Hydrogen sulfide

Hydrogen sulfide
Skeletal formula of hydrogen sulfide with two dimensions
Ball-and-stick model of hydrogen sulfide
Ball-and-stick model of hydrogen sulfide
Spacefill model of hydrogen sulfide
Spacefill model of hydrogen sulfide
  Sulfur, S
  Hydrogen, H
Names
Systematic IUPAC name
Hydrogen sulfide[1]
Other names
  • Dihydrogen monosulfide
  • Sour gas
  • Dihydrogen sulfide
  • Sewer gas
  • Egg gas
  • Sulfane
  • Sulfurated hydrogen
  • Sulfureted hydrogen
  • Sulfuretted hydrogen
  • Sulfur hydride
  • Hydrosulfuric acid
  • Hydrothionic acid
  • Thiohydroxic acid
  • Sulfhydric acid
Identifiers
3D model (JSmol)
3DMet
3535004
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.029.070 Edit this at Wikidata
EC Number
  • 231-977-3
303
KEGG
MeSH Hydrogen+sulfide
RTECS number
  • MX1225000
UNII
UN number 1053
  • InChI=1S/H2S/h1H2 checkY
    Key: RWSOTUBLDIXVET-UHFFFAOYSA-N checkY
  • InChI=1/H2S/h1H2
    Key: RWSOTUBLDIXVET-UHFFFAOYAJ
  • S
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
1.000644 (0 °C)[2]
Structure
C2v
Bent
0.97 D
Thermochemistry
1.003 J K−1 g−1
206 J mol−1 K−1[7]
−21 kJ mol−1[7]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Flammable and highly toxic
GHS labelling:
GHS02: FlammableGHS06: ToxicGHS09: Environmental hazard
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)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
4
4
0
Flash point −82.4 °C (−116.3 °F; 190.8 K)[10]
232 °C (450 °F; 505 K)
Explosive limits 4.3–46%
Lethal dose or concentration (LD, LC):
  • 713 ppm (rat, 1 hr)
  • 673 ppm (mouse, 1 hr)
  • 634 ppm (mouse, 1 hr)
  • 444 ppm (rat, 4 hr)[9]
  • 600 ppm (human, 30 min)
  • 800 ppm (human, 5 min)[9]
NIOSH (US health exposure limits):
PEL (Permissible)
C 20 ppm; 50 ppm [10-minute maximum peak][8]
REL (Recommended)
C 10 ppm (15 mg/m3) [10-minute][8]
IDLH (Immediate danger)
100 ppm[8]
Related compounds
Related hydrogen chalcogenides
Related compounds
Phosphine
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Hydrogen sulfide is a chemical compound with the formula H2S. 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] Swedish chemist Carl Wilhelm Scheele is credited with having discovered the chemical composition of purified hydrogen sulfide in 1777.[12]

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, 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.

  1. ^ "Hydrogen Sulfide - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information.
  2. ^ a b Patnaik, Pradyot (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 978-0-07-049439-8.
  3. ^ a b William M. Haynes (2016). CRC Handbook of Chemistry and Physics (97th ed.). Boca Raton: CRC Press. pp. 4–87. ISBN 978-1-4987-5429-3.
  4. ^ "Hydrogen sulfide". pubchem.ncbi.nlm.nih.gov.
  5. ^ Perrin, D.D. (1982). Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution (2nd ed.). Oxford: Pergamon Press.
  6. ^ Bruckenstein, S.; Kolthoff, I.M., in Kolthoff, I.M.; Elving, P.J. Treatise on Analytical Chemistry, Vol. 1, pt. 1; Wiley, NY, 1959, pp. 432–433.
  7. ^ a b Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
  8. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0337". National Institute for Occupational Safety and Health (NIOSH).
  9. ^ a b "Hydrogen sulfide". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  10. ^ "Hydrogen sulfide". npi.gov.au.
  11. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  12. ^ Smith, Roger P. (2010). "A Short History of Hydrogen Sulfide". American Scientist. 98 (1): 6. doi:10.1511/2010.82.6.
  13. ^ Shackelford, R. E.; Li, Y.; Ghali, G. E.; Kevil, C. G. (2021). "Bad Smells and Broken DNA: A Tale of Sulfur-Nucleic Acid Cooperation". Antioxidants. 10 (11): 1820. doi:10.3390/antiox10111820. PMC 8614844. PMID 34829691.
  14. ^ Reiffenstein, R. J.; Hulbert, W. C.; Roth, S. H. (1992). "Toxicology of Hydrogen Sulfide". Annual Review of Pharmacology and Toxicology. 32: 109–134. doi:10.1146/annurev.pa.32.040192.000545. PMID 1605565.
  15. ^ Bos, E. M; Van Goor, H; Joles, J. A; Whiteman, M; Leuvenink, H. G (2015). "Hydrogen sulfide: Physiological properties and therapeutic potential in ischaemia". British Journal of Pharmacology. 172 (6): 1479–1493. doi:10.1111/bph.12869. PMC 4369258. PMID 25091411.