Iron(III) sulfide

Last updated
Iron(III) sulfide
Names
IUPAC name
Iron(III) sulfide
Other names
Iron sesquisulfide

Ferric sulfide

Diiron trisulfide
Identifiers
ChEBI
PubChem CID
Properties
Fe2S3
Molar mass 207.90 g/mol [1]
Appearanceyellow-green [1]
Density 4.3 g/cm3 [1]
Melting point decomposition [1]
very slightly soluble [1]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)
Infobox references

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 chemical compound

Iron(II) sulfide or ferrous sulfide is one of a family chemical compounds and minerals with the approximate formula FeS. Iron sulfides are often iron-deficient non-stoichiometric. All are black, water-insoluble solids.

FeS2 may refer to:

Contents

This is a relatively unstable artificial product that does not occur in nature.

Preparation and properties

Sources

Fe2S3 is prepared by addition of refrigerated iron(III) chloride solution to also cooled sodium sulfide solution.[ citation needed ]

Iron(III) chloride chemical compound

Iron(III) chloride (FeCl
3
), also called ferric chloride, is an industrial scale commodity chemical compound with iron in the +3 oxidation state. The compound also exist as a hexahydrate with the formula trans-[Fe(H
2
O)
4
Cl
2
]Cl · 2H2O normally written as FeCl
3
 · 6H
2
O
. The anhydrous compound is a crytalline solid with a melting point of 307.6 °C. The color depends on the viewing angle: by reflected light the crystals appear dark green, but by transmitted light they appear purple-red. The hexahydrate has a melting point of 37 °C and appears orange-brown in color. In nature, iron(III) chloride is known as the mineral molysite, but it is rare and mainly found from some fumaroles. It is however an industrial scale commodity.

Sodium sulfide chemical compound

Sodium sulfide is the chemical compound with the formula Na2S, or more commonly its hydrate Na2S·9H2O. Both are colorless water-soluble salts that give strongly alkaline solutions. When exposed to moist air, Na2S and its hydrates emit hydrogen sulfide, which smells like rotten eggs. Some commercial samples are specified as Na2xH2O, where a weight percentage of Na2S is specified. Commonly available grades have around 60% Na2S by weight, which means that x is around 3. Such technical grades of sodium sulfide have a yellow appearance owing to the presence of polysulfides. These grades of sodium sulfide are marketed as 'sodium sulfide flakes'. Although the solid is yellow, solutions of it are colorless.

2 FeCl3 + 3 Na2S → Fe2S3↓ + 6 NaCl

It is also produced as a side-product of desulfurization of fuel gasses. The gas is pumped through a container of hydrated iron(III) oxide, which combines with hydrogen sulfide.

Iron(III) oxide chemical compound

Iron(III) oxide or ferric oxide is the inorganic compound with the formula Fe2O3. It is one of the three main oxides of iron, the other two being iron(II) oxide (FeO), which is rare; and iron(II,III) oxide (Fe3O4), which also occurs naturally as the mineral magnetite. As the mineral known as hematite, Fe2O3 is the main source of iron for the steel industry. Fe2O3 is readily attacked by acids. Iron(III) oxide is often called rust, and to some extent this label is useful, because rust shares several properties and has a similar composition. To a chemist, rust is considered an ill-defined material, described as hydrated ferric oxide.

Hydrogen sulfide Poisonous, corrosive and flammable gas

Hydrogen sulfide is the chemical compound with the formula H
2
S
. It is a colorless chalcogen hydride gas with the characteristic foul odor of rotten eggs. It is very poisonous, corrosive, and flammable.

Fe
2
O
3
(s) + H
2
O
(l) + 3 H
2
S
(g)Fe
2
S
3
(s) + 4 H
2
O
(l)

Reactions

Iron(III) sulfide decays at a temperature over 20 °C into iron(II) sulfide (FeS) and elemental sulfur: [2]

Fe2S3 → 2 FeS + S↓

With hydrochloric acid it decays according to the following reaction equation: [3]

Fe2S3 + 4 HCl → 2 FeCl2 + 2 H2S↑ + S↓

Related Research Articles

Stoichiometry calculation of relative quantities of reactants and products in chemical reactions

Stoichiometry is the calculation of reactants and products in chemical reactions.

Sulfuric acid chemical compound

Sulfuric acid (alternative spelling sulphuric acid), also known as vitriol, is a mineral acid composed of the elements sulfur, oxygen and hydrogen, with molecular formula H2SO4. It is a colorless, odorless, and syrupy liquid that is soluble in water, in a reaction that is highly exothermic.

In chemistry, a reactivity series (or activity series) is an empirical, calculated, and structurally analytical progression of a series of metals, arranged by their "reactivity" from highest to lowest. It is used to summarize information about the reactions of metals with acids and water, double displacement reactions and the extraction of metals from their ores.

Classical qualitative inorganic analysis is a method of analytical chemistry which seeks to find the elemental composition of inorganic compounds. It is mainly focused on detecting ions in an aqueous solution, therefore materials in other forms may need to be brought to this state before using standard methods. The solution is then treated with various reagents to test for reactions characteristic of certain ions, which may cause color change, precipitation and other visible changes.

Iron(II,III) oxide chemical compound

Iron(II,III) oxide is the chemical compound with formula Fe3O4. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others being iron(II) oxide (FeO), which is rare, and iron(III) oxide (Fe2O3) also known as hematite. It contains both Fe2+ and Fe3+ ions and is sometimes formulated as FeO ∙ Fe2O3. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ferrimagnetic, but is sometimes incorrectly described as ferromagnetic. Its most extensive use is as a black pigment. For this purpose, it is synthesised rather than being extracted from the naturally occurring mineral as the particle size and shape can be varied by the method of production.

Iron(II) chloride chemical compound

Iron(II) chloride, also known as ferrous chloride, is the chemical compound of formula FeCl2. It is a paramagnetic solid with a high melting point. The compound is white, but typical samples are often off-white. FeCl2 crystallizes from water as the greenish tetrahydrate, which is the form that is most commonly encountered in commerce and the laboratory. There is also a dihydrate. The compound is highly soluble in water, giving pale green solutions.

Gold(III) chloride chemical compound

Gold(III) chloride, traditionally called auric chloride, is a chemical compound of gold and chlorine. With the molecular formula Au2Cl6, the name gold trichloride is a simplification, referring to the empirical formula, AuCl3. The Roman numerals in the name indicate that the gold has an oxidation state of +3, which is common for gold compounds. There is also another related chloride of gold, gold(I) chloride (AuCl). Chloroauric acid, HAuCl4, the product formed when gold dissolves in aqua regia, is sometimes referred to as "gold chloride" or "acid gold trichloride". Gold(III) chloride is very hygroscopic and highly soluble in water as well as ethanol. It decomposes above 160 °C or in light.

Tin(II) chloride chemical compound

Tin(II) chloride, also known as stannous chloride, is a white crystalline solid with the formula SnCl2. It forms a stable dihydrate, but aqueous solutions tend to undergo hydrolysis, particularly if hot. SnCl2 is widely used as a reducing agent (in acid solution), and in electrolytic baths for tin-plating. Tin(II) chloride should not be confused with the other chloride of tin; tin(IV) chloride or stannic chloride (SnCl4).

Iron(III) oxide-hydroxide chemical compound

Iron(III) oxide-hydroxide or ferric oxyhydroxide is the chemical compound of iron, oxygen, and hydrogen with formula FeO(OH).

Antimony trichloride chemical compound

Antimony trichloride is the chemical compound with the formula SbCl3. The soft colorless solid with a pungent odor was known to the alchemists as butter of antimony.

iron(II) carbonate, or ferrous carbonate, is a chemical compound with formula FeCO
3
, that occurs naturally as the mineral siderite. At ordinary ambient temperatures, it is a green-brown ionic solid consisting of iron(II) cations Fe2+
and carbonate anions CO2−
3
.

Thiosulfuric acid chemical compound

Thiosulfuric acid is a sulfur oxoacid. The acid cannot be made by acidifying aqueous thiosulfate salt solutions as the acid readily decomposes in water. The decomposition products can include sulfur, sulfur dioxide, hydrogen sulfide, polysulfanes, sulfuric acid and polythionates, depending on the exact reaction conditions. Anhydrous methods of producing the acid were developed by Carol Schmidt:

Hydrochloric acid strong mineral acid

Hydrochloric acid or muriatic acid is a colorless inorganic chemical system with the formula H
2
O:HCl
. Hydrochloric acid has a distinctive pungent smell. It is classified as strongly acidic and can attack the skin over a wide composition range, since the hydrogen chloride completely dissociates in aqueous solution.

Gallium(III) sulfide, Ga2S3, is a compound of sulfur and gallium, that is a semiconductor that has applications in electronics and photonics.

Aluminium triacetate, formally named aluminium acetate, is a chemical compound with composition Al(CH
3
CO
2
)
3
. Under standard conditions it appears as a white, water-soluble solid that decomposes on heating at around 200 °C. The triacetate hydrolyses to a mixture of basic hydroxide / acetate salts, and multiple species co-exist in chemical equilibrium, particularly in aqueous solutions of the acetate ion; the name aluminium acetate is commonly used for this mixed system.

References

  1. 1 2 3 4 5 Charles D. Hodgman, Handbook of Chemistry and Physics (1961), p.590
  2. Holleman, Wiberg (2001). Inorganic Chemistry. p. 1451. ISBN   0-12-352651-5.
  3. H. Roempp, Chemie (1997), S. 1099; ISBN   3-13-734710-6