Why Is Iron (III) Sulfide Fe2S3???? | Yahoo Answers ~ Live Science: The Most Interesting Articles, Mysteries & Discoveries

Iron sulfides are probably the most encountered semiconductive deposit types in oil and gas production and transmission pipelines. Numerous iron sulfides can exist, the nature of which is dependent on the environment and operating parameters.Iron(III) sulfide, also known as ferric sulfide or sesquisulfide, is one of the three iron sulfides besides FeS and FeS2. It is a solid, black powder but decays at ambient temperature into a yellow-green powder. Iron(II) sulfide or ferrous sulfide (Br.E. sulphide) is a chemical compound with the formula...Iron(III) sulfide Fe2S3 particles were produced using a polyol method. Although pyrrhotite Fe1−xS appeared together with Fe2S3, the relative yield of Fe2S3 changed when the concentration of reagents in the oleylamine changed. Mössbauer spectra of the particles showed superparamagnetic doublets...железа(III) сульфид — geležies(III) sulfidas statusas T sritis chemija formulė Fe₂S₃ atitikmenys: angl. ferric sulfide; iron(III) sulfide rus. железа трисульфид; железа(III) сульфид ryšiai: sinonimas - digeležies trisulfidas …IUPAC Name: Iron(3+) trisulfide Synonyms of Iron(III) sulfide (CAS NO.12063-27-3) : Ferric sulfide ; Iron sesquisulfide ; Iron(3+) sulfide CAS NO When Iron(III) sulfide (CAS NO.12063-27-3) is heated to decomposition ,it emits toxic fumes of SOx. See also IRON COMPOUNDS and SULFIDES.

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English. iron(III) sulfide. esperanto. fera(III) sulfido. español. Sulfuro de hierro. فارسی. سولفید آهن(III).Iron (III ) sulphide Fe2S3 is a solid, black substance, but decomposes at room temperature into a yellowish-gray powder mixture of iron (II ) sulfide, and Is added to an ice-cooled aqueous solution of iron ( III ) chloride also a cooled aqueous solution of sodium sulfide, then a black precipitate of iron...Iron(III) sulfide, also known as ferric sulfide or sesquisulfide, is one of the three iron sulfides besides FeS and FeS2. It is a solid, black powder but decays at ambient temperature into a yellow-green powder.Iron(III) Sulfide. Alias: Ferric Sulfide.

Iron (III) sulfide particles produced by a polyol method | Request PDF

Iron(III) sulfide, also known as ferric sulfide or sesquisulfide, is one of the three iron sulfides besides FeS and FeS2. It is a solid, black powder but decays at ambient temperature into a yellow-green powder. This is a relatively unstable artificial product that does not occur in nature.iron(III) sulfide (Q420355). From Wikidata. Jump to navigation Jump to search. Also known as. English. iron(III) sulfide. chemical compound.iron sulfide. iron(II) sulfide. The oxidation number of iron in iron sulphide is 2. Synthesis.Iron(III) sulfide, also known as ferric sulfide or sesquisulfide, is one of the three iron sulfides besides FeS and FeS2. It is a solid, black powder but decays at ambient temperature into a yellow-green powder. This is a relatively unstable artificial product that does not occur in nature.Iron III Sulfide is a compound consisting of 2 atoms of iron and 3 atoms of sulfur. This is rapidly oxidised by air.Iron(II,III) sulfide Fe3S4, which is found in nature as a mineral greigite and is ferromagnetic like Fe3O4.

Iron(III) sulfide, often referred to as ferric sulfide or sesquisulfide, is one of the three iron sulfides besides FeS and FeS2. It is a forged, black powder but decays at ambient temperature right into a yellow-green powder.

This is a fairly unstable synthetic product that does not happen in nature.

Preparation and houses

Fe2S3 is ready via addition of refrigerated iron(III) chloride dilution to additionally cooled sodium sulfide dilution.

2 FeCl3 + Three Na2S → Fe2S3↓ + 6 NaCl

which decays at a temperature over 20°C into FeS and sulphur. [2]

Fe2S3 → 2 FeS + S↓

With hydrochloric acid it decays in step with the next reaction equation: [3]

Fe2S3 + Four HCl → 2 FeCl2 + 2 H2S↑ + S↓

References

^ a b c d e Charles D. Hodgman, Handbook of Chemistry and Physics (1961), p.590 ^ Holleman, Wiberg: Inorganic Chemistry (2001), p. 1451; ISBN 0-12-352651-5 ^ H. Roempp, Chemie (1997), S. 1099; ISBN 3-13-734710-6