Which of the following is an example of comproportionation reaction?

P b (s) + P b O_{2} (s) + 2 H_{2} S O_{4} (a q) \to 2 P b S O_{4} (s) + 2 H_{2} O (l)

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15 S e + S e C l_{4} + 4 A l C l_{3} \to 2 S e_{8} [A l C l_{4}]_{2}

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2 H_{2} S (g) + S O_{2} (g) \to 2 S (s) + 2 H_{2} O (g)

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2 A g^{2 +} (a q) + A g (s) \to 2 A g^{+} (a q)

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Solution

The correct options are
A $2 H_{2} S (g) + S O_{2} (g) \to 2 S (s) + 2 H_{2} O (g)$
B $2 A g^{2 +} (a q) + A g (s) \to 2 A g^{+} (a q)$
C $15 S e + S e C l_{4} + 4 A l C l_{3} \to 2 S e_{8} [A l C l_{4}]_{2}$
D $P b (s) + P b O_{2} (s) + 2 H_{2} S O_{4} (a q) \to 2 P b S O_{4} (s) + 2 H_{2} O (l)$
A reaction in which an element in a higher oxidation state reacts with the same element in a lower oxidation state to give the element in an intermediate oxidation state is known as comproportionation or symproportionation.
The reactions of options (A), (B), (C) and (D) are examples of comproportionation or symproportionation reaction.
$P b (s) + P b O_{2} (s) + 2 H_{2} S O_{4} (a q) \to 2 P b S O_{4} (s) + 2 H_{2} O (l)$
$15 S e + S e C l_{4} + 4 A l C l_{3} \to 2 S e_{8} [A l C l_{4}]_{2}$
$2 H_{2} S (g) + S O_{2} (g) \to 2 S (s) + 2 H_{2} O (g)$
$2 A g^{2 +} (a q) + A g (s) \to 2 A g^{+} (a q)$

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Similar questions

15 S e

S e C l_{4}

4 A l C l_{3}

\to

2 S e_{8}

A l C l_{4}

_{2}

Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions:

(a) 2AgBr (s) + C₆H₆O₂(aq) → 2Ag(s) + 2HBr (aq) + C₆H₄O₂(aq)

(b) HCHO(l) + 2[Ag (NH₃)₂]⁺(aq) + 3OH^–(aq) → 2Ag(s) + HCOO^–(aq) + 4NH₃(aq) + 2H₂O(l)

(d) N₂H₄(l) + 2H₂O₂(l) → N₂(g) + 4H₂O(l)

(e) Pb(s) + PbO₂(s) + 2H₂SO₄(aq) → 2PbSO₄(s) + 2H₂O(l)

P b

P b (s)

P b O_{2} (s)

2 H_{2} S O_{4} (a q)

\to

2 P b S O_{4} (s)

2 H_{2} O (l)

P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4 (a q)} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)}

A g^{2 +} (a q) + A g (s) \to 2 A g^{+} (a q)

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