1 / 13

Sulphur and its Compounds

Sulphur and its Compounds. Chapter 42. General properties. Group VIA (1s 2 2s 2 2p 6 3s 2 3p 4 ) m.p. 113 o C, b.p. 445 o C Allotropes: (1) Rhombic sulphur, S 8 (room to 96 o C) (2) Monoclinic sulphur, S 8 (stable btn. 96-119 o C) (3) Plastic sulphur, long polymeric chains.

thyra
Download Presentation

Sulphur and its Compounds

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Sulphur and its Compounds Chapter 42

  2. 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.

  3. Range of sulphur compounds

  4. 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

  5. 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

  6. 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

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

  8. 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)

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

  10. 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

  11. 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

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

  13. 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

More Related