Aqueous sodium hydroxide, when heated, reacts with chlorine. $6\text{NaOH(aq)} + 3\text{Cl}_2(g) \rightarrow 5\text{NaCl(aq)} + \text{NaClO}_3(aq) + 3\text{H}_2\text{O(l)}$ Which statement is correct?
- AThe oxidation numbers of chlorine and hydrogen both change in the reaction.
- BThe oxidation numbers of chlorine in the products are $-1$ and $+1$.
- CIf the aqueous sodium hydroxide is cold the reaction produces NaClO instead of NaClO$_3$.
- DSodium undergoes disproportionation in this reaction.