Reaction of chlorine with hot/cold solution of hydroxide When chlorine reacts with cold solution of say potasium hydroxide, the disproportionation goes to lower oxidation states:

$\ce{Cl2 + 2 KOH -&gt; KCl + KClO + H2O} $ 

Whilst with hot solution the oxidation state of chlorine goes up to $+V$:

$\ce{3 Cl2 + 6 KOH -&gt; KClO3 + 5 KCl + 3 H2O} $ 

Why is that? Does the heat make the oxidation to higher ox. states easier?
The chlorate ($\ce{ClO3-}$) is formed by disproportionation of hypochlorite and hypochlorous acid:

$$\ce{ClO- + 2 HClO -&gt; ClO3- + 2 HCl}$$

Higher temperature promotes the formation of hypochlorous acid through hydrolysis of hypochlorite and therefore speeds up the reaction.