1. Tardigrade
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  3. Chemistry
  4. In the disproportionation reaction 3 HClO3 arrow HClO4 + Cl2 + 2 O2 + H2O the equivalent mass of the oxidising agent is (molar mass of HClO3 = 84.45)

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Q. In the disproportionation reaction $3 \, HClO_3 \rightarrow HClO_4 + Cl_2 + 2 O_2 + H_2O$ the equivalent mass of the oxidising agent is (molar mass of $HClO_3 = 84.45$)

Redox Reactions

Solution:

$ClO^{-}_3 \rightarrow Cl_2^{0}$;
In $ClO^{-}_3 = x - 6 = - 1$ or $x = + 5$
Eq. mass of $ClO^{-}_3 $
$ = \frac{\text{Mol. mass of } ClO^{-}_3}{\text{Oxidation number change}} = \frac{84.45}{5} = 16.89$