Question

In the disproportionation reaction ${3 \, HClO_3 -> HClO_4 + Cl_2 + 2 O_2 + H_2O}$ the equivalent mass of the oxidising agent is (molar mass of ${HClO_3 = 84.45}$)

• A. 16.89
• B. 32.22
• C. 84.45
• D. 28.15

Answer 1

Answer: (A)

16.89

Answer 2

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