When chlorine reacts with cold solution of say potasium hydroxide, the disproportionation goes to lower oxidation states:
$\ce{Cl2 + 2 KOH -> KCl + KClO + H2O} $
Whilst with hot solution the oxidation state of chlorine goes up to $+V$:
$\ce{3 Cl2 + 6 KOH -> KClO3 + 5 KCl + 3 H2O} $
Why is that? Does the heat make the oxidation to higher ox. states easier?
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