In the disproportionation reaction, 3HClO3 → HClO4 + Cl2 + 2O2 + H2O, the equivalent mass of the oxidising agent is(molar mass of HClO3 = 84.45)

2HCl+5O3→HCl+7O4+Cl20+2O2+H2OHere HClO3 reduces to Cl2, So it acts as an oxidizing agent.EHClO3(as oxident)=Mchange in ox.state=84.455=16.89

In the disproportionation reaction, 3HClO3 → HClO4 + Cl2 + 2O2 + H2O, the equivalent mass of the oxidising agent is(molar mass of HClO3 = 84.45)

2HCl+5O3→HCl+7O4+Cl20+2O2+H2OHere HClO3 reduces to Cl2, So it acts as an oxidizing agent.EHClO3(as oxident)=Mchange in ox.state=84.455=16.89

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In the disproportionation reaction, 3HClO₃ → HClO₄ + Cl₂ + 2O₂ + H₂O, the equivalent mass of the oxidising agent is
(molar mass of HClO₃ = 84.45)

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16.89

32.22

84.45

28.15

answer is A.

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$2 H \overset{+ 5}{Cl} O_{3} \to H \overset{+ 7}{Cl} O_{4} + \overset{0}{{Cl}_{2}} + 2 O_{2} + H_{2} O$

Here HClO₃ reduces to Cl₂, So it acts as an oxidizing agent.

$E_{{HClO}_{3}} (as oxident) = \frac{M}{change in ox . state} = \frac{84.45}{5} = 16.89$

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In the disproportionation reaction, 3HClO3 → HClO4 + Cl2 + 2O2 + H2O, the equivalent mass of the oxidising agent is(molar mass of HClO3 = 84.45)

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In the disproportionation reaction, 3HClO₃ → HClO₄ + Cl₂ + 2O₂ + H₂O, the equivalent mass of the oxidising agent is
(molar mass of HClO₃ = 84.45)