Which of the following is an example of disproportionation redox reaction?

Question

Which of the following is an example of disproportionation redox reaction? (A) N2(g)+ O 2(g) arrow 2 NO (g) (B) 2 H 2(g)+ O 2(g) arrow 2 H 2 O (l) (C) 2 Pb ( NO 3)2(s) arrow 2 PbO (s)+4 NO 2(g)+ O 2(g) (D) NaH (s)+ H 2 O (l) arrow NaOH (a q)+ H 2(g)

Tardigrade Admin · Accepted Answer

Disproportionation redox reaction involves simultaneous oxidation and reduction of atoms of same element from one oxidation state to two different oxidation states.

2 N O_{2} + 4 (g) + 2 O H^{-} \to N O_{2}^{-} + 3 + N O_{3}^{-} + 5 + H_{2} O

In this reaction,

N

of nitrogen dioxide is of

+ 4

oxidation state but after the reaction,

N

is present in

+ 3

and

+ 5

oxidation state simultaneously. So, this reaction is an example of disproportionation redox reaction.

Q. Which of the following is an example of disproportionation redox reaction?

$N_{2} (g) + O_{2} (g) \to 2 NO (g)$

$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$

$2 P b (N O_{3})_{2} (s) \to 2 P b O (s) + 4 N O_{2} (g) + O_{2} (g)$

$N a H (s) + H_{2} O (l) \to N a O H (a q) + H_{2} (g)$

$2 N O_{2} (g) + 2 O H^{-} \to NO 2^{-} (a q) + N O_{3}^{-} (a q) + H_{2} O (l)$

Q. Which of the following is an example of disproportionation redox reaction?

N2​(g)+O2​(g)→2NO(g)

2H2​(g)+O2​(g)→2H2​O(l)

2Pb(NO3​)2​(s)→2PbO(s)+4NO2​(g)+O2​(g)

NaH(s)+H2​O(l)→NaOH(aq)+H2​(g)

2NO2​(g)+2OH−→NO2−(aq)+NO3−​(aq)+H2​O(l)

$N_{2} (g) + O_{2} (g) \to 2 NO (g)$

$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$

$2 P b (N O_{3})_{2} (s) \to 2 P b O (s) + 4 N O_{2} (g) + O_{2} (g)$

$N a H (s) + H_{2} O (l) \to N a O H (a q) + H_{2} (g)$

$2 N O_{2} (g) + 2 O H^{-} \to NO 2^{-} (a q) + N O_{3}^{-} (a q) + H_{2} O (l)$