State True or False.
The following reaction is a disproportionation reaction.
${N H}_{4} {N O}_{3} Δ - \to N_{2} O + 2 H_{2} O$

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Solution

${N H}_{4}^{+}$ ( $N . O$ of $N = - 3$ ) oxidises to $N_{2}$ ( $O . N$ of $N = + 1$ ).
${N O}_{3}^{-}$ ( $O . N$ of $N = + 5$ ) reduces to $N_{2} O$ .
Hence, it is a redox reaction and not disproportionation.
Hence it is false.

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