(a) Outline the procedures for the treatment of water for town supply.
(b) (i) State two main impurities present in bauxite.
(ii) Give one reason why bauxite is usually preferred as the ore for the extraction of aluminium.
(iii) Outline the manufacture of aluminium form purified bauxite.
(c) (i) Explain briefly the term fine chemical industry.
(ii) State two differences between a fine chemical and a heavy chemical.
(d) (i) Write a balanced chemical equation for the combustion of coal.
(ii) If 5.4 g of coal is burnt completely, calculate the amount of oxygen measured at s.t.p. that would be required for the combustion.
[C = 12.0, O = 16.0, Molar volume of a gas at s.t.p. = 22.4 dm\(^3\)]
(e) Name two substances which can be used as electrodes during the electrolysis of acidified water.
(a)
- addition of alum / addition of coagulating agent
- sedimentation
- filtration
- disinfection / chlorination / addition of chlorine
(b) (i) - iron (III) oxide
- silicon (IV) oxide / sand
- trioxosilicates (IV)
(ii) because aluminium oxide has too high a melting point to eletrolyse on its own / bauxite has low silica content
(iii) - Alumina and molten cryolite
(c) (i) A fine chemical industry is the one that manufactures chemicals in smaller
quantities / amounts for specific use with high level of purity
(ii)
| Fine chemical |
Heavy chemical |
|
- they are produced in |
- they are produced in larger |
|
- they are highly pure |
- they are not pure |
|
- they are final products |
- they are intermediate products |
|
- they are more costly / |
- less costly / less expensive |
(d) (i) C\(_{(s)}\) + O\(_{2(g)}\)
(ii) Amount of coal burnt = \(\frac{5.4}{12}\) mol\(^{-1}\)
= 0.45mol
From the equation of the reaction moles of O\(_2\) used = moles of C burnt = 0.45
1 moles of O\(_2\) = 22.4 dm\(^3\)
0.45 mol O\(_2\) = 22.4 x 0.45
= 10.1dm\(^3\)
(e) - platinum
- carbon
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