Sulfur Dioxide
Industrial sources
- Burning of fuels containing sulfur such as coal and oil - Extraction of metals from ore e.g. metals from sulfide ores
Characteristics
- Colourless gass - Strong suffocating odour - Easily dissolves in water
Burning of fuels containing sulfur contaminants such as coal and oil
S(s)+O2(g) -> SO2(g)
Equation for sulfur dioxide reacting with water to form sulfurous acid
SO2(g)+H2O(l) ⇌H2SO3
Sulfur trioxide can react with water to form sulfuric acid
SO3(g)+H2O(l) -> H2SO4(aq)
Natural Sources
- Volcanic and geothermal hot springs - Natural decay of vegetation on land, in wetlands and in oceans
These can be further oxidise in the atmosphere to form sulfuric acid
2H2SO3(g)+O2(g) -> 2H2SO4(aq)
Extraction of metals from ores
2ZnS(s)+3O2(g) -> 2ZnO(s)+2SO2(g)