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Question
Identify disproportionation reaction
Options
\[\ce{CH4 + 2O2 -> CO2 + 2H2O}\]
\[\ce{CH4 + 4Cl2 -> CCl4 + 4HCl}\]
\[\ce{2F2 + 2OH- -> 2F- + OF2 + H2O}\]
\[\ce{2NO2 + 2OH- -> NO^{-}2 + NO^{-}3 + H2O}\]
Solution
\[\ce{2NO2 + 2OH- -> NO^{-}2 + NO^{-}3 + H2O}\]
Explanation:
Disproportionate reactions are defined as the reactions in which the same substance is oxidized as well as reduced. Here, the below reaction is given as-
\[\ce{2NO2 + 2OH- -> NO^{-}2 + NO^{-}3 + H2O}\]
In this reaction, N is both oxidized as well as reduced since O.N. of N increases from +4 in \[\ce{NO^{-}3}\] to +5 in \[\ce{NO2}\] and decreases from +4 in \[\ce{NO}\] to +3 in \[\ce{NO^{-}2}\].
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