iron sulfide
FeS(g). Thermodynamic properties of iron sulfide in the standard state at temperatures of 100 - 6000 K are given in table. FeS.
The FeS molecular constants used to calculate the thermodynamic functions are given in Table 1. Fe.4.
The electronic spectrum of FeS in the gas phase is not known. Some IR and visible bands in the spectrum of iron sulfides isolated in a low-temperature matrix [75DEV/FRA] were attributed to the FeS molecule. The photoelectron spectrum of the anion FeS - [ 2003ZHA/KIR ] was studied; in addition to the ground state, 6 excited states of FeS were observed in the spectrum. The microwave spectrum has been studied [ 2004TAK/YAM ]. The authors identified 5 series of transitions associated with v = 0 and two series associated with v = 1 of the ground state X 5D. In addition, they found 5 series of transitions, which were attributed to the 7 Σ or 5 Σ state. The ground state is perturbed.
Theoretical studies [ 75HIN/DOB, 95BAU/MAI, 2000BRI/ROT ] are devoted to the main X 5 D state of FeS. An unsuccessful calculation of the electronic structure is presented in [75HIN/DOB], according to the calculation, the first excited state 7 Σ has an energy of 20600 cm -1 .
Vibrational constant in X 5 D state w e = 530 ± 15 cm -1 was estimated based on the frequency of 520 ± 30 found in the photoelectron spectrum and the frequency of 540 cm -1 measured in the spectrum of the low-temperature matrix [75DEV/FRA]. Rotational constants B e and D e calculated from microwave spectrum data for the Ω = 4 component [2004TAK/YAM]. The estimate r e = 2.03 ± 0.05 Å, obtained from the semiempirical relation r MS = 0.237 + 1.116 × r MO proposed by Barrow and Cousins [71BAR/COU]. Calculations [95BAU/MAI, 2000BRI/ROT] give close values of the constants w e and r e. In [2004TAK/YAM] an attempt was made to determine the multiplet splitting of the ground state by fitting the data to the known 5D state formula; due to perturbations, only the components Ω = 4, 3, 1 were taken into account in the calculation for v = 0, and for v = 1 the components Ω = 4, 3. The results obtained (A(v=0) = -44.697 and A(v= 1) = -74.888) are doubtful; therefore, in this work, we estimate the multiplet splitting of the ground state to be approximately the same as that of the FeO molecule.
The study of the photoelectronic spectrum [ 2003ZHA/KIR ] FeS - gives information about 6 excited states. It is difficult to agree with the interpretation of the authors: the spectrum is very similar to the photoelectron spectrum of FeO, both in the position of the states and in their vibrational structure. The authors attribute an intense single peak at 5440 cm -1 to the first excited state 7 Σ (the energy of this state in FeO is 1140 cm -1 , it causes a disturbance in the ground state and has a developed vibrational structure). This peak most likely belongs to the 5 Σ state (the energy of this state in FeO is 4090 cm -1 , the vibrational structure is not developed). The peaks at 8900, 10500 and 11500 cm -1 correspond to the states of FeOy 3 Δ, 5 Φ and 5 Π with energies of 8350, 10700 and 10900 cm -1 with a well-developed vibrational structure, and the region where the peaks at 21700 and 23700 cm in the photoelectron spectrum of FeO was not studied. Based on the analogy of the FeS and FeO molecules, the unobserved electronic states were estimated in the same way as for the FeO molecule, while it was assumed that the upper limit for all configurations has the energy D 0 (FeS) + I 0 (Fe) " 90500 cm -1 .
The thermodynamic functions of FeS(g) were calculated using equations (1.3) - (1.6) , (1.9) , (1.10) , (1.93) - (1.95) . Values Q ext and its derivatives were calculated by equations (1.90) - (1.92) taking into account sixteen excited states (components of the ground X 5 D states were considered as singlet states with L ¹ 0) under the assumption that Q no.vr ( i) = (pi/p X)Q no.vr ( X) . Value Q no.vr ( X) and its derivatives for the main X 5 D 4 states were calculated by equations (1.73) - (1.75) by direct summation over vibrational levels and integration over the values J using equations like (1.82) . The calculation took into account all energy levels with values J < Jmax,v, where Jmax,v was determined by relation (1.81) . Vibrational-rotational levels of state X 5 D 4 states were calculated by equations (1.65) , (1.62) . Coefficient values Ykl in these equations were calculated by relations (1.66) for the isotopic modification corresponding to the natural isotopic mixture of iron and sulfur atoms, from the molecular constants for 56 Fe 32 S given in Table. Fe.4. Values Ykl, as well as vmax and Jlim are given in table. Fe.5.
The errors in the calculated thermodynamic functions of FeS(r) over the entire temperature range are mainly due to the inaccuracy of the energies of the excited states. Errors in Φº( T) at T= 298.15, 1000, 3000 and 6000 K are estimated at 0.3, 1, 0.8 and 0.7 J×K -1 × mol -1 , respectively.
Previously, the thermodynamic functions of FeS(r) were calculated in the JANAF tables [85CHA/DAV] up to 6000 K, taking into account the excited states, whose energies were assumed to be identical to the levels of the Fe2+ ion under the assumption that in the ground state p X= 9 (without multiplet splitting), B e = 0.198 and w e = 550 cm -1 . Discrepancies between the FeS table data and the data [
Abstract on the topic:
Iron sulfides ( FeS , FeS 2 ) and calcium ( CaS )
Made by Ivanov I.I.
Introduction
Properties
Origin (genesis)
Sulfides in nature
Properties
Origin (genesis)
Spreading
Application
Pyrrhotite
Properties
Origin (genesis)
Application
Marcasite
Properties
Origin (genesis)
Place of Birth
Application
Oldgamite
Receipt
Physical Properties
Chemical properties
Application
chemical weathering
Thermal analysis
thermogravimetry
Derivatography
Derivatographic analysis of pyrite
Sulfides
Sulfides are natural sulfur compounds of metals and some non-metals. Chemically, they are considered as salts of hydrosulfide acid H 2 S. A number of elements form polysulfides with sulfur, which are salts of polysulfuric acid H 2 S x. The main elements that form sulfides are Fe, Zn, Cu, Mo, Ag, Hg, Pb, Bi, Ni, Co, Mn, V, Ga, Ge, As, Sb.
Properties
The crystal structure of sulfides is due to the densest cubic and hexagonal packing of S 2- ions, between which metal ions are located. the main structures are represented by coordination (galena, sphalerite), insular (pyrite), chain (antimonite) and layered (molybdenite) types.
The following general physical properties are characteristic: metallic luster, high and medium reflectivity, relatively low hardness and high specific gravity.
Origin (genesis)
They are widely distributed in nature, making up about 0.15% of the mass of the earth's crust. The origin is predominantly hydrothermal; some sulfides are also formed during exogenous processes in a reducing environment. They are ores of many metals - Cu, Ag, Hg, Zn, Pb, Sb, Co, Ni, etc. The class of sulfides includes antimonides, arsenides, selenides and tellurides close to them in properties.
Sulfides in nature
Under natural conditions, sulfur occurs in two valence states of the S 2 anion, which forms S 2- sulfides, and the S 6+ cation, which is included in the S0 4 sulfate radical.
As a result, the migration of sulfur in the earth's crust is determined by the degree of its oxidation: a reducing environment promotes the formation of sulfide minerals, and oxidizing conditions favor the formation of sulfate minerals. Neutral atoms of native sulfur represent a transitional link between two types of compounds, depending on the degree of oxidation or reduction.
Pyrite
Pyrite is a mineral, iron disulfide FeS 2, the most common sulfide in the earth's crust. Other names for the mineral and its varieties: cat's gold, fool's gold, iron pyrite, marcasite, bravoite. The sulfur content is usually close to theoretical (54.3%). Ni, Co impurities are often present (a continuous isomorphic series with CoS; usually, cobalt pyrite contains from tenths of % to several % of Co), Cu (from tenths of % to 10%), Au (often in the form of tiny inclusions of native gold), As (up to several%), Se, Tl (~ 10-2%), etc.
Properties
The color is light brassy and golden yellow, reminiscent of gold or chalcopyrite; sometimes contains microscopic inclusions of gold. Pyrite crystallizes in the cubic system. Crystals in the form of a cube, a pentagon-dodecahedron, less often an octahedron, are also found in the form of massive and granular aggregates.
Hardness on a mineralogical scale 6 - 6.5, density 4900-5200 kg / m3. On the surface of the Earth, pyrite is unstable, easily oxidized by atmospheric oxygen and groundwater, turning into goethite or limonite. Luster is strong, metallic.
Origin (genesis)
It is established in almost all types of geological formations. It is present as an accessory mineral in igneous rocks. It is usually an essential component in hydrothermal veins and metasomatic deposits (high-, medium- and low-temperature). In sedimentary rocks, pyrite occurs as grains and nodules, for example, in black shales, coals, and limestones. Sedimentary rocks are known, consisting mainly of pyrite and chert. Often forms pseudomorphs after fossil wood and ammonites.
Spreading
Pyrite is the most common mineral of the sulfide class in the earth's crust; occurs most often in deposits of hydrothermal origin, massive sulfide deposits. The largest industrial accumulations of pyrite ores are located in Spain (Rio Tinto), the USSR (Urals), Sweden (Bouliden). In the form of grains and crystals, it is distributed in metamorphic schists and other iron-bearing metamorphic rocks. Pyrite deposits are developed mainly to extract the impurities contained in it: gold, cobalt, nickel, copper. Some pyrite-rich deposits contain uranium (Witwatersrand, South Africa). Copper is also extracted from massive sulfide deposits in Ducktown (Tennessee, USA) and in the valley of the river. Rio Tinto (Spain). If there is more nickel in the mineral than iron, it is called bravoite. Oxidized, pyrite turns into limonite, so buried pyrite deposits can be detected by limonite (iron) hats on the surface. Main deposits: Russia, Norway, Sweden, France, Germany, Azerbaijan, USA.
Application
Pyrite ores are one of the main types of raw materials used to produce sulfuric acid and copper sulphate. Non-ferrous and precious metals are extracted from it along the way. Due to its ability to strike sparks, pyrite was used in the wheel locks of the first guns and pistols (steel-pyrite pair). Valuable collectible.
Pyrrhotite
Properties
Pyrrhotite is fiery red or dark orange in color, magnetic pyrites, a mineral from the class of sulfides of the Fe 1-x S composition. Ni, Co are included as impurities. The crystal structure has the densest hexagonal packing of S atoms.
The structure is defective, because not all octahedral voids are occupied by Fe, due to which a part of Fe 2+ has passed into Fe 3+ . The structural deficiency of Fe in pyrrhotite is different: it gives compositions from Fe 0.875 S (Fe 7 S 8) to FeS (the stoichiometric composition of FeS is troilite). Depending on the deficiency of Fe, the parameters and symmetry of the crystal cell change, and at x ~ 0.11 and below (up to 0.2), pyrotine from the hexagonal modification passes into the monoclinic one. The color of pyrrhotite is bronze-yellow with a brown tint; metallic luster. In nature, continuous masses, granular segregations, consisting of germinations of both modifications, are common.
Hardness on a mineralogical scale 3.5-4.5; density 4580-4700 kg/m3. The magnetic properties vary depending on the composition: hexagonal (poor S) pyrrhotites are paramagnetic, monoclinic (rich in S) are ferromagnetic. Separate pyrotine minerals have a special magnetic anisotropy - paramagnetism in one direction and ferromagnetism in the other, perpendicular to the first.
Origin (genesis)
Pyrrhotite is formed from hot solutions with a decrease in the concentration of dissociated S 2- ions.
It is widely distributed in hypogene deposits of copper-nickel ores associated with ultrabasic rocks; also in contact-metasomatic deposits and hydrothermal bodies with copper-polymetallic, sulfide-cassiterite, and other mineralization. In the oxidation zone it passes into pyrite, marcasite and brown iron ore.
Application
Plays an important role in the production of iron sulfate and crocus; as an ore for obtaining iron is less significant than pyrite. It is used in the chemical industry (production of sulfuric acid). Pyrrhotite usually contains impurities of various metals (nickel, copper, cobalt, etc.), which makes it interesting in terms of industrial applications. First, this mineral is an important iron ore. And secondly, some of its varieties are used as nickel ore. It is valued by collectors.
Marcasite
The name comes from the Arabic "marcasitae", which alchemists used to designate sulfur compounds, including pyrite. Another name is "radiant pyrite". Spectropyrite is named for its similarity to pyrite in color and iridescent tint.
Marcasite, like pyrite, is iron sulfide - FeS2, but differs from it in its internal crystalline structure, greater brittleness and lower hardness. Crystallizes in a rhombic crystal system. Marcasite is opaque, has a brassy-yellow color, often with a greenish or grayish tint, occurs in the form of tabular, acicular and spear-shaped crystals, which can form beautiful star-shaped radial-radiant intergrowths; in the form of spherical nodules (ranging in size from the size of a nut to the size of a head), sometimes sintered, kidney-shaped and grape-shaped formations, and crusts. Often replaces organic remains, such as ammonite shells.
Properties
The color of the trait is dark, greenish-gray, metallic luster. Hardness 5-6, brittle, imperfect cleavage. Marcasite is not very stable in surface conditions, over time, especially at high humidity, it decomposes, turning into limonite and releasing sulfuric acid, so it should be stored separately and with extreme care. When struck, marcasite emits sparks and a sulfur smell.
Origin (genesis)
In nature, marcasite is much less common than pyrite. It is observed in hydrothermal, predominantly veined deposits, most often in the form of druses of small crystals in voids, in the form of powders on quartz and calcite, in the form of crusts and sintered forms. In sedimentary rocks, mainly coal-bearing, sandy-clay deposits, marcasite occurs mainly in the form of nodules, pseudomorphs after organic remains, as well as finely dispersed sooty matter. Macroscopically, marcasite is often mistaken for pyrite. In addition to pyrite, marcasite is usually associated with sphalerite, galena, chalcopyrite, quartz, calcite, and others.
Place of Birth
Of the hydrothermal sulfide deposits, Blyavinskoye in the Orenburg region in the South Urals can be noted. Sedimentary deposits include Borovichi coal-bearing deposits of sandy clays (Novgorod region), containing various forms of concretions. The Kurya-Kamensky and Troitsko-Bainovsky deposits of clay deposits on the eastern slope of the Middle Urals (east of Sverdlovsk) are also famous for the variety of forms. Of note are deposits in Bolivia, as well as Clausthal and Freiberg (Westphalia, North Rhine, Germany), where well-formed crystals are found. In the form of concretions or especially beautiful, radially radiant flat lenses in once silty sedimentary rocks (clays, marls and brown coals), marcasite deposits were found in Bohemia (Czech Republic), the Paris Basin (France) and Styria (Austria, samples up to 7 cm). Marcasite is mined at Folkestone, Dover and Tavistock in the UK, in France, and in the US excellent specimens are obtained from Joplin and other locations in the TriState mining region (Missouri, Oklahoma and Kansas).
Application
In the case of large masses, marcasite can be developed for the production of sulfuric acid. Beautiful but fragile collectible material.
Oldgamite
Calcium sulfide, calcium sulfide, CaS - colorless crystals, density 2.58 g/cm3, melting point 2000 °C.
Receipt
Known as the mineral Oldgamite consisting of calcium sulfide with impurities of magnesium, sodium, iron, copper. The crystals are pale brown to dark brown.
Direct synthesis from elements:
The reaction of calcium hydride in hydrogen sulfide:
From calcium carbonate:
Recovery of calcium sulfate:
Physical Properties
White crystals, cubic face-centered lattice of NaCl type (a=0.6008 nm). Decomposes when melted. In the crystal, each S 2- ion is surrounded by an octahedron consisting of six Ca 2+ ions, while each Ca 2+ ion is surrounded by six S 2- ions.
Slightly soluble in cold water, does not form crystalline hydrates. Like many other sulfides, calcium sulfide undergoes hydrolysis in the presence of water and smells like hydrogen sulfide.
Chemical properties
When heated, it decomposes into components:
Completely hydrolyzes in boiling water:
Diluted acids displace hydrogen sulfide from salt:
Concentrated oxidizing acids oxidize hydrogen sulfide:
Hydrogen sulfide is a weak acid and can be displaced from salts even by carbon dioxide:
With an excess of hydrogen sulfide, hydrosulfides are formed:
Like all sulfides, calcium sulfide is oxidized by oxygen:
Application
It is used for the preparation of phosphors, as well as in the leather industry to remove hair from hides, and is also used in the medical industry as a homeopathic remedy.
chemical weathering
Chemical weathering is a combination of various chemical processes that result in further destruction of rocks and a qualitative change in their chemical composition with the formation of new minerals and compounds. The most important chemical weathering factors are water, carbon dioxide and oxygen. Water is an energetic solvent of rocks and minerals.
The reaction that occurs during the roasting of iron sulfide in oxygen:
4FeS + 7O 2 → 2Fe 2 O 3 + 4SO 2
The reaction that occurs during the firing of iron disulfide in oxygen:
4FeS 2 + 11O 2 → 2Fe 2 O 3 + 8SO 2
When pyrite is oxidized under standard conditions, sulfuric acid is formed:
2FeS 2 +7O 2 +H 2 O→2FeSO 4 +H 2 SO 4
When calcium sulfide enters the furnace, the following reactions can occur:
2CaS + 3O 2 → 2CaO + 2SO 2
CaO + SO 2 + 0.5O 2 → CaSO 4
with the formation of calcium sulfate as the final product.
When calcium sulfide reacts with carbon dioxide and water, calcium carbonate and hydrogen sulfide are formed:
A 5-second activation of pyrite leads to a noticeable increase in the exotherm area, a decrease in the temperature range of oxidation, and a greater mass loss upon heating. Increasing the treatment time in the furnace up to 30 s causes stronger transformations of pyrite. The configuration of the DTA and the direction of the TG curves noticeably change, and the temperature ranges of oxidation continue to decrease. A break appears on the differential heating curve, corresponding to a temperature of 345 ºС, which is associated with the oxidation of iron sulfates and elemental sulfur, which are the products of the oxidation of the mineral. The type of DTA and TG curves of a mineral sample treated for 5 min in an oven differs significantly from the previous ones. The new clearly pronounced exothermic effect on the differential heating curve with a temperature of about 305 º C should be attributed to the oxidation of neoplasms in the temperature range of 255 - 350 º C. The fact that the fraction obtained as a result of 5-minute activation is a mixture of phases.
| Iron(II) sulfide | |
| Iron(II)-sulfide-unit-cell-3D-balls.png | |
| General | |
|---|---|
| Systematic Name |
Iron(II) sulfide |
| Chem. formula | FeS |
| Physical Properties | |
| State | solid |
| Molar mass | 87.910 g/mol |
| Density | 4.84 g/cm³ |
| Thermal properties | |
| T. melt. | 1194°C |
| Classification | |
| Reg. CAS number | 1317-37-9 |
| SMILES | |
| Data is based on standard conditions (25 °C, 100 kPa) unless otherwise noted. | |
Description and structure
Receipt
The reaction begins when a mixture of iron and sulfur is heated in a burner flame, then it can proceed without heating, with the release of heat.
Chemical properties
1. Interaction with concentrated HCl:
2. Interaction with concentrated HNO 3:
Application
Iron(II) sulfide is a common starting material in the production of hydrogen sulfide in the laboratory. Iron hydrosulfide and/or its corresponding basic salt is an essential component of some therapeutic muds.
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Notes
Literature
- Lidin R. A. “Handbook of a student. Chemistry "M.: Astrel, 2003.
- Nekrasov B.V. Fundamentals of General Chemistry. - 3rd edition. - Moscow: Chemistry, 1973. - T. 2. - S. 363. - 688 p.
Links
An excerpt characterizing Iron(II) sulfide
She stopped again. No one interrupted her silence.- Woe is our common, and we will divide everything in half. Everything that is mine is yours,” she said, looking around at the faces that stood before her.
All eyes looked at her with the same expression, the meaning of which she could not understand. Whether it was curiosity, devotion, gratitude, or fear and distrust, the expression on all faces was the same.
“Many are pleased with your grace, only we don’t have to take the master’s bread,” said a voice from behind.
- Yes, why? - said the princess.
No one answered, and Princess Mary, looking around the crowd, noticed that now all the eyes she met immediately dropped.
- Why don't you want to? she asked again.
Nobody answered.
Princess Marya felt heavy from this silence; she tried to catch someone's gaze.
- Why don't you speak? - the princess turned to the old old man, who, leaning on a stick, stood in front of her. Tell me if you think you need anything else. I'll do anything," she said, catching his eye. But he, as if angry at this, lowered his head completely and said:
- Why agree, we do not need bread.
- Well, should we quit everything? Do not agree. Disagree... There is no our consent. We pity you, but there is no our consent. Go on your own, alone…” was heard in the crowd from different directions. And again the same expression appeared on all the faces of this crowd, and now it was probably no longer an expression of curiosity and gratitude, but an expression of embittered determination.
“Yes, you didn’t understand, right,” said Princess Marya with a sad smile. Why don't you want to go? I promise to accommodate you, feed you. And here the enemy will ruin you ...
But her voice was drowned out by the voices of the crowd.
- There is no our consent, let them ruin! We do not take your bread, there is no our consent!
Princess Mary tried again to catch someone's gaze from the crowd, but not a single glance was directed at her; her eyes obviously avoided her. She felt strange and uncomfortable.
“Look, she taught me cleverly, follow her to the fortress!” Ruin the houses and into bondage and go. How! I'll give you bread! voices were heard in the crowd.
Princess Mary, lowering her head, left the circle and went into the house. Having repeated the order to Dron that there should be horses for departure tomorrow, she went to her room and was left alone with her thoughts.
For a long time that night, Princess Marya sat by the open window in her room, listening to the sounds of peasants talking from the village, but she did not think about them. She felt that no matter how much she thought about them, she could not understand them. She kept thinking about one thing - about her grief, which now, after the break made by worries about the present, has already become past for her. She could now remember, she could cry and she could pray. As the sun went down, the wind died down. The night was calm and cool. At twelve o'clock the voices began to subside, a rooster crowed, the full moon began to emerge from behind the linden trees, a fresh, white dew mist rose, and silence reigned over the village and over the house.
Iron(II) sulfide is an inorganic substance with the chemical formula FeS.
Brief description of iron (II) sulfide:
Iron(II) sulfide- an inorganic substance of brown-black color with a metallic luster, a compound of iron and sulfur, a salt of iron and hydrosulfide acid.
Iron(II) sulfide is brown-black crystals.
Chemical formula of iron(II) sulfide FeS.
Does not dissolve in water. Not attracted by a magnet. Refractory.
Decomposes on heating in vacuum.
When wet, it is sensitive to atmospheric oxygen, tk. reacts with oxygen to form iron(II) sulfite.
Physical properties of iron (II) sulfide:
| Parameter name: | Meaning: |
| Chemical formula | FeS |
| Synonyms and names in a foreign language | iron(II) sulfide |
| Substance type | inorganic |
| Appearance | brown-black hexagonal crystals |
| Color | brown-black |
| Taste | —* |
| Smell | without smell |
| Aggregate state (at 20 °C and atmospheric pressure 1 atm.) | solid |
| Density (state of matter - solid, at 20 ° C), kg / m 3 | 4840 |
| Density (state of matter - solid, at 20 ° C), g / cm 3 | 4,84 |
| Boiling point, °C | — |
| Melting point, °C | 1194 |
| Molar mass, g/mol | 87,91 |
* Note:
- no data.
Obtaining iron (II) sulfide:
Iron(II) sulfide is obtained as a result of the following chemical reactions:
- 1.interactions of iron and sulfur:
Fe + S → FeS (t = 600-950 o C).
The reaction proceeds by fusing aluminum with carbon in an arc furnace.
- 2.interactions of iron oxide and hydrogen sulfide:
FeO + H 2 S → FeS + H 2 O (t = 500 o C).
- 3. interactions of ferric chloride and sodium sulfide:
FeCl 2 + Na 2 S → FeS + 2NaCl.
- 4. interactions of ferrous sulfate and sodium sulfide:
FeSO 4 + Na 2 S → FeS + Na 2 SO 4.
Chemical properties of iron (II) sulfide. Chemical reactions of iron (II) sulfide:
The chemical properties of iron (II) sulfide are similar to those of other sulfides. metals. Therefore, it is characterized by the following chemical reactions:
1.reaction of iron(II) sulfide and silicon:
Si + FeS → SiS + Fe (t = 1200 o C).
silicon sulfide and iron.
2.reaction of iron(II) sulfide and oxygen:
FeS + 2O 2 → FeSO 4.
As a result of the reaction, iron (II) sulfate is formed. The reaction proceeds slowly. The reaction uses wet iron sulfide. Impurities are also formed: sulfur S, iron oxide polyhydrate (III) Fe 2 O 3 nH 2 O.
3.reaction of iron (II) sulfide, oxygen and water:
4FeS + O 2 + 10H 2 O → 4Fe(OH) 3 + 4H 2 S.
As a result of the reaction, iron hydroxide and hydrogen sulfide.
4.reaction of iron (II) sulfide, calcium oxide and carbon:
FeS + CaO + C → Fe + CO + CaS (tо).
As a result of the reaction, iron, carbon monoxide and calcium sulfide.
5.reaction of iron(II) sulfide and copper sulfide:
CuS + FeS → CuFeS 2 .
As a result of the reaction, dithioferrate (II) is formed copper(II) (chalcopyrite).
6.reactions of iron (II) sulfide with acids:
Iron(II) sulfide reacts with strong mineral acids.
7. the reaction of thermal decomposition of iron (II) sulfide:
FeS → Fe + S (t = 700 o C).
As a result of the reaction of thermal decomposition of iron (II) sulfide, iron and sulfur. The reaction takes place in