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Journal articles on the topic 'CuFeS2'

Author: Grafiati

Published: 6 September 2023

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1

Auernik, Kathryne S., and Robert M. Kelly. "Impact of Molecular Hydrogen on Chalcopyrite Bioleaching by the Extremely Thermoacidophilic Archaeon Metallosphaera sedula." Applied and Environmental Microbiology 76, no. 8 (February 26, 2010): 2668–72. http://dx.doi.org/10.1128/aem.02016-09.

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ABSTRACT Hydrogen served as a competitive inorganic energy source, impacting the CuFeS 2 bioleaching efficiency of the extremely thermoacidophilic archaeon Metallosphaera sedula. Open reading frames encoding key terminal oxidase and electron transport chain components were triggered by CuFeS2. Evidence of heterotrophic metabolism was noted after extended periods of bioleaching, presumably related to cell lysis.

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2

Chang, Shun-An, Po-Yu Wen, Tsunghsueh Wu, and Yang-Wei Lin. "Microwave-Assisted Synthesis of Chalcopyrite/Silver Phosphate Composites with Enhanced Degradation of Rhodamine B under Photo-Fenton Process." Nanomaterials 10, no. 11 (November 20, 2020): 2300. http://dx.doi.org/10.3390/nano10112300.

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A new composite by coupling chalcopyrite (CuFeS2) with silver phosphate (Ag3PO4) (CuFeS2/Ag3PO4) was proposed by using a cyclic microwave heating method. The prepared composites were characterized by scanning and transmission electron microscopy and X-ray diffraction, Fourier-transform infrared, UV–Vis diffuse reflectance spectroscopy, and X-ray photoelectron spectroscopy. Under optimum conditions and 2.5 W irradiation (wavelength length > 420 nm, power density = 0.38 Wcm−2), 96% of rhodamine B (RhB) was degraded by CuFeS2/Ag3PO4 within a 1 min photo-Fenton reaction, better than the performance of Ag3PO4 (25% degradation within 10 min), CuFeS2 (87.7% degradation within 1 min), and mechanically mixed CuFeS2/Ag3PO4 catalyst. RhB degradation mainly depended on the amount of hydroxyl radicals generated from the Fenton reaction. The degradation mechanism of CuFeS2/Ag3PO4 from the photo-Fenton reaction was deduced using a free radical trapping experiment, the chemical reaction of coumarin, and photocurrent and luminescence response. The incorporation of CuFeS2 in Ag3PO4 enhanced the charge separation of Ag3PO4 and reduced Ag3PO4 photocorrosion as the photogenerated electrons on Ag3PO4 were transferred to regenerate Cu2+/Fe3+ ions produced from the Fenton reaction to Cu+/Fe2+ ions, thus simultaneously maintaining the CuFeS2 intact. This demonstrates the synergistic effect on material stability. However, hydroxyl radicals were produced by both the photogenerated holes of Ag3PO4 and the Fenton reaction of CuFeS2 as another synergistic effect in catalysis. Notably, the degradation performance and the reusability of CuFeS2/Ag3PO4 were promoted. The practical applications of this new material were demonstrated from the effective performance of CuFeS2/Ag3PO4 composites in degrading various dyestuffs (90–98.9% degradation within 10 min) and dyes in environmental water samples (tap water, river water, pond water, seawater, treated wastewater) through enhanced the Fenton reaction under sunlight irradiation.

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3

Wen, Po-Yu, Ting-Yu Lai, Tsunghsueh Wu, and Yang-Wei Lin. "Hydrothermal and Co-Precipitated Synthesis of Chalcopyrite for Fenton-like Degradation toward Rhodamine B." Catalysts 12, no. 2 (January 26, 2022): 152. http://dx.doi.org/10.3390/catal12020152.

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In this study, Chalcopyrite (CuFeS2) was prepared by a hydrothermal and co-precipitation method, being represented as H-CuFeS2 and C-CuFeS2, respectively. The prepared CuFeS2 samples were characterized by scanning electron microscope (SEM), transmission electron microscope (TEM), energy dispersive X-ray spectroscopy mapping (EDS-mapping), powder X-ray diffractometer (XRD), X-ray photoelectron spectrometry (XPS), and Raman microscope. Rhodamine B (RhB, 20 ppm) was used as the target pollutant to evaluate the degradation performance by the prepared CuFeS2 samples. The H-CuFeS2 samples (20 mg) in the presence of Na2S2O8 (4 mM) exhibited excellent degradation efficiency (98.8% within 10 min). Through free radical trapping experiment, the major active species were •SO4− radicals and •OH radicals involved the RhB degradation. Furthermore, •SO4− radicals produced from the prepared samples were evaluated by iodometric titration. In addition, one possible degradation mechanism was proposed. Finally, the prepared H-CuFeS2 samples were used to degrade different dyestuff (rhodamine 6G, methylene blue, and methyl orange) and organic pollutant (bisphenol A) in the different environmental water samples (pond water and seawater) with 10.1% mineral efficiency improvement comparing to traditional Fenton reaction.

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4

Yu, Huajian, Jianhua Xu, Yanyan Hu, Huadi Zhang, Cong Zhang, Chengcheng Qiu, Xuping Wang, Bing Liu, Lei Wei, and Jing Li. "Synthesis and characterization of CuFeS2 and Se doped CuFeS2−xSex nanoparticles." Journal of Materials Science: Materials in Electronics 30, no. 13 (May 27, 2019): 12269–74. http://dx.doi.org/10.1007/s10854-019-01586-5.

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5

Hu, Junqing, Qingyi Lu, Kaibin Tang, Yitai Qian, Guien Zhou, and Xianming Liu. "A solvothermal reaction route for the synthesis of CuFeS2 ultrafine powder." Journal of Materials Research 14, no. 10 (October 1999): 3870–72. http://dx.doi.org/10.1557/jmr.1999.0523.

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A 100-nm CuFeS2 ultrafine powder was prepared through a solvothermal reaction at 200–250 °C. X-ray powder diffraction and transmission electron microscopy results revealed that chalcopyrite-phase CuFeS2 was crystallized with single-crystalline nature and preferential orientation growth. Mössbauer spectrum exhibited a six-peak hyperfine magnetic spectrum and a single nonmagnetic peak. Elemental analysis gave the atomic ratio of Cu:Fe:S of 1:1.02:2.10. The influence factors on the formation of CuFeS2 ultrafine powder are discussed.

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6

Mikhailovskii, A. P., A. M. Polubotko, V. D. Prochukhan, and Yu V. Rud. "Gapless State in CuFeS2." physica status solidi (b) 158, no. 1 (March 1, 1990): 229–38. http://dx.doi.org/10.1002/pssb.2221580122.

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7

Liu, Zezhong, Zengxu Liu, Zhen Zhao, Danxia Li, Pengfei Zhang, Yanfang Zhang, Xiangyong Liu, Xiaoteng Ding, and Yuanhong Xu. "Photothermal Regulated Nanozyme of CuFeS2 Nanoparticles for Efficiently Promoting Wound Healing Infected by Multidrug Resistant Bacteria." Nanomaterials 12, no. 14 (July 19, 2022): 2469. http://dx.doi.org/10.3390/nano12142469.

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Peroxidase-mediated chemokinetic therapy (CDT) can effectively resist bacteria; however, factors such as the high dosage of drugs seriously limit the antibacterial effect. Herein, CuFeS2 nanoparticles (NPs) nanozyme antibacterial system with the photothermal effect and peroxidase-like catalytic activity are proposed as a combined antibacterial agent with biosafety, high-efficiency, and broad-spectrum antibacterial ability. In addition, the as-obtained CuFeS2 NPs with a low doses of Cu+ and Fe3+ can change the permeability of bacterial cell membranes and break the antioxidant balance by consuming intracellular glutathione (GSH), which results in more conducive ROS production. Meanwhile, the photothermal heating can regulate the CuFeS2 NPs close to their optimal reaction temperature (60 °C) to release more hydroxyl radical in low concentrations of H2O2 (100 µM). The proposed CuFeS2 NPs-based antibacterial system achieve more than 99% inactivation efficiency of methicillin-resistant Staphylococcus aureus (106 CFU mL−1 MRSA), hyperspectral bacteria β-Escherichia coli (106 CFU mL−1 ESBL) and Pseudomonas aeruginosa (106 CFU mL−1 PA), even at low concentration (2 μg mL−1), which is superior to those of the conventional CuO NPs at 4 mg mL−1 reported in the literature. In vivo experiments further confirm that CuFeS2 NPs can effectively treat wounds infected by MRSA and promote the wound healing. This study demonstrates that excellent antibacterial ability and good biocompatibility make CuFeS2 NPs a potential anti-infection nanozyme with broad application prospects.

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8

Korzun, Barys, and Anatoly Pushkarev. "XRPD and Scanning Electron Microscopy of Alloys of the CuAlS2 – CuFeS2 System Prepared by Thermobaric Treatment." MRS Advances 3, no. 56 (2018): 3323–28. http://dx.doi.org/10.1557/adv.2018.558.

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ABSTRACTAlloys of the CuAlS2 – CuFeS2 system were prepared by thermobaric treatment at high pressure of 5.5 GPa and temperatures ranging from 573 to 1573 K and phase formation in the system was investigated using X-ray powder diffraction, optical microscopy and scanning electron microscopy equipped with energy dispersive spectroscopy. The unit-cell parameters (the lattice constants and the unit-cell volume) were computed as a function of the composition. Absence of complete solubility in the (CuAlS2)1-x-(CuFeS2)x system was established. Formation of solid solutions with the tetragonal structure of chalcopyrite was detected for compositions with the molar part of CuFeS2 x not exceeding 0.10.

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9

Sugathan, Anumol, Biswajit Bhattacharyya, V. V. R. Kishore, Abhinav Kumar, Guru Pratheep Rajasekar, D. D. Sarma, and Anshu Pandey. "Why Does CuFeS2 Resemble Gold?" Journal of Physical Chemistry Letters 9, no. 4 (January 30, 2018): 696–701. http://dx.doi.org/10.1021/acs.jpclett.7b03190.

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10

Korzun, B. V., A. A. Fadzeyeva, G. Kloess, and K. Bente. "Microstructure of CuFeS2-δ-CuInS2alloys." physica status solidi (c) 6, no. 5 (May 2009): 1055–58. http://dx.doi.org/10.1002/pssc.200881160.

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11

Dickens, Christopher, Adam O. J. Kinsella, Matt Watkins, and Matthew Booth. "The Presence of Charge Transfer Defect Complexes in Intermediate Band CuAl1-pFepS2." Crystals 12, no. 12 (December 14, 2022): 1823. http://dx.doi.org/10.3390/cryst12121823.

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Despite chalcopyrite (CuFeS2) being one of the oldest known copper ores, it exhibits various properties that are still the subject of debate. For example, the relative concentrations of the ionic states of Fe and Cu in CuFeS2 can vary significantly between different studies. The presence of a plasmon-like resonance in the visible absorption spectrum of CuFeS2 nanocrystals has driven a renewed interest in this material over recent years. The successful synthesis of CuAl1−pFepS2 nanocrystals that exhibit a similar optical resonance has recently been demonstrated in the literature. In this study, we use density functional theory to investigate Fe substitution in CuAlS2 and find that the formation energy of neutral [FeCu]2++[CuAl]2− defect complexes is comparable to [FeAl]0 antisites when p≥0.5. Analysis of electron density and density of states reveals that charge transfer within these defect complexes leads to the formation of local Cu2+/Fe2+ ionic states that have previously been associated with the optical resonance in the visible absorption of CuFeS2. Finally, we comment on the nature of the optical resonance in CuAl1−pFepS2 in light of our results and discuss the potential for tuning the optical properties of similar systems.

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12

Dizer, Oleg, Kirill Karimov, Aleksei Kritskii, and Denis Rogozhnikov. "Synthetic Sulfide Concentrate Dissolution Kinetics in HNO3 Media." Materials 15, no. 22 (November 17, 2022): 8149. http://dx.doi.org/10.3390/ma15228149.

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The nature of tennantite (Cu12As4S13), chalcopyrite (CuFeS2) and sphalerite (ZnS) particles’ mixture dissolution in nitric acid (HNO3) media was investigated in this study. The effects of temperature (323–368 K), HNO3 (1–8 mol/L) and Fe3+ (0.009–0.036 mol/L) concentrations, reaction time (0–60 min) and pyrite (FeS2) additive (0.5/1–2/1; FeS2/sulf.conc.) on the conversion of the minerals were evaluated. It has been experimentally shown that the dissolution of the mixture under optimal conditions (>353 K; 6 mol/L HNO3; FeS2/synt. conc = 1/1) allows Cu12As4S13, CuFeS2 and ZnS conversion to exceed 90%. The shrinking core model (SCM) was applied for describing the kinetics of the conversion processes. The values of Ea were calculated as 28.8, 33.7 and 53.7 kJ/mol, respectively, for Cu12As4S13, CuFeS2 and ZnS. Orders of the reactions with respect to each reactant were calculated and the kinetic equations were derived to describe the dissolution rate of the minerals. It was found that the interaction between HNO3 solution and Cu12As4S13, CuFeS2 and ZnS under the conditions investigated in this are of a diffusion-controlled nature. Additionally, the roles of Fe(III) in the initial solution and FeS2 in the initial pulp as catalysts were studied. The results indicated that the increase in Fe3+ concentration significantly accelerates the dissolution of the mixture, while the addition of FeS2 forms a galvanic coupling between FeS2, and Cu12As4S13 and CuFeS2, which also accelerates the reaction rate. The results of the study are considered useful in developing a hydrometallurgical process for polymetallic sulfide raw materials treatment.

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13

Usman, Dudi Nasrudin, Sri Widayati, Sriyanti Sriyanti, and Era Setiawan. "Rock Formation Acid Mine Drainage in Epithermal Gold Mineralization, Pandeglang, Banten Province." Journal of Geoscience, Engineering, Environment, and Technology 4, no. 4 (December 30, 2019): 271–76. http://dx.doi.org/10.25299/jgeet.2019.4.4.3903.

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Mine acid water is acidic water and contains iron and sulfate, which is formed under natural conditions when geological strata containing pyrites are exposed to an oxidizing atmosphere or environment. One of the impacts of the mineralization zone where there is a mining process is the potential for the formation of acid mine drainage, especially in the Cibaliung gold mineralization area and its surroundings, Pandeglang Regency, Banten Province. Acid-forming sulfide minerals include pyrite (FeS2), headquarters (FeS2), picoliters (FexSx), calcocytes (CuS), covellite (CuS), chalcopyrite (CuFeS2), molybdenite (MoS), mulenite (NiS), chalocytes (CuS), covellite (CuS), chalcopyrite (CuFeS2), molybdenite (MoS), mulenite (NiS), chalocytes (CuS), covellite (CuS), chalcopyrite (CuFeS2), molybdenite (MoS), mulenite (NiS), galena (PbS) ) and sphalerite (ZnS). Of all these minerals, pyrite is the most dominant sulfide in acid formation. Alkaline mine water (alkaline mine drainage) is mine water that has an acidity level (pH) of 6 or more, containing alkalinity but still containing dissolved metals that can produce acids. The quality of mine water, acid or alkali, depends on the presence or absence of acid mineral content (sulfides) and alkaline materials in the geological strata. Acid water formation tends to be more intensive in mining areas. This can be prevented by avoiding exposure to sulfide-containing materials in the free air. Acid-forming sulfide minerals include pyrite (FeS2), headquarters (FeS2), picoliters (FexSx), calcocytes (CuS), covellite (CuS), chalcopyrite (CuFeS2), molybdenite (MoS), mulenite (NiS), chalocytes (CuS), covellite (CuS), chalcopyrite (CuFeS2), molybdenite (MoS), mulenite (NiS), chalocytes (CuS), covellite (CuS), chalcopyrite (CuFeS2), molybdenite (MoS), mulenite (NiS), galena (PbS) ) and sphalerite (ZnS). Of all these minerals, pyrite is the most dominant sulfide in acid formation. Formation of potential acidic water also occurs in tailings which are residues/processing residues containing sulfide minerals. The formation of acid mine drainage does not always develop in every sulfide-ore mining. In certain types of ore deposits, there are neutralizing agents which prevent the formation of acid mine drainage.

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14

Bhattacharyya, Biswajit, and Anshu Pandey. "CuFeS2 Quantum Dots and Highly Luminescent CuFeS2 Based Core/Shell Structures: Synthesis, Tunability, and Photophysics." Journal of the American Chemical Society 138, no. 32 (August 4, 2016): 10207–13. http://dx.doi.org/10.1021/jacs.6b04981.

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15

Boon, J. W. "The crystal structure of chalcopyrite (CuFeS2) and AgFeS2: The permutoidic reactions KFeS2 → CuFeS2 and KFeS2 → AgFeS2." Recueil des Travaux Chimiques des Pays-Bas 63, no. 4 (September 3, 2010): 69–80. http://dx.doi.org/10.1002/recl.19440630402.

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16

Vardner, Jonathon, Elifsu Gencer, Raymond Farinato, Devarayasamudram Nagaraj, Scott Banta, and Alan West. "(Digital Presentation) Electron Mediators for the Reductive Leaching of Chalcopyrite: Replacing Smelting with Electrolysis for Copper Production." ECS Meeting Abstracts MA2022-01, no. 56 (July 7, 2022): 2359. http://dx.doi.org/10.1149/ma2022-01562359mtgabs.

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Copper is expected to be in high demand in the coming decades due to the emergence of wind and solar technologies, which require about five times as much copper as traditional energy sources. Copper, however, is expected to be in short supply in the coming decades due to the high costs associated with the mining, concentrating, and processing of chalcopyrite (CuFeS2), which accounts for about 70% of all copper reserves. This work introduces a potentially transformative hydrometallurgical process for domestic production of copper from CuFeS2. Commercialization of such a process could sustain a high rate of copper production throughout the 21st century. Chalcopyrite is reacted with a redox couple to enable the rapid, clean, and complete recovery of copper. The reductant may be regenerated by an electrolysis unit. Reactions 1 and 2 show the direct electrochemical reduction of CuFeS2 to Cu2S and Cu0, respectively 2 CuFeS2 + 6H+ + 2e- → Cu2S + 2 Fe2+ + 3 H2 S [1] Cu2S + 2H+ + 2e- → 2 Cu0 + H2 S [2] The cathodic reduction of CuFeS2 competes with the hydrogen evolution reaction and therefore becomes inefficient at current densities exceeding 40 mA/cm2. Conversely, the cathodic reduction of an electron mediator circumvents the hydrogen evolution reaction and enables current densities exceeding 100 mA/cm2. Figure 1 shows a result that highlights the use of an electron mediator to facilitate the rapid and complete reduction of chalcopyrite, followed by the dissolution of the resultant solid product into sulfuric acid for the complete recovery of copper. In figure 1a, the release of Fe2+ ions to solution during the progression of the reaction with electron mediator is shown. In all cases, the solution contains 4M H2SO4 and various loadings of CuFeS2 concentrate. Error bars show standard deviations of replicates in triplicate. The reaction nearly goes to completion in 10 minutes. In figure 1b, the subsequent extraction of Cu2+ from mineral products dissolution into 1M H2SO4. The resulting concentration of copper in the sulfuric acid is amenable to electrowinning. Results are shown for high loadings of chalcopyrite, within a practical range for economic viability. In this work, we report successful results from two redox couples that can be effectively regenerated via electrolysis. A preliminary technoeconomic analysis is discussed, identifying potential opportunities as well as technical challenges. Figure 1

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17

Cheng, Zhiqiang, Xiaoyou Niu, Shenlong Jiang, and Qun Zhang. "State-selective exciton–plasmon interplay in a hybrid WSe₂/CuFeS₂ nanosystem." Journal of Chemical Physics 156, no. 14 (April 14, 2022): 144701. http://dx.doi.org/10.1063/5.0090467.

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The integration of confined exciton and localized surface plasmon in a hybrid nanostructure has recently stimulated extensive interests. The mechanistic insights into the elusive exciton–plasmon interplay at the nanoscale are of both fundamental and applicable values. Herein, by taking a hybrid WSe2/CuFeS2 system as a prototype, in which the excitonic semiconductor WSe2 nanosheets are interfaced with the plasmonic semiconductor CuFeS2 nanocrystals to form a heterostructure, we design and perform an ultrafast dynamics study to glean information in this regard. Specifically, the band-alignment relationship between the two components enables the contrasting case studies in which the excitonic excited states of WSe2 are pre-selected to be on-/off-resonant with the plasmon band of CuFeS2. As revealed by the joint observations from steady-state absorption and photoexcitation-dependent/temperature-dependent femtosecond time-resolved transient absorption (fs-TA) spectroscopy, an effective energy transfer process occurs in this exciton–plasmon system where the energy donor (acceptor) is the excitonic WSe2 (plasmonic CuFeS2) and its efficiency is modulated by the exciton–plasmon coupling strength. Furthermore, as inferred from the temperature-dependent fs-TA analysis, the opening of such an energy-transfer channel turns out to take place during the early phase of plasmon decay (∼1 ps). In addition, the activation energy of energy transfer for a specific exciton-state-selected case is estimated (∼200 meV). This work provides a dynamics perspective to the plasmon semiconductor-involved exciton–plasmon interplay that features excited-state selectivity of exciton band and, hence, would be of guiding value for rational design and optimization of relevant applications based on exciton–plasmon manipulation.

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18

Nyembwe, Kolela J., Elvis Fosso-Kankeu, Frans Waanders, and Martin Mkandawire. "Iron-Speciation Control of Chalcopyrite Dissolution from a Carbonatite Derived Concentrate with Acidic Ferric Sulphate Media." Minerals 11, no. 9 (September 3, 2021): 963. http://dx.doi.org/10.3390/min11090963.

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The mechanisms involved in the dissolution of chalcopyrite from a carbonatite concentrate in a ferric sulphate solution at pH 1.0, 1.5 and 1.8, and temperatures 25 °C and 50 °C were investigated. Contrary to expectations and thermodynamic predictions according to which low pH would favour high Cu dissolution, the opposite was observed. The dissolution was also highly correlated to the temperature. CuFeS2 phase dissolution produced intermediate Cu rich phases: CuS, Cu2S and Cu5FeS4, which appeared to envelop CuFeS2. Thermodynamic prediction revealed CuS to be refractory and could hinder dissolution. CuFeS2 phase solid-state dissolution process was further discussed. Free Fe3+ and its complexes (Fe(HSO4)2+, Fe(SO4)2– and FeSO4+ were responsible for Cu dissolution, which increased with increasing pH and temperature. The dissolution improved at pH 1.8 rather than 1.0 due to the increase of (Fe(HSO4)2+, Fe(SO4)2– and FeSO4+, which were also the predominating species at a higher temperature. The fast and linear first dissolution stage was attributed to the combined effect of Fe3+ and its complex (Fe(HSO4)2+, while Fe(SO4)2– was the main species for the second Cu dissolution stage characterised by a slow rate.

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19

Д, Сангаа, Даваа С, Зузаан П, Отгоолой Б, Дэлгэрбат Л, Жаргалжав Г, Ням-Очир Л, and Отгонбаяр Д. "Зэсийн хүдрийн рентгенографын тоон анализ." Физик сэтгүүл 10, no. 179 (March 14, 2022): 225–33. http://dx.doi.org/10.22353/physics.v10i179.748.

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20

Conejeros, Sergio, Pere Alemany, Miquel Llunell, Ibério de P. R. Moreira, Vı́ctor Sánchez, and Jaime Llanos. "Electronic Structure and Magnetic Properties of CuFeS2." Inorganic Chemistry 54, no. 10 (May 5, 2015): 4840–49. http://dx.doi.org/10.1021/acs.inorgchem.5b00399.

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21

Jing, Mingxing, Jing Li, and Kegao Liu. "Research progress in photolectric materials of CuFeS2." IOP Conference Series: Earth and Environmental Science 128 (March 2018): 012087. http://dx.doi.org/10.1088/1755-1315/128/1/012087.

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22

Boekema, C., A. M. Krupski, M. Varasteh, K. Parvin, F. van Til, F. van der Woude, and G. A. Sawatzky. "Cu and Fe valence states in CuFeS2." Journal of Magnetism and Magnetic Materials 272-276 (May 2004): 559–61. http://dx.doi.org/10.1016/j.jmmm.2003.11.206.

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23

Hu, Junqing, Qingyi Lu, Bin Deng, Kaibin Tang, Yitai Qian, Yuzhi Li, Guien Zhou, and Xianming Liu. "A hydrothermal reaction to synthesize CuFeS2 nanorods." Inorganic Chemistry Communications 2, no. 12 (December 1999): 569–71. http://dx.doi.org/10.1016/s1387-7003(99)00154-9.

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24

Wang, Yu-Hsiang A., Ningzhong Bao, and Arunava Gupta. "Shape-controlled synthesis of semiconducting CuFeS2 nanocrystals." Solid State Sciences 12, no. 3 (March 2010): 387–90. http://dx.doi.org/10.1016/j.solidstatesciences.2009.11.019.

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25

Takaki, Hirokazu, Kazuaki Kobayashi, Masato Shimono, Nobuhiko Kobayashi, Kenji Hirose, Naohito Tsujii, and Takao Mori. "Thermoelectric properties of a magnetic semiconductor CuFeS2." Materials Today Physics 3 (December 2017): 85–92. http://dx.doi.org/10.1016/j.mtphys.2017.12.006.

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26

Barkat, L., N. Hamdadou, M. Morsli, A. Khelil, and J. C. Bernède. "Growth and characterization of CuFeS2 thin films." Journal of Crystal Growth 297, no. 2 (December 2006): 426–31. http://dx.doi.org/10.1016/j.jcrysgro.2006.10.105.

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27

Sainctavit, Ph, J. Petiau, A. M. Flank, J. Ringeissen, and S. Lewonczuk. "XANES in chalcopyrites semiconductors: CuFeS2, CuGaS2, CuInSe2." Physica B: Condensed Matter 158, no. 1-3 (June 1989): 623–24. http://dx.doi.org/10.1016/0921-4526(89)90413-4.

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28

Baba-Kishi, K. Z. "Electron microscopy of the mineral chalcopyrite, CuFeS2." Journal of Applied Crystallography 25, no. 6 (December 1, 1992): 737–43. http://dx.doi.org/10.1107/s0021889892005715.

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29

Harmer, Sarah L., Allen R. Pratt, Wayne H. Nesbitt, and Michal E. Fleet. "Sulfur species at chalcopyrite (CuFeS2) fracture surfaces." American Mineralogist 89, no. 7 (July 2004): 1026–32. http://dx.doi.org/10.2138/am-2004-0713.

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30

SHABUNINA, G. G., T. G. AMINOV, and A. V. FILATOV. "ChemInform Abstract: Interaction of CuFeS2 with Cr2S3." ChemInform 29, no. 35 (June 20, 2010): no. http://dx.doi.org/10.1002/chin.199835029.

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31

Popov, V. V., P. P. Konstantinov, and Yu V. Rud’. "Kinetic phenomena in zero-gap semiconductors CuFeS2 and CuFeTe2: Effect of pressure and heat treatment." Journal of Experimental and Theoretical Physics 113, no. 4 (October 2011): 683–91. http://dx.doi.org/10.1134/s1063776111090093.

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32

Ozkendir, O. M. "Influence of temperature dependence and Li substitution on the electronic structure of delafossite CuFeO2 and CuFeS2 semiconductors." Materialia 15 (March 2021): 100965. http://dx.doi.org/10.1016/j.mtla.2020.100965.

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33

Tinoco, T., J. P. Itié, A. Polian, A. San Miguel, E. Moya, P. Grima, J. Gonzalez, and F. Gonzalez. "Combined x-ray absorption and x-ray diffraction studies of CuGaS2, CuGaSe2, CuFeS2 and CuFeSe2 under high pressure." Le Journal de Physique IV 04, no. C9 (November 1994): C9–151—C9–154. http://dx.doi.org/10.1051/jp4:1994923.

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Park, Junsoo, Yi Xia, and Vidvuds Ozoliņš. "First-principles assessment of thermoelectric properties of CuFeS2." Journal of Applied Physics 125, no. 12 (March 28, 2019): 125102. http://dx.doi.org/10.1063/1.5088165.

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35

Velásquez, P., H. Gómez, D. Leinen, and J. R. Ramos-Barrado. "Electrochemical impedance spectroscopy analysis of chalcopyrite CuFeS2 electrodes." Colloids and Surfaces A: Physicochemical and Engineering Aspects 140, no. 1-3 (September 1998): 177–82. http://dx.doi.org/10.1016/s0927-7757(97)00276-8.

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36

Lovesey, S. W., K. S. Knight, C. Detlefs, S. W. Huang, V. Scagnoli, and U. Staub. "Acentric magnetic and optical properties of chalcopyrite (CuFeS2)." Journal of Physics: Condensed Matter 24, no. 21 (April 25, 2012): 216001. http://dx.doi.org/10.1088/0953-8984/24/21/216001.

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37

Klauber, Craig. "Fracture-induced reconstruction of a chalcopyrite (CuFeS2) surface." Surface and Interface Analysis 35, no. 5 (2003): 415–28. http://dx.doi.org/10.1002/sia.1539.

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38

Dutkova, Erika, Matej Baláž, Nina Daneu, Batukhan Tatykayev, Yordanka Karakirova, Nikolay Velinov, Nina Kostova, Jaroslav Briančin, and Peter Baláž. "Properties of CuFeS2/TiO2 Nanocomposite Prepared by Mechanochemical Synthesis." Materials 15, no. 19 (October 5, 2022): 6913. http://dx.doi.org/10.3390/ma15196913.

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CuFeS2/TiO2 nanocomposite has been prepared by a simple, low-cost mechanochemical route to assess its visible-light-driven photocatalytic efficiency in Methyl Orange azo dye decolorization. The structural and microstructural characterization was studied using X-ray diffraction and high-resolution transmission electron microscopy. The presence of both components in the composite and a partial anatase-to-rutile phase transformation was proven by X-ray diffraction. Both components exhibit crystallite size below 10 nm. The crystallite size of both phases in the range of 10–20 nm was found and confirmed by TEM. Surface and morphological properties were characterized by scanning electron microscopy and nitrogen adsorption measurement. Scanning electron microscopy has shown that the nanoparticles are agglomerated into larger grains. The specific surface area of the nanocomposite was determined to be 21.2 m2·g−1. Optical properties using UV-Vis and photoluminescence spectroscopy were also investigated. CuFeS2/TiO2 nanocomposite exhibits strong absorption with the determined optical band gap 2.75 eV. Electron paramagnetic resonance analysis has found two types of paramagnetic ions in the nanocomposite. Mössbauer spectra showed the existence of antiferromagnetic and paramagnetic spin structure in the nanocomposite. The CuFeS2/TiO2 nanocomposite showed the highest discoloration activity with a MO conversion of ~ 74% after 120 min irradiation. This study has shown the possibility to prepare nanocomposite material with enhanced photocatalytic activity of decoloration of MO in the visible range by an environmentally friendly manner

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Tsang, Jeffrey J., and David L. Parry. "Metal Mobilization from Complex Sulfide Ore Concentrate: Effect of Light and pH." Australian Journal of Chemistry 57, no. 10 (2004): 971. http://dx.doi.org/10.1071/ch04081.

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The aim of this study was to determine the influence of photo-irradiation and pH on the mobilization of metals from a complex sulfide ore concentrate containing known semiconductors (PbS, ZnS, CdS, FeS2, and CuFeS2). The mobilization of Zn, Fe, and Cd increased under illumination, which is attributed to the semiconductor nature of ZnS, FeS2, and CdS, respectively. An increase in mobilization of Zn, Fe, and Cd under light is observed with decreasing pH, because of increased surface protonation and the greater oxidizing property of photoholes. The semiconductor nature of PbS and CuFeS2 is observed at pH 2. However, at higher pH the concentrations of mobilized Pb and Cu are greater in darkness than under illumination. This is attributed to the light enhanced exchange reactions involving dissolved Pb and Cu with metal sulfides more soluble than PbS and CuS.

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Couderc, Jean-Jacques, and Christa Hennig-Michaeli. "TEM study of mechanical twinning in experimentally deformed chalcopyrite (CuFeS2) single crystals." European Journal of Mineralogy 1, no. 2 (May 3, 1989): 275–94. http://dx.doi.org/10.1127/ejm/1/2/0275.

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41

Hennig-Michaeli, Christa, and Jean-Jacques Couderc. "TEM study of mechanical twinning in experimentally deformed chalcopyrite (CuFeS2) single crystals." European Journal of Mineralogy 1, no. 2 (May 3, 1989): 295–314. http://dx.doi.org/10.1127/ejm/1/2/0295.

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42

Vilcáez, Javier, Koichi Suto, and Chihiro Inoue. "Modeling the Auto-Thermal Performance of a Thermophilic Chalcopyrite Bioleaching Heap Employing Mesophilic and Thermophilic Microbes." Advanced Materials Research 20-21 (July 2007): 70–74. http://dx.doi.org/10.4028/www.scientific.net/amr.20-21.70.

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A model was prepared to study the performance of a thermophilic bioleaching heap that employs mixed mesophilic and thermophilic microbes for copper extraction from CuFeS2. Mesophiles’ preference for and ease of dissolving additional FeS2 provided to the heap enables the transition from a mesophilic to a thermophilic bioleaching state without the necessity of additional energy supply. In this sense, the mathematical description of the bioleaching process is done taking into consideration the dependency of both microbes’ biological states on physicochemical factors such as the temperature and O2 availability. With regard to the flow rates of the liquid and air phases, simulation results have shown that these flow rates govern not just the heat transfer and variation of cell distribution, but also the leaching rate regardless of the fraction of CuFeS2 per FeS2 leached (FCP) which is the other variable influencing to the heat accumulation in the heap.

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43

Pogoreltsev, Aleksandr, Vadim Matukhin, Ekaterina Shmidt, Valery Galiakhmetov, and Yaroslav Shaikhutdinov. "The distribution of the electron density and spin density in the interplanar areas CuFeS2 by NMR 63,65Cu in a local field." E3S Web of Conferences 288 (2021): 01050. http://dx.doi.org/10.1051/e3sconf/202128801050.

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Chalcopyrite CuFeS2 is a known semiconductor mineral with a wide range of unique physical and chemical properties. These materials can be used as elements of solar batteries, coherent and incoherent sources of polarized radiation, in photovoltaic, thermoelectric and spintronic devices. Despite the relatively large number of studies on CuFeS2, many questions about its magnetic and electronic properties, are still outstanding. In this paper we were carried out studies of the distribution of the electron density and spin density in the nuclei of iron and copper in the semiconductor mineral CuFeS2. Special attention was devoted to interrelation of electronic and spin subsystems of the compound. The results of studies of the compound obtained in NMR 63,65Cu local field at low temperatures were used to perform the corresponding analysis. The cluster approach was used. The biggest cluster had Cu9Fe10S28-4 formula. Calculations were carried out in the framework of restricted self-consistent Hartree - Fock with open shells (SCF-LCAO-ROHF), MINI basis. The calculations were made with the “foundation” on the quadrupole parameters (quadrupole νQ frequency and the asymmetry parameter of the electric field gradient tensor η), obtained from the experiment. Study of electron density maps were performed for the regions containing chains of Fe-S-Cu and S-Fe-S for the different layers of metals and sulfur atoms. It is shown that the nature of the connection of iron atoms belonging to neighboring layers with sulfur atoms of the intermediate layer is different, which is reflected on the electron density distribution.

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Liang, Da Xin, Jian Li, Lu Li, and Guang Sheng Pang. "Fenton Degradation of Methylene Blue by CuFeS₂ Ultrafine Powders." Key Engineering Materials 609-610 (April 2014): 449–54. http://dx.doi.org/10.4028/www.scientific.net/kem.609-610.449.

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Fenton reagent was made by CuFeS2 ultrafine powders with peroxide, and this Fenton reagent can degrade methylene blue solution with 10 mg/L concentration within 1 min. UV-vis spectra were used to investigate this Fenton reagent's degradation activity of methylene blue.

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Kuncaka, Agus, Eko Sugiharto, and Yasinta Endah Nastiti. "EXTRACTION OF COPPER ELECTROLYTICALLY BY USING SOLID MIXTURE OF CuFeS₂ AND CaCO₃ (CHALCOPYCA) AS ANODE." Indonesian Journal of Chemistry 5, no. 3 (June 15, 2010): 295–301. http://dx.doi.org/10.22146/ijc.21807.

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Study on a new road of copper electroextraction to make use the solid mixture of CuFeS2 and CaCO3 as anode has been done. The aim of these research was to determine reaction kinetic and faradic efficiency of anodic copper dissolution and catodic copper precipitation. A solid mixture of CuFeS2 and CaCO3 at weight ratio 9:1 was functioned as anode. Electrolysis was carried out at 1.5 mA by varying times of 30,60,120, and 240 minutes in Na2SO4 0.5 M + H2SO4 0.01 M electrolyte. The quantity of copper at the electrolyte and cathode was analyzed by Atomic Absorption Spectrophotometer (AAS). The result of these research showed that copper was deposited in the cathode simultaneously with anodic dissolution. The kinetic of copper dissolution follow zero order with rate constant of 5.10-6 mg/second. The faradic efficiency of copper dissolution and precipitation for those various time respectively were 17.31%; 14.00%; 11,16%; 62.31%; and 1.60%; 8.61%; 7.59%; 60.63%. Keywords: electroextraction, faradic efficiency, copper dissolution.

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46

Engin, T. E., A. V. Powell, and S. Hull. "A high temperature diffraction-resistance study of chalcopyrite, CuFeS2." Journal of Solid State Chemistry 184, no. 8 (August 2011): 2272–77. http://dx.doi.org/10.1016/j.jssc.2011.06.036.

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47

Sekiya, H., T. Isobe, A. Nakajima, and S. Matsushita. "Can CuFeS2 be used in a sensitized thermal cell?" Materials Today Energy 17 (September 2020): 100469. http://dx.doi.org/10.1016/j.mtener.2020.100469.

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48

Wang, M. X., L. S. Wang, G. H. Yue, X. Wang, P. X. Yan, and D. L. Peng. "Single crystal of CuFeS2 nanowires synthesized through solventothermal process." Materials Chemistry and Physics 115, no. 1 (May 2009): 147–50. http://dx.doi.org/10.1016/j.matchemphys.2008.11.032.

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49

Poloko, Nenguba, Gwiranai Danha, and Tshepho Gaogane. "Processing and characterization of chalcopyrite (CuFeS2) sample from Botswana." Procedia Manufacturing 35 (2019): 488–93. http://dx.doi.org/10.1016/j.promfg.2019.05.070.

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50

Velásquez, P., H. Gómez, J. R. Ramos-Barrado, and D. Leinen. "Voltammetry and XPS analysis of a chalcopyrite CuFeS2 electrode." Colloids and Surfaces A: Physicochemical and Engineering Aspects 140, no. 1-3 (September 1998): 369–75. http://dx.doi.org/10.1016/s0927-7757(97)00293-8.

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