(a) (i) write an equation for the reaction in which sulphur (iv) oxide gas is prepared. (ii) why is it necessary to keep the gases pure and dry? (iii) write an equation for the reaction that takes place in the converter. (iv) describe the process that takes place in chamber g. (v) name two major gases that escape into the environment.

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# Brief Explanations:
- (i) Lead sulphate ($PbSO_4$) reacts with air ($O_2$) to produce sulphur (IV) oxide ($SO_2$). The chemical equation is based on the principle of conservation of mass.
- (ii) Impurities can act as catalysts poisons and moisture can cause corrosion and unwanted side - reactions in the subsequent processes.
- (iii) In the converter, sulphur (IV) oxide ($SO_2$) reacts with oxygen ($O_2$) to form sulphur (VI) oxide ($SO_3$).
- (iv) Chamber G is likely involved in the absorption of sulphur (VI) oxide ($SO_3$) to form sulphuric acid ($H_2SO_4$).
- (v) After the reactions, unreacted gases like oxygen ($O_2$) and nitrogen ($N_2$) (from the air) escape.

# Answer:
- (i) $2PbSO_4+O_2
ightarrow 2PbO + 2SO_2$
- (ii) Impurities may poison the catalyst and moisture can cause corrosion and unwanted side - reactions.
- (iii) $2SO_2+O_2
ightleftharpoons 2SO_3$
- (iv) Sulphur (VI) oxide ($SO_3$) is absorbed (e.g., in a suitable liquid like concentrated sulphuric acid) to form sulphuric acid ($H_2SO_4$).
- (v) Oxygen ($O_2$) and nitrogen ($N_2$)

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