Sulfur

@@Sources of Sulfur:@@

  • Underground beds; Mexico, Poland and USA
  • Around volcanoes
  • Compound in metal ores; Galena (PbS), Copper pyrites (CuFeS2) and Zinc Blende (ZnS)
  • Occur naturally in fossil fuels

@@Extraction:@@

From oil and Gas

  • Natural gas is mainly methane (contains 30% hydrogen sulfide)
  • H2S Seperated from methane
  • H2S Oxidised/ Reacted with oxygen

2H2S + O2 → 2S + 2H20

Hydrogen sulfide + oxygen → Sulfur + Water

@@Properties of Sulfur:@@

  • Brittle Yellow solid
  • Allotropes; Rhombic sulfur and monoclinic sulfur
  • Low melting point (Molecular)
  • Non-conducting/ Insulator
  • Insoluble
  • Reacts with metals to form sulfides
    • Fe + S → FeS
  • Burns in air to form sulfur dioxide

@@Uses of Sulfur:@@

  • Sulfuric Acid
  • Added to rubber to toughen it (vulcanising)
  • Drugs, pesticides, dyes, matches, paper
  • Cosmetics, shampoos, Body lotion
  • Sulfur concrete (not attacked by acid rain)

@@Properties of Sulfur Dioxide:@@

  • Colorless gas, heavier than air with a strong smell
  • Acidic oxide H2O + SO2 → H2SO3
  • Bleaches when damp (reduces colored compounds)
  • Kills bacteria

@@Uses of Sulfur dioxide:@@

  • Making sulfuric acid
  • Bleach, wool, silk, and wood pulp
  • Food preservative (stops bacterial growth

@@Making sulfuric acid CONTACT PROCESS:@@

Sulfur, air and water

1.Sulfur burned in air

S + O2 → SO2

  1. Sulfur dioxide mixed with more air to form sulfur trioxide

Conditions for contact process: Vanadium oxide as a catalyst at 450C

 2SO2 + O2 → 2SO3

  1. Sulfur trioxide is then dissolved in sulfuric acid to form OLEUM

SO3 + H2SO4 → H2S2O7

  1. Oleum mixed with water to form sulfuric acid

H2S2O7 + H20 → 2H2SO4

@@Uses and properties of sulfuric acid:@@

  • Strong acid
  • Fertilisers
  • Paints, pigments and dyes
  • Fibre and plastics
  • Acid in car batteries
  • Concentrated sulfuric acid can be used as dehydrating agent