IRON(+2)SULFIDE
Ferrous sulfide
CAS: 1317-37-9
Molecular Formula: FeS
IRON(+2)SULFIDE - Names and Identifiers
| Name | Ferrous sulfide |
| Synonyms | pyrrhotite IRON SULFIDE FERROUS SULFIDE Ferrous sulfide IRON(+2)SULFIDE IRON MONOSULFIDE FERROUS SULPHIDE IRON(II) SULFIDE Iron (II) sulfide IRON(II) SULPHIDE |
| CAS | 1317-37-9 |
| EINECS | 215-268-6 |
| InChI | InChI=1/Fe.S/rFeS/c1-2 |
IRON(+2)SULFIDE - Physico-chemical Properties
| Molecular Formula | FeS |
| Molar Mass | 87.91 |
| Density | 4.84g/mLat 25°C(lit.) |
| Melting Point | 1195 °C |
| Boling Point | decomposes [HAW93] |
| Water Solubility | Soluble in water(0.0062g/L ), in acids with evolution of hydrogen sulfide. Insoluble in nitric acid. |
| Vapor Presure | 0Pa at 25℃ |
| Appearance | Black powder |
| Specific Gravity | 4.84 |
| Color | Grayish-black |
| Odor | Odorless |
| Solubility Product Constant(Ksp) | pKsp: 17.2 |
| Merck | 14,4058 |
| Storage Condition | no restrictions. |
| Stability | Stable. Incompatible with strong acids, strong bases, metal oxides. Avoid moisture. |
| Sensitive | Moisture Sensitive |
| MDL | MFCD00011013 |
| Physical and Chemical Properties | Melting Point: 1195 density: 4.84 |
| Use | Used as an analytical reagent |
IRON(+2)SULFIDE - Risk and Safety
| Hazard Symbols | N - Dangerous for the environment |
| Risk Codes | R31 - Contact with acids liberates toxic gas R50 - Very Toxic to aquatic organisms |
| Safety Description | S60 - This material and its container must be disposed of as hazardous waste. S61 - Avoid release to the environment. Refer to special instructions / safety data sheets. S50 - Do not mix with ... |
| UN IDs | UN 3077 9/PG 3 |
| WGK Germany | 3 |
| FLUKA BRAND F CODES | 13 |
| TSCA | Yes |
| HS Code | 28309011 |
| Hazard Class | 4.1 |
| Packing Group | III |
IRON(+2)SULFIDE - Nature
Open Data Verified Data
The Pure product is colorless hexagonal crystal, and the general commodity is dark brown or gray-black flake or granular. Melting point 1194 C; d 4.84. In the humid air gradually oxidized and decomposed into sulfur and iron oxide. Soluble in acid can release hydrogen sulfide gas. Insoluble in water. Contact with acid or acid gas can produce toxic gases. By high heat decomposition of toxic gases. Flammable, irritating.
Last Update：2024-01-02 23:10:35
IRON(+2)SULFIDE - Preparation Method
Open Data Verified Data
pure reduced iron powder and sublimed sulfur powder were proportionally mixed and placed in a high vacuum closed quartz tube. After heating at 1000 ° C. And completion of the reaction, a brittle gray flash pure ferrous sulfide was obtained.
Last Update：2022-01-01 09:02:07
IRON(+2)SULFIDE - Introduction
Sensitive to humidity. Oxidation to sulfur and ferric oxide in humid air. Dissolved in acids to decompose hydrogen sulfide, almost insoluble in water. It's irritating.
Last Update：2022-10-16 17:13:20
IRON(+2)SULFIDE - Use
Open Data Verified Data
Analytical reagents. Preparation of hydrogen sulfide and other sulfides.
Last Update：2022-01-01 09:02:07
IRON(+2)SULFIDE - Safety
Open Data Verified Data
belongs to low toxicity class, with stimulating effect. Ingestion may cause gastrointestinal irritation. Long-term inhalation of the dust may cause changes in pneumoconiosis. Staff should be protected. If the skin and eyes are touched, they should be immediately rinsed with flowing water. The working environment should have good ventilation conditions. The substance should be stored in a cool, ventilated warehouse. It should be stored separately from oxidants, acids and edible chemical raw materials.
Last Update：2022-01-01 09:02:07
IRON(+2)SULFIDE - Reference Information
| EPA chemical information | Information provided by: ofmpub.epa.gov (external link) |
| Iron sulfide compound | Ferrous sulfide is a compound formed by two elements of sulfur and iron. It is dark brown or black block-like crystals or particles. The bulk has a metallic luster. The relative density is 4.74 and the melting point is 1193~1199 ℃. Insoluble in ammonia, insoluble in water, soluble in dilute acid, releasing toxic hydrogen sulfide gas. In humid air, it is gradually oxidized to ferric oxide and sulfur. In its crystal structure, the sulfur atoms are hexagonal close-packed, the iron atoms are surrounded by 6 sulfur atoms at the apex angle, forming an octahedral structure, and the sulfur atoms are in 6 at the apex angle of the tripartite prism. The iron atoms are surrounded. The coordination number of iron and sulfur atoms is 6, and the atomic number ratio is 1:1. Ferrous sulfide can be obtained by adding alkali metal sulfide to the divalent iron salt. Industrial iron filings and sulfur powder are mixed and prepared by high temperature reaction in a high vacuum quartz sealed tube. In the laboratory, it is mainly used to prepare hydrogen sulfide gas and use it as an analytical reagent. It is used in industry to make ceramics, paints and pigments. It is also used to make other ferrous salts. At high temperatures, ferrous sulfide can be oxidized to iron oxides or sulfates by oxygen or ozone; it can be reduced to elemental iron by carbon or metallic manganese. Ferrous sulfide dissolves in oxidizing acid to form ferric salt and sulfur, sulfur dioxide or sulfuric acid; dissolves in non-oxidizing acid to form divalent iron salt and hydrogen sulfide. |
| Chemical reaction | At high temperatures, ferrous sulfide can be oxidized by oxygen or ozone to iron oxides or sulfates; it can be reduced by carbon or metallic manganese To elemental iron. Ferrous sulfide dissolves in oxidizing acid to form ferric salt and sulfur, sulfur dioxide or sulfuric acid; dissolves in non-oxidizing acid to form divalent iron salt and hydrogen sulfide. 4FeS 6HNO3 6H2SO4 = 2Fe 2(SO4)3 3N2O3 4S ↓ 9H2OFeS 6HNO3 = Fe(NO)3 H2SO4 3NO 2H2O2FeS 10H2SO4 (concentrated) = Fe2(SO4)3 9SO2 10H2OFeS + H2SO4 (dilute) = FeSO4 H2SFeS 2HCl = FeCl2 H2S ferrous sulfide reacts with salts or oxides as follows: |
| preparation method | ferrous sulfide is obtained by eutectic (1000 ℃) of iron and sulfur in a high vacuum quartz sealed pipe or by adding soluble sulfide to neutral or alkaline ferrous salt solution. |
| eggs should not be cooked for a long time | eggs are rich in nutrition. cooking eggs is the simplest and best way to maintain their nutrition. however, it is necessary to master the temperature and time if the eggs are cooked properly, both hardness and hardness are moderate and not raw. If the egg is boiled for too long, the ferrous ions in the egg yolk will combine with the sulfur ions in the protein to form a substance called ferrous sulfide, which is difficult to be absorbed and utilized by the human body, thereby reducing The nutritional value of eggs. Therefore, it is not appropriate to boil eggs for too long. The best way is to put the eggs in a pot with cold water and boil them for another 5 minutes. |
| Use | Used as analytical reagent Laboratory preparation of hydrogen sulfide, ceramic industry. |
| toxic substance data | information provided by: pubchem.ncbi.nlm.nih.gov (external link) |
Last Update：2024-04-10 22:29:15
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