Sulfur Cycle
Sulfur Cycle
- Number of oxidation states
- -2(sulfhydryl, R-SH, and sulfide, HS–), 0(elemental sulfur, S0), and +6(sulfate,SO42-) are significant in nature
- Primarily gypsum (CaSO4) and sulfide minerals (pyrite, FeS2) constitute bulk of Earth’s S
- Significant amount of SO2 gas enters the sulfur cycle from human activities
- Primarily burning fossil fuels
Hydrogen Sulfide and Sulfate Reaction
- H2S major volatile sulfur gas
- SO42-+ 4H2 → H2S + 2H2O + 2OH–
- H2S exist below pH-7
- Nonvolatile HS– and S2- exist above pH-7
- In marine sediments rate of sulfate reduction is carbon limited and can be greatly increased by an influx of organic matter
- Hydrogen sulfide is toxic to plants and animals
- Sulfur is detoxified in nature by binding with iron for FeS.
Sulfide and Elemental Sulfur Oxidation-Reduction
- Under oxic conditions sulfide oxidizes at neutral pH
- Sulfur-oxidizing chemolithotrophic bacteria(aerobes) can catalyze oxidation of sulfide
- Microbial sulfide oxidation is significant only in areas where H2S emerges from anoxic environments and meets air
- Elemental Sulfur is chemically stable but is readily oxidized by sulfur-oxidizing chemolithotrophic bacteria.
- S0 is insoluble
- Bacteria that oxidize must attach to S0 crystals to obtain their substrate
- S0 forms sulfuric acid and thus S0 oxidation characteristically lowers the pH in the environment
- Reduction of S0 to sulfide(anaerobic respiration) is major ecological process
- Organic forms of sulfur
- Dimethyl sulfide