Which of the followings is not a intramolecular redox reaction?

N H_{4} N O_{2} \to N_{2} + 2 H_{2} O

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N H_{4} N O_{3} \to N_{2} O + 2 H_{2} O

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2 K C l O_{3} \to 2 K C l + 3 O_{2}

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2 H_{2} O_{2} \to 2 H_{2} O + O_{2}

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Solution

The correct option is D $2 H_{2} O_{2} \to 2 H_{2} O + O_{2}$
Intramolecular redox reactions are the reactions in which one element of a compound is oxidised while the other is reduced.
Disproportionation is a specific type of redox reaction in which a species is simultaneously reduced and oxidised to form two different products.
$H_{2} O_{2} \to H_{2} O + O_{2}$
-1 -2 0
It is a disproportionation reaction and not intramolecular redox reaction .
$N H_{4} N O_{2} \to N_{2} + 2 H_{2} O$
-3 +3 0
$N H_{4} N O_{3} \to N_{2} O + 2 H_{2} O$
-3 +5 +1
$2 K C l O_{3} \to 2 K C l + 3 O_{2}$
+5 -1 0
All these three are intramolecular redox reaction.

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Similar questions

I : {({N H}_{4})}_{2} {C r}_{2} O_{7} ⟶ N_{2} + {C r}_{2} O_{3} + H_{2} O

I I : {N H}_{4} {N O}_{3} ⟶ N_{2} O + 2 H_{2} O

I I I : 2 K C l O_{3} ⟶ 2 K C l + 3 O_{2}

I . N H_{4} N O_{3} Δ \to N_{2} O + 2 H_{2} O

I I . N H_{4} N O_{2} Δ \to N_{2} + 2 H_{2} O

I I I . P C l_{5} Δ \to P C l_{3} + C l_{2}

2 H_{2} O_{2} \to 2 H_{2} O + O_{2}

2 H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}

2 H_{2} O_{2} \to 2 H_{2} O + O_{2}

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