Properties and Compounds of Sulphur
Learn about the general properties, allotropes, compounds, and chemical reactions of sulphur. Explore its burning properties, formation of sulphur dioxide and sulphuric acid, and oxidizing properties. Discover the production process of sulphuric(VI) acid and its chemical properties. Dive into a flow diagram depicting the manufacturing process of sulphuric acid.
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Presentation Transcript
General properties Group VIA (2:8:6) 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 S2-, H2S S8 SCl2, S2O32- SO2, SO32-, H2SO3 SO3, SO42-, H2SO4 Oxidation state -2 0 +2 +4 +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, V2O5as catalyst) SO3+ H2SO4 H2S2O7 (then H2S2O7+ H2O 2H2SO4)
A flow diagram Catalytic chamber Purifier and drier Heat exchanger Sulphur burner Air drySO2+air Purifier and drier water Air SO3 Absorption tower H2SO4store oleum 98% H2SO4 c.H2SO4
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 BaCl2acidified 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
