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Sulfur dioxide (SO₂) is a colorless, toxic gas with a sharp, pungent odor reminiscent of burning matches. It is highly soluble in water, forming sulfurous acid (H₂SO₃), and is both naturally occurring and human-generated.

Chemically, sulfur dioxide consists of one sulfur atom covalently bonded to two oxygen atoms, with a molecular weight of approximately 64.07 g/mol. It has a melting point of -72.7°C and a boiling point of -10°C, making it a gas under standard conditions. SO₂ is denser than air, with a gas density of about 2.93 g/L at 0°C and 1 atm, and is easily liquefied under pressure or at low temperatures. It is stable when dry but becomes corrosive in the presence of moisture.

Industrially, sulfur dioxide is crucial for the production of sulfuric acid, one of the most widely produced chemicals globally. It is also used as a bleaching agent in paper and textile manufacturing, a preservative in food and beverages (notably in winemaking and dried fruits), a disinfectant, and a reducing agent in various chemical processes. In metallurgy, SO₂ is used in ore processing and metal extraction.

References

1. National Aeronautics and Space Administration (NASA). NW-2011-10-093-GSFC. Sulfur Dioxide Poster (Oct 2011)
2. Wikipedia. Sulfur Dioxide (edited on May 22, 2025)
3. Chemical Book. CAS Database List: Sulfur Dioxide (updated on Jan 27, 2025)
4. Black Ling (Jun 9, 2025). Sulfur Dioxide: Properties, Uses, and Environmental Impact. ALTOMERGE
5. cK-12 (acccessed Jul 17, 2025). What are the physical properties of sulphur dioxide?
6. American Chemical Society (Aug 28, 2023). Molecule of the Week Archive: Sulfur Dioxide