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The important sulfur cycle is a biogeochemical cycle in which the sulfur moves between rocks, waterways and living systems. It is important in geology as it affects many minerals and in life because sulfur is an essential element (), being a constituent of many proteins and cofactors, and sulfur compounds can be used as oxidants or reductants in microbial respiration. [1]
This is an accepted version of this page This is the latest accepted revision, reviewed on 1 February 2025. This article is about the chemical element. For other uses, see Sulfur (disambiguation). Chemical element with atomic number 16 (S) Sulfur, 16 S Sulfur Alternative name Sulphur (pre-1992 British spelling) Allotropes see Allotropes of sulfur Appearance Lemon yellow sintered microcrystals ...
The fractionations of oxygen produced by sulfur disproportionation from elemental sulfur have been found to be higher, with reported values from 8 to 18.4‰, which suggests a kinetic isotope effect in the pathways involved in oxidation of elemental sulfur to sulfate, although more studies are necessary to determine what are the specific steps ...
The H 2 S in the liquid where it reacts with sulfur dioxide (SO 2) to form elemental sulfur and water according to the following chemical equation. 2 H 2 S + SO 2 → 3 S + 2 H 2 O The formed elemental sulfur remains dissolved in the hydrocarbon solution.
Treatment of sulfur with hydrogen gives hydrogen sulfide.When dissolved in water, hydrogen sulfide is mildly acidic: [5] H 2 S ⇌ HS − + H +. Hydrogen sulfide gas and the hydrosulfide anion are extremely toxic to mammals, due to their inhibition of the oxygen-carrying capacity of hemoglobin and certain cytochromes in a manner analogous to cyanide and azide.
Disulfur dichloride is a yellow liquid that fumes in moist air due to reaction with water: 16 S 2 Cl 2 + 16 H 2 O → 8 SO 2 + 32 HCl + 3 S 8. It is produced by partial chlorination of elemental sulfur. The reaction proceeds at usable rates at room temperature. In the laboratory, chlorine gas is led into a flask containing elemental sulfur.
The electron donor for the sulfur-reducing bacterium is acetate, coupled with elemental sulfur reduction to sulfide. The green sulfur bacterium produces H 2 re-oxidizing the H 2 S previously produced, in presence of light. During these cocultures experiments no elemental sulfur appears in the medium because it is immediately reduced. [64]
The Claus reaction is an example of comproportionation reaction (the inverse of disproportionation) involving hydrogen sulfide (H 2 S) and sulfur dioxide (SO 2) to produce elemental sulfur and water as follows: 2 H 2 S + SO 2 → 3 S + 2 H 2 O