liquid-like ice grain boundary region play a critical role. The proposed phenomenon of enhanced dissolution of iron oxides in ice may provide a new pathway of bioavailable iron production. The frozen atmospheric ice with iron-containing dust particles in the upper atmosphere thaws upon descending and may provide bioavailable iron upon deposition onto the ocean surface.

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Jeong, D., K. Kim, and W. Choi. "Accelerated dissolution of iron oxides in ice." Atmospheric Chemistry and Physics 12, no. 22 (November 23, 2012): 11125–33. http://dx.doi.org/10.5194/acp-12-11125-2012.

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Abstract. Iron dissolution from mineral dusts and soil particles is vital as a source of bioavailable iron in various environmental media. In this work, the dissolution of iron oxide particles trapped in ice was investigated as a new pathway of iron supply. The dissolution experiments were carried out in the absence and presence of various organic complexing ligands under dark condition. In acidic pH conditions (pH 2, 3, and 4), the dissolution of iron oxides was greatly enhanced in the ice phase compared to that in water. The dissolved iron was mainly in the ferric form, which indicates that the dissolution is not a reductive process. The extent of dissolved iron was greatly affected by the kind of organic complexing ligands and the surface area of iron oxides. The iron dissolution was most pronounced with high surface area iron oxides and in the presence of strong iron binding ligands. The enhanced dissolution of iron oxides in ice is mainly ascribed to the "freeze concentration effect", which concentrates iron oxide particles, organic ligands, and protons in the liquid like ice grain boundary region and accelerates the dissolution of iron oxides. The ice-enhanced dissolution effect gradually decreased when decreasing the freezing temperature from −10 to −196 °C, which implies that the presence and formation of the liquid-like ice grain boundary region play a critical role. The proposed phenomenon of enhanced dissolution of iron oxides in ice may provide a new pathway of bioavailable iron production. The frozen atmospheric ice with iron-containing dust particles in the upper atmosphere thaws upon descending and may provide bioavailable iron upon deposition onto the ocean surface.

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5

BRUCHAJZER, ELŻBIETA, BARBARA FRYDRYCH, and JADWIGA SZYMAŃSKA. "Iron oxides – calculated on Fe Documentation of proposed values of occupational exposure limits (OELs)." Podstawy i Metody Oceny Środowiska Pracy 33, no. 2(92) (June 29, 2017): 51–87. http://dx.doi.org/10.5604/01.3001.0009.9360.

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Iron (III) oxide, (Fe2O3, nr CAS 1309-37-1) in natural conditions occurs as iron ore. The most common (hematite) contains about 70% pure iron. Iron (III) oxide is used as a red dye in ceramics, glass and paper industries and as a raw material for abrasive metalworking (cutting). Iron (II) oxide, (FeO, CAS 1345-25-1) occurs as a mineral wurtzite and is used as a black dye in cosmetics and as a component of tattoo ink. Iron (II) iron (III) oxide (Fe3O4, CAS 1309-38-2; 1317- -61-9) is a common mineral. It has strong magnetic properties (so called magnetite). It occurs in igneous rocks (gabbro, basalt). It is the richest and the best iron ore for industry. Occupational exposure to iron oxides occurs in the mining and metallurgical industry in the production of iron, steel and its products. Welders, locksmiths, lathes and workers employed in milling ores and polishing silver are exposed to iron oxides. According to data from the State Sanitary Inspection, in 2013, 389 people in Poland were exposed to iron oxide in concentrations exceeding the current NDS (5 mg/m3) and in 2014 – 172 people. After single and multiple intratracheal and inhalation exposure of animals, transient intensification of oxidative stress and inflammatory reactions were reported. Iron (III) oxide did not cause genotoxic and carcinogenic effects. In literature, there are no data on its effects on fertility, reproduction and pregnancy. Data on chronic toxicity of iron oxides for humans exposed in working environment are limited. In epidemiological studies, all information presented in the documentation comes from observations of people exposed to the combined effects of iron oxides and other factors. It is not stated whether occupational exposure was related to the specific iron oxide and to what concentrations workers were exposed. The most commonly encountered toxic effect in the occupational exposure of iron ore miners and iron welders and welders was minor lung fibrosis lesions and iron-silicon dust (as seen in the RTG study). Siderose is the occupational disease of miners and iron ore metallurgists. Moreover, cases of lung cancer have been reported in miners, steel workers and welders, but they were caused by total exposure to other compounds, including radioactive radon, carcinogenic chromium, manganese, nickel, other oxides (SiO2, ZnO, CO, NO, NO2, MgO) as well as exhaust gases from diesel engines. According to IARC, iron (III) oxide belongs to group 3 (cannot be classified as carcinogenic to humans). Iron (III) oxides can accumulate in a lung tissue, this process may be responsible for the occurrence of fibrosis sites, particularly in higher parts of external lung parts. These effects were visible in the X-ray examination only. Pneumoconiosis (siderosis) caused by exposure to iron oxides is usually asymptomatic (lack of clinical symptoms and changes in lung function parameters). The basis for the proposed MAC-TWA value for inhalable iron oxide fraction was NOAEL of 10 mg Fe/m3. People exposed for more than 10 years to iron (III) oxide had no pulmonary changes. After application of an uncertainty factor of 2 (for differences in personal sensitivity in humans), the MAC-TWA value for the iron oxide fraction was proposed at 5 mg/m3 (calculated as Fe). The same observations on humans were the basis for calculating the MAC-TWA value for respirable fraction of iron (III) oxide. On 12% of workers exposed to respirable fraction at mean concentrations of 10 ÷ 15 mg/m3, changes in pulmonary X-ray were observed. The value of 10 mg/m3 was assumed as LOAEL. After applying the appropriate uncertainty coefficients, the MAC-TWA value for the iron oxide respirable fraction was proposed at 2.5 mg/m3. The authors propose to leave the short-term value (STEL) of 10 mg/m3 for inhaled fraction for iron oxides and to introduce STEL value of 5 mg/m3 for respirable fraction. It is recommended to label the substances with "I" - irritant substance.

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Plemiannikov, Mykola, and Nataliіa Zhdanіuk. "Determination of the influence of temperature, concentration of ferric oxides and oxidative conditions of glass boiling on the displacement of the equilibrium of ferric oxides Fе2O3↔FеO." Technology audit and production reserves 3, no. 1(71) (June 29, 2023): 10–14. http://dx.doi.org/10.15587/2706-5448.2023.283267.

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The object of research is the state of equilibrium of ferrum(II) and ferrum(III) oxides in glass melts at temperatures of 1000–1400 °С, welded in oxidizing, neutral and reducing conditions with a content of ferrum oxides up to 1.5 %. This problem is relevant in the following aspects. The first aspect of this problem is the unwanted coloring of the glass: FeO colors the glass blue, and Fe2O3 – yellow. The combined presence of ferrum(II) oxide and ferrum(III) oxide determines the gradations of glass shades that fall on the green spectrum. The second aspect concerns the thermophysics of processes of boiling glasses containing iron oxides. Ferrum(II) oxide causes a strong absorption band of infrared radiation in the region of 1.1 μm. This becomes an obstacle to the volumetric heating of glass in the processes of cooking, forming, and annealing. The third aspect of the problem concerns the structure of glasses and glass-crystalline materials with an increased content of iron oxides. Iron oxides significantly affect the processes of glass structuring, as ferrum(III) oxide is a typical network former, and ferrum(II) oxide is a typical modifier. The state of FeO↔Fe2O3 equilibrium in glass is significantly influenced by the glass cooking environment, the total amount of iron oxides, and the temperature of the melt. The glass brewing environment has the greatest influence on the balance of iron oxides in the glass. The share of FeO oxide in the total amount of iron oxides (FeO+Fe2O3) increases sharply when moving from an oxidizing medium to a neutral one and then to a reducing one. During thermostating at a temperature of 1400 °С, the proportion of FeO in the glass increases by 1.4–1.7 times during cooking in an oxidizing environment, by 1.2–1.3 times in a neutral environment, and by approximately 1.1 times in a reducing environment. At the same time, this growth is more noticeable in glasses with a lower iron content. Thus, the equilibrium state of FeO↔Fe2O3 in glass significantly affects the technological and operational properties of silicate melts and the final glass. The ratio of formed oxides of trivalent and divalent ferrum was studied by chemical (titrometric) analysis. The research results can be used in practice to develop the composition of glasses with an increased content of iron oxides.

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Zhang, Lin, Di Lun Sheng, Rui Zhang, En Yi Chu, Ju Peng Liu, and Sheng Li Zhou. "Preparation of Self-Assembled Iron Oxide Nanorings with Nano-Aluminum." Applied Mechanics and Materials 446-447 (November 2013): 210–13. http://dx.doi.org/10.4028/www.scientific.net/amm.446-447.210.

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To make fuels and oxides react better, Iron oxide nanoring was synthesized using hydrothermal method and then self-assembled with nano aluminum particles. Iron oxide were characterized by hollow column morphology with outer diameters of 200-240nm, inner diameters of 90-120nm and heights of 120-150nm using SEM and TEM. Iron oxide and aluminum were evenly distributed and contact closely by self-assembly.The touch of fuels and oxides increased effectively.While the ultrasonically-mixed sample scattered randomly and aggregated seriously. Self-assembly is proved to be a effective method for the touch and distribution of oxides and fuels.

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Zhu, Yi. "The influence of iron oxides on wheel–rail contact: A literature review." Proceedings of the Institution of Mechanical Engineers, Part F: Journal of Rail and Rapid Transit 232, no. 3 (January 11, 2017): 734–43. http://dx.doi.org/10.1177/0954409716689187.

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In contrast to other third-body layers – such as water, oil, sand, and leaves – iron oxides exert a constant influence on the friction and wear of wheel–rail contact. However, studies that focus on the influence of iron oxides have not been conducted systematically until the 21st century. This study is a comprehensive presentation of early and recent research works related to the influence of iron oxides on the wheel–rail contact. The characteristics of iron oxides in general and those between railway wheels and rails are discussed. A comparison of various laboratory tests and their relation to actual conditions is also presented. The authors find that the influence of various types of iron oxides on friction and adhesion differs. The thickness of the iron oxide layer also affects the friction and wear. However, the results obtained from laboratory rigs differ from those obtained in field testing. Therefore, it is critical to formulate a standard procedure that produces iron oxides that are similar to those observed in the field. Compared to the case of wheel–rail friction and adhesion, the influence of iron oxides on wear is not so well investigated. Thus, further research in those areas is warranted.

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Al-Hamawandi, M. J., D. R. Azeez, and D. K. Ali. "Behavior and Distribution of Free Iron Oxides in Some Soil Orders in Iraq." IOP Conference Series: Earth and Environmental Science 1252, no. 1 (December 1, 2023): 012067. http://dx.doi.org/10.1088/1755-1315/1252/1/012067.

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Abstract This study was conducted to investigating the behavior of free iron oxides in some soil orders in Iraq. Soil samples were collected from five Pedons for soil orders Entisols, Aridisols, Inceptisols, Vertisols and Mollisols. Total free iron oxides (Fed) were extracted by CBD, amorphous iron oxides by acid ammonium oxalate and iron oxide linked with organic matter by alkaline Sodium pyrophosphate. the distribution of iron oxides in (Fep) to crystallized iron oxides were compared. The results showed that (Fed-Feo) there is no particular direction that controls the vertical distribution of Fed Mollisols and Vertisols pedons excelled in the content of Fed compared to the other orders. Amorphous Feo accumulates in surface horizons and Mollisols pedon was excelled on all pedons in Feo content followed by Vertisols, Inceptisols, Aridisols and Entisols. The Pedons of Inceptisols, Aridisols and Entisols soil order contain higher amounts of crystalline Fed-O oxides compared to the Mollisols and Vertisols as well the vertical distribution taken a different pattern for all pedons. (Fep) was low compared to other forms of iron oxides and is accumulated in surface soil horizon in all pedons.

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Moro, Koua, Aimé Serge Ello, Konan Roger Koffi, and N’goran Séverin Eroi. "Mixed Maghemite/Hematite Iron Oxide Nanoparticles Synthesis for Lead and Arsenic Removal from Aqueous Solution." Journal of Nanomaterials 2023 (April 26, 2023): 1–8. http://dx.doi.org/10.1155/2023/8216889.

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This work focused on the synthesis of iron oxide nanoparticles by the coprecipitation method with three basic solutions, namely, NH4OH, KOH, and NaOH. The synthesized iron oxides were characterized by various techniques such as XRD, MET, BET, and a SQUID magnetometer. The results showed nanosized particles of 13.2, 9.17, and 8.42 nm and different phases associated to maghemite and maghemite/hematite. The surface areas were 113, 94, and 84 m2/g and the magnetization strength were 58, 61, and 75 emu/g to iron oxides synthesized with NaOH, KOH, and NH4OH, respectively. The magnetic iron oxides obtained using NaOH were more efficient in the removal of lead and arsenic by adsorption than iron oxides obtained with KOH and NH4OH. However, the magnetic strength decreases using NaOH and KOH. The highest adsorption capacities attained for lead and arsenic removal were 16.6 and 14 mg/g, respectively, using NaOH-based iron oxides.

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Dissertations / Theses on the topic "Iron oxides"

1

Yang, Xiaofang. "Interactions between iron oxides and silicates /." Luleå : Division of Chemistry, Department of Chemical Engineering and Geosciences, Luleå University of Technology, 2008. http://epubl.ltu.se/1402-1757/2008/31/.

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Leake, Thomas Russell. "Zinc removal using biogenic iron oxides." Pullman, Wash. : Washington State University, 2009. http://www.dissertations.wsu.edu/Thesis/Fall2009/T_Leake_120409.pdf.

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Thesis (M.S. in enviromental engineering)--Washington State University, December 2009.
Title from PDF title page (viewed on Jan. 28, 2010). "Department of Civil and Environmental Engineering." Includes bibliographical references (p. 27-31).

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Majzlan, Juraj. "Thermodynamics of iron and aluminum oxides /." For electronic version search Digital dissertations database. Restricted to UC campuses. Access is free to UC campus dissertations, 2002. http://uclibs.org/PID/11984.

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Rennert, Thilo. "Sorption of iron cyanide complexes on iron oxides and in soils." [S.l.] : [s.n.], 2002. http://deposit.ddb.de/cgi-bin/dokserv?idn=964937069.

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Lee, Sung Oh School of Chemical Engineering &amp Industrial Chemistry UNSW. "Dissolution of iron oxides by oxalic acid." Awarded by:University of New South Wales. School of Chemical Engineering & Industrial Chemistry, 2005. http://handle.unsw.edu.au/1959.4/23924.

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The iron content of industrial minerals can be reduced by physical and chemical processing. Chemical processing is very efficient to achieve a high degree of iron removal at minimum operating cost. Both inorganic acids and organic acids have been used for clay refining. However, due to environmental pollution and contamination of products with the SO42- and Cl-, inorganic acids should be avoided as much as possible. This research investigated the use of oxalic acid to dissolve iron oxides and the dissolution characteristics of natural iron oxides. The dissolution of iron oxides in oxalic acid was found to be very slow at temperatures ranging from 25??? to 60???, but increased rapidly at a temperature above 90oC with increasing oxalic acid concentration, whereas the pH caused the reaction rate to decrease at pH>2.5 and improved the rate from pH 1 to pH 2.5. The iron oxides such as goethite (??-FeOOH), lepidocrocite (??-FeOOH) and iron hydroxide (Fe(OH)3) can be dissolved faster at the presence of magnetite which exhibits an induction period at the initial stage and showed the bell-shaped curves for the dissolution. In titration tests, however, the increase of temperature causes an increase in solubility of the oxalate complexes, resulting in an increased stability of ionized species in solution. During the addition of NaOH, NaHC2O4???H2O was precipitated without forming Na2C2O4???H2O, but it was re-dissolved at pH>4.0. On the other hand with NH4OH, NH4HC2O4???H2O and (NH4) 2C2O4???H2O co-precipitated at pH 0.93, but also re-dissolved at over pH 2.03. The reaction temperature was found not to affect the removal of iron from the ferric oxalate complex solution using lime. Iron is removed as iron hydroxide and calcium oxalate is then precipitated during the iron removal step. The formation of Fe(OH)3 in the solution was affected by the dissociation of Ca(OH)2. The thermodynamics of sodium, ammonium and iron oxalate complexes were investigated and the standard free energy, ??Go was calculated using thermodynamic data and solubility products. The dissolution of pure hematite by oxalate was found to follow a shrinking core model of which the kinetic step of the reaction is the controlled mechanism.

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Gonzalez, Lucena Fedora. "Mineral magnetism of synthetic microcrystalline and nanophase iron oxides and iron oxyhydroxides." Thesis, University of Ottawa (Canada), 2004. http://hdl.handle.net/10393/26646.

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A suite of well-characterized synthetic microcrystalline hematite samples, 2-line and 6-line ferrihydrite samples and nanohematite samples are studied through magnetization-field curves measured at room temperature. The single-domain microcrystalline hematite samples are analyzed through basic hysteresis parameters providing sample characteristics such as magnetic anisotropy information, the effect of annealing on the origin of the magnetization and the relatively constant intrinsic high field susceptibility. The application of a magnetic granulometry method on the magnetic data of the superparamagnetic nanohematite and ferrihydrite samples provides fundamental information such as the intrinsic mass magnetization and estimated particle size. Additionally, it gives insight into possible moment formation mechanisms within the superparamagnetic particles. The observed differences between the magnetic properties of the magnetically blocked and the superparamagnetic samples considered are also discussed.

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Bertel, Douglas E. "Characterizations of Iron Sulfides and Iron Oxides Associated with Acid Mine Drainage." University of Akron / OhioLINK, 2011. http://rave.ohiolink.edu/etdc/view?acc_num=akron1302276664.

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Ferraioli, C. Christopher. "Nanocrystals, core-shells, and nanocapsules of iron oxide." Click here for download, 2008. http://proquest.umi.com/pqdweb?did=1559855251&sid=1&Fmt=2&clientId=3260&RQT=309&VName=PQD.

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Mäkie, Peter. "Surface reactions of Organophosphorus compounds on Iron Oxides." Doctoral thesis, Umeå universitet, Kemiska institutionen, 2012. http://urn.kb.se/resolve?urn=urn:nbn:se:umu:diva-53958.

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Nadler, Jason Hayes. "The hydrogen reduction of iron and chromium oxides." Diss., Georgia Institute of Technology, 2003. http://hdl.handle.net/1853/19410.

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Books on the topic "Iron oxides"

1

Schwertmann, U., and R. M. Cornell, eds. Iron Oxides in the Laboratary. Weinheim, Germany: Wiley-VCH Verlag GmbH, 2000. http://dx.doi.org/10.1002/9783527613229.

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2

Smith, Mark Royston. Studies of iron catalysts and iron/zirconium oxides. Birmingham: University of Birmingham, 1986.

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Schwertmann, U. Iron oxides in the laboratory: Preparation and characterization. Weinheim: VCH, 1991.

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McGarvey, G. B. Interactions between iron oxides and copper oxides under hydrothermal conditions. Pinawa, Man: AECL, Whiteshell Laboratories, 1995.

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McGarvey, G. B. Interactions between iron oxides and copper oxides under hydrothermal conditions. Pinewa, Man: Research Chemistry Branch, Whiteshell Laboratories, 1995.

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Geological Survey (U.S.), ed. Sites in the Virginia-Washington, D.C.-Maryland metro area to observe or collect bacteria that precipitate iron and manganese oxides. [Reston, Va.?: U.S. Dept. of the Interior, U.S. Geological Survey, 1998.

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Geological Survey (U.S.), ed. Sites in the Virginia-Washington, D.C.-Maryland metro area to observe or collect bacteria that precipitate iron and manganese oxides. [Reston, Va.?: U.S. Dept. of the Interior, U.S. Geological Survey, 1998.

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Geological Survey (U.S.), ed. Sites in the Virginia-Washington, D.C.-Maryland metro area to observe or collect bacteria that precipitate iron and manganese oxides. [Reston, Va.?: U.S. Dept. of the Interior, U.S. Geological Survey, 1998.

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Geological Survey (U.S.), ed. Sites in the Virginia-Washington, D.C.-Maryland metro area to observe or collect bacteria that precipitate iron and manganese oxides. [Reston, Va.?: U.S. Dept. of the Interior, U.S. Geological Survey, 1998.

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Geological Survey (U.S.), ed. Sites in the Virginia-Washington, D.C.-Maryland metro area to observe or collect bacteria that precipitate iron and manganese oxides. [Reston, Va.?: U.S. Dept. of the Interior, U.S. Geological Survey, 1998.

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Book chapters on the topic "Iron oxides"

1

Rothwell, R. G. "Iron Oxides." In Minerals and Mineraloids in Marine Sediments, 139–43. Dordrecht: Springer Netherlands, 1989. http://dx.doi.org/10.1007/978-94-009-1133-8_14.

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Murad, Enver, and John Cashion. "Iron Oxides." In Mössbauer Spectroscopy of Environmental Materials and Their Industrial Utilization, 159–88. Boston, MA: Springer US, 2004. http://dx.doi.org/10.1007/978-1-4419-9040-2_5.

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Schwertmann, U., and R. M. Taylor. "Iron Oxides." In SSSA Book Series, 379–438. Madison, WI, USA: Soil Science Society of America, 2018. http://dx.doi.org/10.2136/sssabookser1.2ed.c8.

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Bigham, J. M., R. W. Fitzpatrick, and D. G. Schulze. "Iron Oxides." In Soil Mineralogy with Environmental Applications, 323–66. Madison, WI, USA: Soil Science Society of America, 2018. http://dx.doi.org/10.2136/sssabookser7.c10.

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Gooch, Jan W. "Iron Oxides." In Encyclopedic Dictionary of Polymers, 397. New York, NY: Springer New York, 2011. http://dx.doi.org/10.1007/978-1-4419-6247-8_6472.

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Chesworth, Ward, Augusto Perez‐Alberti, Emmanuelle Arnaud, H. J. Morel‐Seytoux, H. J. Morel‐Seytoux, and U. Schwertmann. "Iron oxides." In Encyclopedia of Soil Science, 363–69. Dordrecht: Springer Netherlands, 2008. http://dx.doi.org/10.1007/978-1-4020-3995-9_302.

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Bährle-Rapp, Marina. "Iron Oxides." In Springer Lexikon Kosmetik und Körperpflege, 284. Berlin, Heidelberg: Springer Berlin Heidelberg, 2007. http://dx.doi.org/10.1007/978-3-540-71095-0_5281.

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Gooch, Jan W. "Natural Iron Oxides." In Encyclopedic Dictionary of Polymers, 479. New York, NY: Springer New York, 2011. http://dx.doi.org/10.1007/978-1-4419-6247-8_7795.

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Gooch, Jan W. "Iron Oxides, Synthetic." In Encyclopedic Dictionary of Polymers, 397–98. New York, NY: Springer New York, 2011. http://dx.doi.org/10.1007/978-1-4419-6247-8_6473.

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Wickham, D. G., Joel Mark, and Kerro Knox. "Metal Iron(III) Oxides." In Inorganic Syntheses, 152–56. Hoboken, NJ, USA: John Wiley & Sons, Inc., 2007. http://dx.doi.org/10.1002/9780470132401.ch41.

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Conference papers on the topic "Iron oxides"

1

Yamaguchi, K., T. Fujii, S. Kuranouchi, Y. Yamanobe, and A. Ueno. "Magnetic properties of iron-boron-oxides and iron-phospher-oxides glasses prepared by sol-gel method." In International Magnetics Conference. IEEE, 1989. http://dx.doi.org/10.1109/intmag.1989.689957.

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Merca, Senfred Matthew O., Julius Caezar II M. Damo, Hannah Kristel D. Vargas, Ramel John Anthony V. Biñas, Catherine Angeli R. San Jose, Sean Benson A. See, Yasmin D. G. Edañol, Ken Aldren Usman, and Marlon T. Conato. "Tuned Photodegradation Efficiency of Bimetallic Copper-Iron Oxide Catalysts via Precursor Stoichiometry Control for Water Decontamination." In International Conference on Advanced Materials, Mechanics and Structural Engineering. Switzerland: Trans Tech Publications Ltd, 2024. http://dx.doi.org/10.4028/p-umwd6s.

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Inadequate handling and disposal of contaminated industrial waste significantly contribute to environmental pollution. The presence of pollutants, including dyes, in wastewater necessitates the development of innovative remediation techniques. Metal oxide-catalyzed photodegradation capitalizes on the capacity of a dye to absorb light energy, offering a rapid method to break down the dye into less harmful, colorless byproducts. In this work, bimetallic copper-iron oxides with various copper to iron were synthesized for the photodegradation of fuchsine. The photocatalysts were prepared through oxalate precipitation followed by thermal decomposition. Structural analysis revealed a MOF-like structure of the bimetallic oxalate precursors. Thermal decomposition of the oxalates yielded photocatalytic bimetallic copper-iron oxides. Photodegradation studies demonstrated that the addition of copper-iron oxides accelerated the degradation of fuchsine and a higher concentration of CuO enhances the performance of the photocatalyst. Notably, the copper-iron oxide with a 1:1 (CuFe) ratio proved to be the most effective catalyst for the photodegradation of fuchsine. Furthermore, the photodegradation of fuchsine conforms to a pseudo-first order model and exhibits characteristics of a first-order reaction. Our findings emphasize that simple and high-efficiency bimetallic oxide catalysts can be used for water decontamination applications.

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Kenney, Janice, Jonathan Ritson, and Hannah Rigby. "Overmedicated Minerals: Pharmaceutical Sorption to Iron Oxides." In Goldschmidt2020. Geochemical Society, 2020. http://dx.doi.org/10.46427/gold2020.1280.

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Choi, Wonyong, Kitae Kim, and Sunil Paul M. Menacherry. "Dissolution of Iron Oxides in the Frozen Solution." In Goldschmidt2020. Geochemical Society, 2020. http://dx.doi.org/10.46427/gold2020.432.

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Rentz, Jeremy A., and Jeffrey L. Ullman. "Copper and Zinc Removal Using Biogenic Iron Oxides." In World Environmental And Water Resources Congress 2012. Reston, VA: American Society of Civil Engineers, 2012. http://dx.doi.org/10.1061/9780784412312.072.

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Lim, B. L., L. R. Stace, and G. Zhang. "Index Properties of Soils Rich in Iron Oxides." In GeoShanghai International Conference 2006. Reston, VA: American Society of Civil Engineers, 2006. http://dx.doi.org/10.1061/40860(192)31.

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Hayes, Scott, Heather Hamlett, and Roberta Bustin. "Carbon Reduction of Iron Oxides in Lunar Simulants." In Fifth International Conference on Space. Reston, VA: American Society of Civil Engineers, 1996. http://dx.doi.org/10.1061/40177(207)100.

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Brooks, G., M. Pownceby, M. Rhamdhani, and T. Triana. "Ammonia Direct Reduction of Iron Oxides — Preliminary Assessment." In AISTech 2024. AIST, 2024. http://dx.doi.org/10.33313/388/035.

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9

Panichkin, A. V., and B. B. Kshibekova. "Assessment of the flux composition effect on the removal efficiency of non-metallic inclusions in high-chromium cast iron." In Challenges of Science. Institute of Metallurgy and Ore Beneficiation, 2023. http://dx.doi.org/10.31643/2023.36.

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The problem to refine high-chromium cast iron melts obtained with the use of a large proportion of scraped metal and scrap is considered herein. Since fluxes containing calcium fluoride are currently considered to be environmentally polluting, it is required to reduce the use of fluorides, or completely replace them. It was shown that a decrease in the melting point of the flux can be achieved with the use of a mixture of calcium and magnesium fluorides or by the introduction of boron oxide into the composition of the fluxes. However, the efficiency of these fluxes, as well as silicocalcium additives and vacuum remelting in the high-chromium cast iron melting when a high proportion of scrap in the charge is used, has not been previously considered. In this regard, the effect of these refining methods on the removal of non-metallic inclusions in high-chromium cast iron of Grade 340Х18HML was experimentally assessed. Thermodynamic calculations were performed for the interaction of magnesium and calcium fluorides with non-metallic oxide inclusions typical of high-chromium cast irons and with oxides used for neutral lining of induction furnaces. It has been shown that fluxes based on boron oxide, magnesium and calcium fluorides and their mixtures effectively remove oxide and sulfide non-metallic inclusions; however, they have a destructive effect on the lining of furnaces, significantly reducing its service life. The addition of silicocalcium reduces the content of sulfides but does not affect the content of non-metallic inclusions in the form of oxides and nitrides. Vacuum remelting effectively reduces the number of nitride inclusions.

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Paul, Cynthia J., and Robert G. Ford. "Sequential Extractions for Partitioning of Arsenic on Hydrous Iron Oxides and Iron Sulfides." In World Water and Environmental Resources Congress 2001. Reston, VA: American Society of Civil Engineers, 2001. http://dx.doi.org/10.1061/40569(2001)480.

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Reports on the topic "Iron oxides"

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Beaudoin, G. Iron oxides: indicator minerals for exploration. Natural Resources Canada/ESS/Scientific and Technical Publishing Services, 2017. http://dx.doi.org/10.4095/300294.

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Beaudoin, G. Iron oxides: indicator minerals for exploration. Natural Resources Canada/ESS/Scientific and Technical Publishing Services, 2013. http://dx.doi.org/10.4095/292690.

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Bongiovanni, R., E. Pelizzetti, E. Borgarello, and D. Meisel. On the formation of iron(III) oxides via oxidation of iron(II). Office of Scientific and Technical Information (OSTI), September 1994. http://dx.doi.org/10.2172/10179902.

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Menting, Victor. Solubility Studies of Iron(III) Oxides and Hydroxides. Portland State University Library, January 2000. http://dx.doi.org/10.15760/etd.6729.

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Burgos, W. D. Impact of Iron-Reducing Bacteria on Metals and Radionuclides Adsorbed to Humic-Coated Iron(III) Oxides. Office of Scientific and Technical Information (OSTI), February 2005. http://dx.doi.org/10.2172/876706.

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Fendorf, Scott. Subsurface Conditions Controlling Uranium Incorporation in Iron Oxides: A Redox Stable Sink. Office of Scientific and Technical Information (OSTI), April 2016. http://dx.doi.org/10.2172/1245538.

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Akyurtlu, A. Hot gas desulfurization with sorbents containing oxides of zinc, iron, vanadium and copper. Office of Scientific and Technical Information (OSTI), October 1991. http://dx.doi.org/10.2172/6041806.

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Akyurtlu, A., and J. F. Akyurtlu. Hot gas desulfurization with sorbents containing oxides of zinc, iron, vanadium and copper. Office of Scientific and Technical Information (OSTI), January 1992. http://dx.doi.org/10.2172/7008198.

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Chambers, S. A., and Jr G. E. Brown. Molecular-Level Processes Governing the Interaction of Contaminants with Iron and Manganese Oxides. Office of Scientific and Technical Information (OSTI), June 1999. http://dx.doi.org/10.2172/825969.

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Chambers, S. A., and Jr G. E. Brown. Molecular-Level Processes Governing the Interaction of Contaminants with Iron and Manganese Oxides. Office of Scientific and Technical Information (OSTI), June 2000. http://dx.doi.org/10.2172/825970.

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