Aqueous synthesis of finely divided pyrite particles

Wei, Dawei; Osseo‐Asare, K.

doi:10.1016/s0927-7757(95)03502-8

Cited by 30 publications

(26 citation statements)

References 52 publications

Supporting

Mentioning

Contrasting

Unclassified

Order By: Relevance

“…The water used was deionized (18.2 MΩ), boiled, and argon purged during cooling, before introducing it in the glovebox. Nanosized pyrite was synthesized according to the protocol published by D. Wei et al (1996) 27,28 and Liu X et al (2008). 16 A solution of 250 mL of 0.2 M NaHS was poured into 250 mL of 0.1 M FeCl 3 solution and stored in a 500 mL bottle under persistent stirring.…”

Section: ■ Materials and Methodsmentioning

confidence: 99%

“…31 The ATOMS package 32 was used to generate the atomic clusters centered on the absorber atom (Se), which were used as reference structures for calculating theoretical amplitude and phase backscattering functions with the FEFF8 package. 33 ■ RESULTS AND DISCUSSION Trying to synthesize highly purified pyrite, using a 1:2 ratio of FeCl 3 versus NaHS, 16,27,28 resulted in a significant amount (28%) of greigite (Fe 2+ Fe 3+ 2 S 4 ) in the final product ( Figure S1). reported that Fe 3 S 4 is one of the important precursors for pyrite formation and is absent in highly reduced environments.…”

Section: ■ Materials and Methodsmentioning

confidence: 99%

See 1 more Smart Citation

Nanocomposite Pyrite–Greigite Reactivity toward Se(IV)/Se(VI)

Charlet

Kang

Bardelli

et al. 2012

Environ. Sci. Technol.

View full text Add to dashboard Cite

A nanopyrite/greigite composite was synthesized by reacting FeCl(3) and NaHS in a ratio of 1:2 (Wei et al. 1996). Following this procedure, the obtained solid phases consisted of 30-50 nm sized particles containing 28% of greigite (Fe(2+)Fe(3+)(2)S(4)) and 72% pyrite (FeS(2)). Batch reactor experiments were performed with selenite or selenate by equilibrating suspensions containing the nanosized pyrite-greigite solid phase at different pH-values and with or without the addition of extra Fe(2+). XANES-EXAFS spectroscopic techniques revealed, for the first time, the formation of ferroselite (FeSe(2)) as the predominant reaction product, along with elemental Se. In the present experimental conditions, at pH 6 and in equilibrium with Se(0), the solution is oversaturated with respect to ferrosilite. Furthermore, thermodynamic computations show that reaction kinetics likely played a significant role in our experimental system.

show abstract

Section: ■ Materials and Methodsmentioning

confidence: 99%

Section: ■ Materials and Methodsmentioning

confidence: 99%

Nanocomposite Pyrite–Greigite Reactivity toward Se(IV)/Se(VI)

Charlet

Kang

Bardelli

et al. 2012

Environ. Sci. Technol.

View full text Add to dashboard Cite

show abstract

“…This morphology is typical of elemental sulfur. [32] It is interesting to note that a lot of these particles seem to be well attached on the irregular surface of reacted FeS grains. This suggests that they have grown on FeS surface but not into solution.…”

Section: Scanning Electron Microscopy (Sem)mentioning

confidence: 98%

Iron monosulfide (FeS) oxidation by dissolved oxygen: characteristics of the product layer

Chiriţă

2009

Surface & Interface Analysis

View full text Add to dashboard Cite

Samples of FeS were oxidized by oxygen-bearing acidic solutions at 25• C and different initial pH values (2.75 ≤ pH ≤ 3.45). The reacted FeS samples were investigated by scanning electron microscopy (SEM), nitrogen adsorption/desorption isotherms measurements, and FT-Raman spectroscopy. A sulfur rich phase (layer) is inferred to be form on reacting FeS surface based on sequential extraction with acidic chromium(II) chloride solutions. The sulfur-rich layer (SRL) formed on oxidized FeS samples is traversed by various mesopores with average pore size <450Å. It is reasonable to assume that the mesopores facilitate the migration of iron and sulfur from FeS structure into solution across SRL. The FT-Raman spectra of oxidized FeS samples show an intense peak at 162 cm −1 , which can be attributed to SRL developed on FeS surface. A model for SRL development on FeS during its oxidation by dissolved oxygen has been proposed from the present results and previous studies.

show abstract

“…The pyrite used was synthesized using the method developed by D. Wei et al [13]. The procedure is described briefly as follows: A batch of pyrite samples was made in 50 mL vials in the glove box.…”

Section: Pyrite Synthesismentioning

confidence: 99%

Selenide retention onto pyrite under reducing conditions

Liu¹,

Fattahi²,

Montavon³

et al. 2008

Radiochimica Acta

View full text Add to dashboard Cite

Pyrite (FeS2) is a mineral phase often present as inclusions in temperate soils. Moreover, it turns out to be a sorption sink for certain radionuclides in deep geological disposals. The present study was thus initiated to determine the capacity of pyrite to immobilize selenide (Se(-II)). Due to the fact that pyrite surface oxidizes readily, potentials were applied in order to minimise its surface evolution, and ensure the reducing conditions necessary for stabilizing Se(-II). The sorption experiments were carried out in NaCl electrolyte and were amperometrically controlled. After only several minutes of reaction, at least 97% of Se(-II) initially present in solution was disappeared. The Kd values vary from 7–65 L/g and the isotherm curve shows site saturation at higher initial selenide concentrations and no pH-dependence. By means of several spectroscopic techniques, the reaction mechanism was investigated. The XRD and in situ XANES results indicate the presence of Se(0) on pyrite surface, which explain the rapid disappearance of Se observed in the sorption experiments. Moreover, XPS results obtained from Se-reacted pyrite particles reveal cleavage of S–S bonding which resulted in formation of S2− on pyrite surface. Thus, we conclude that Se(-II) can be immobilized by pyrite via surface redox reaction: ≡FeS2 + HSe− ⇔ ≡FeS + Se(0) + HS−

show abstract

Aqueous synthesis of finely divided pyrite particles

Cited by 30 publications

References 52 publications

Nanocomposite Pyrite–Greigite Reactivity toward Se(IV)/Se(VI)

Nanocomposite Pyrite–Greigite Reactivity toward Se(IV)/Se(VI)

Iron monosulfide (FeS) oxidation by dissolved oxygen: characteristics of the product layer

Selenide retention onto pyrite under reducing conditions

Contact Info

Product

Resources

About