Sulphur and its Compounds

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Presentation transcript:

Sulphur and its Compounds Chapter 42

General properties Group VIA (1s22s22p63s23p4) m.p. 113oC, b.p. 445oC Allotropes: (1) Rhombic sulphur, S8 (room to 96oC) (2) Monoclinic sulphur, S8 (stable btn. 96-119oC) (3) Plastic sulphur, long polymeric chains.

Range of sulphur compounds Chemical formulae Oxidation state S2-, H2S -2 S8 SCl2, S2O32- +2 SO2, SO32-, H2SO3 +4 SO3, SO42-, H2SO4 +6

Burning of sulphur Sulphur burns with a dull blue flame to form sulphur dioxide, trace of misty sulphur trioxide are also formed. S + O2  SO2

Sulphur dioxide A colourless gas with choking smell An acidic gaseous pollutant Readily liquefied under pressure Very soluble in water and reacts to form sulphuric(IV) acid Can be further oxidized to SO3, which dissolves in water to form sulphuric(VI) acid, H2SO4

Oxidizing properties of SO2 2Mg + SO2  2MgO + S 2H2S + SO2  2H2O + 3S Aqueous SO2  SO32-(aq) 2MnO4- + 5SO32- + 6H+  2Mn2+ + 5SO42- + 3H2O Cr2O72- + 3SO32- + 8H+  2Cr3+ + 3SO42- + 4H2O

Oxidizing properties of SO2 Br2+ SO32- + H2O  2Br- + SO42- + 2H+ Dye + SO32- + H2O  Dye-O + SO42- + 2H+

Sulphuric(VI) Acid Contact Process S + O2  SO2 (or 4FeS2 + 11O2  2Fe2O3 + 8SO2) 2SO2 + O2  2SO3 (450oC, V2O5 as catalyst) SO3 + H2SO4  H2S2O7 (then H2S2O7 + H2O  2H2SO4)

A flow diagram Catalytic chamber Heat exchanger drySO2+air SO3 Purifier and drier Air Heat exchanger Catalytic chamber Absorption tower Sulphur burner H2SO4 store water 98% H2SO4 c.H2SO4 oleum drySO2+air SO3

Chemical properties of H2SO4 Dilute H2SO4, a typical acid Zn + H2SO4  ZnSO4 + H2 2NaOH + H2SO4  Na2SO4 + H2O CuO + H2SO4  CuSO4 + H2O MgCO3 + H2SO4  MgSO4 + H2O + CO2 2NaHCO3 + H2SO4  Na2SO4 + H2O + CO2

Chemical properties of H2SO4 Concentrated H2SO4 As an oxidizing agent Cu + 2H2SO4  CuSO4 + SO2 + 2H2O C + 2H2SO4  CO2 + 2SO2 + 2H2O As a dehydrating agent Reaction with HX 2HBr + H2SO4  Br2 + SO2 + 2H2O 8HI + 2H2SO4  4I2 + H2S + 4H2O

Uses of sulphuric(VI) acid Manufacture of detergents, dyestuffs, polymers, fibres, paints, fertilizers

Test for sulphate(VI) ions Can be tested by adding a solution of BaCl2 acidified with dil. HNO3 Ba2+ + SO42-  BaSO4, a white ppt. Note: Ba2+ +CO32-  BaCO3 Ba2+ +SO32-  BaSO3 BaCO3 + 2HNO3  Ba(NO3)2 + H2O + CO2 BaSO3 + 2HNO3  Ba(NO3)2 + H2O + SO2