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)