Question

Identify disproportionation reaction.

• A. $C{H}_4+2O_2\to C{O}_2+2H_{2}O$
• B. $C{H}_4+4C{l}_2\to CC{l}_4+4HCl$
• C. $2F_2+2O{H}^{-}\to 2F^{-}+O{F}_2+H_{2}O$
• D. $2N{O}_2+2O{H}^{-}\to N{O}_2^{-}+N{O}_3^{-}+H_{2}O$

Answer 1

Answer: (D)

$2N{O}_2+2O{H}^{-}\to N{O}_2^{-}+N{O}_3^{-}+H_{2}O$

Disproportionation reaction is a redox reaction in which a compound of intermediate oxidation state converts to two different compounds, one of higher and one of lower oxidation states

A. $\stackrel{+4}{C}{H}_4+2\stackrel{0}{O_2}\to \stackrel{+4}{C}\stackrel{-2}{O_2}+2H_{2}O$ - Not a disproportionate reaction

B. $\stackrel{+4}{C}{H}_4+4\stackrel{0}{C{l}_2}\to \stackrel{+4}{C}\stackrel{-1}{C{l}_4}+4HCl$- Not a disproportionate reaction

C. $2\stackrel{0}{F_2}+2\stackrel{-2}{O}{H}^{-}\to 2\stackrel{-1}{F^{-}}+\stackrel{+2}{O}\stackrel{-1}{F_2}+H_{2}O$- redox reaction but not disproportionate reaction

D. $2\stackrel{+4}{N}{O}_2+2O{H}^{-}\to \stackrel{+3}{N}{O}_2^{-}+\stackrel{+5}{N}{O}_3^{-}+H_{2}O$- N changes from +4 to +3 and +5 thus its a disproportionate reaction