Hydrogen sulfide
Poisonous, corrosive and flammable gas / From Wikipedia, the free encyclopedia
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Hydrogen sulfide is a chemical compound with the formula H
2S. It is a colorless chalcogen-hydride gas, and is poisonous, corrosive, and flammable, with trace amounts in ambient atmosphere having a characteristic foul odor of rotten eggs.[11] The underground mine gas term for foul-smelling hydrogen sulfide-rich gas mixtures is stinkdamp. Swedish chemist Carl Wilhelm Scheele is credited with having discovered the chemical composition of purified hydrogen sulfide in 1777.[12] The British English spelling of this compound is hydrogen sulphide, a spelling no longer recommended by the Royal Society of Chemistry or the International Union of Pure and Applied Chemistry.
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| Names | |||
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| Systematic IUPAC name
Hydrogen sulfide[1] | |||
Other names
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| Identifiers | |||
3D model (JSmol) |
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| 3DMet | |||
| 3535004 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider |
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| ECHA InfoCard | 100.029.070  | ||
| EC Number |
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| 303 | |||
| KEGG |
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| MeSH | Hydrogen+sulfide | ||
PubChem CID |
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| RTECS number |
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| UNII | |||
| UN number | 1053 | ||
CompTox Dashboard (EPA) |
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| Properties | |||
| H2S | |||
| Molar mass | 34.08 g·mol−1 | ||
| Appearance | Colorless gas | ||
| Odor | Foul, pungent, like that of rotten eggs | ||
| Density | 1.539 g.L−1 (0°C)[2] | ||
| Melting point | −85.5[3] °C (−121.9 °F; 187.7 K) | ||
| Boiling point | −59.55[3] °C (−75.19 °F; 213.60 K) | ||
| 3.980 g dm−3 (at 20 °C) [4] | |||
| Vapor pressure | 1740 kPa (at 21 °C) | ||
| Acidity (pKa) | 7.0[5][6] | ||
| Conjugate acid | Sulfonium | ||
| Conjugate base | Bisulfide | ||
| −25.5·10−6 cm3/mol | |||
Refractive index (nD) |
1.000644 (0 °C)[2] | ||
| Structure | |||
| C2v | |||
| Bent | |||
| 0.97 D | |||
| Thermochemistry | |||
Heat capacity (C) |
1.003 J K−1 g−1 | ||
Std molar entropy (S⦵298) |
206 J mol−1 K−1[7] | ||
Std enthalpy of formation (ΔfH⦵298) |
−21 kJ mol−1[7] | ||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards |
Flammable and highly toxic | ||
| GHS labelling: | |||
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| Danger | |||
| H220, H330, H400 | |||
| P210, P260, P271, P273, P284, P304+P340, P310, P320, P377, P381, P391, P403, P403+P233, P405, P501 | |||
| NFPA 704 (fire diamond) | |||
| Flash point | −82.4 °C (−116.3 °F; 190.8 K)[8] | ||
| 232 °C (450 °F; 505 K) | |||
| Explosive limits | 4.3–46% | ||
| Lethal dose or concentration (LD, LC): | |||
LC50 (median concentration) |
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LCLo (lowest published) |
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| NIOSH (US health exposure limits): | |||
PEL (Permissible) |
C 20 ppm; 50 ppm [10-minute maximum peak][10] | ||
REL (Recommended) |
C 10 ppm (15 mg/m3) [10-minute][10] | ||
IDLH (Immediate danger) |
100 ppm[10] | ||
| Related compounds | |||
Related hydrogen chalcogenides |
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Related compounds |
Phosphine | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Hydrogen sulfide is toxic to humans and most other animals by inhibiting cellular respiration in a manner similar to hydrogen cyanide. When it is inhaled or its salts are ingested in high amounts,[clarification needed] damage to organs occurs rapidly with symptoms ranging from breathing difficulties to convulsions and death.[13][14] Despite this, the human body produces small amounts of this sulfide and its mineral salts, and uses it as a signalling molecule.[15]
Hydrogen sulfide is often produced from the microbial breakdown of organic matter in the absence of oxygen, such as in swamps and sewers; this process is commonly known as anaerobic digestion, which is done by sulfate-reducing microorganisms. It also occurs in volcanic gases, natural gas deposits, and sometimes in well-drawn water.