Describe the manufacture of H₂SO₄ by contact process.

2

(a)

Write the conditions to maximise the yield of sulphuric acid by Contact process.

2

(a)

Complete the following chemical reaction equations:
(i) I₂ + HNO₃ (conc.) \(\rightarrow\)
(ii) HgCl₂ PH₃ \(\rightarrow\)

2

(a)

How would you account for the following?
(i) Hydrogen fluoride is much less volatile than hydrogen chloride.
(ii) Interhalogen compounds are strong oxidising agents>

2

(a)

Assign a reason for each of the following:
(i) In group 15 the bond angle H-M-H decreases in the following order NH₃ (107.8^o), PH₃ (93.6^o), AsH₃ (91.8^o).
(ii) Sulphur hexafluoride is used as a gaseous electrical insulator.

2

(a)

Complete the following reaction equations:
(i) Ca(OCI)₂ + HCI \(\to\)
(ii) Ca₃(PO₄)₂ + SiO₂ + C \(\rightarrow\)

\(\)

2

(a)

Complete the following chemical reaction equations:
(i) Xe(g) + F₂(g)\(\underset { (in\ excess) }{ F_{2}(g) } \) \(\xrightarrow [7 bar]{873\ K}\)
(ii) Li + N₂  \(\rightarrow\)

2

(a)

Write the structures of the following:
(i) BrF₃ (ii) XeF₄

2

(a)

Complete the following equations:
(i) C + conc. H₂SO₄\(\longrightarrow \)
(ii) \(XeF_{ 2 }+H_{ 2 }O\rightarrow \)

2

(a)

Why is nitric oxide paramagnetic in gaseous state but the solid obtained on cooling it is diamagnetic?

2

(a)

Name three oxoacids of nitrogen.  Write the disproportionation reaction of that oxoacid of nitrogen in which nitrogen is in +3 oxidation state.

2

(a)

Nitric acid forms an oxide of nitrogen on reaction with P₄O₁₀.  Write the reaction involved. Also wirte the resonating structure of the oxide of nitrogen formed.

2

(a)

Give an example to show the effect of concentration of nitric acid on the formation of oxidation product.

2

(a)