Bromine reacts with aqueous sodium hydroxide at ${25^ \circ }C$.
reaction 1 $B{r_2}\left( {aq} \right) + 2NaOH\left( {aq} \right) \to NaBr\left( {aq} \right) + NaOBr\left( {aq} \right) + {H_2}O\left( l \right)$
The NaOBr formed is unstable at ${25^ \circ }C$ and reacts further.
reaction 2 $3NaOBr\left( {aq} \right) \to 2NaBr\left( {aq} \right) + NaBr{O_3}\left( {aq} \right)$
Which reactions are disproportionations?
both reaction 1 and reaction 2
2 )
neither reaction 1 nor reaction 2
3 )
reaction 1 only
4 )
reaction 2 only
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