In the disproportionation reaction 3HClO3 xrightarrowHClO4+Cl2+2O2+H2O, the equivalent mass of the oxidizing agent is (molar mass of HClO3=84.45 )

Question

In the disproportionation reaction 3HClO3 xrightarrowHClO4+Cl2+2O2+H2O, the equivalent mass of the oxidizing agent is (molar mass of HClO3=84.45 ) (A) 16.89 (B) 32.22 (C) 84.45 (D) 28.15

Tardigrade Admin · Accepted Answer

This is a disproportionation reaction since here the oxidation state of chlorine decreases from +5 to 0 in

C l_{2}

as well as increases from +5 to +7 in

H Cl O_{4}

. Thus,

H Cl O_{3}

acts as oxidizing as well as reducing agent. Equivalent mass of oxidizing agent (i.e.,

H Cl O_{3}

)

= \frac{m o l a r ma ss}{C han g e in o x i d a t i o n n u mb er}

= \frac{84.45}{( 5 - 0 )} = 16.89

Q. In the disproportionation reaction
$3 H Cl O_{3} H Cl O_{4} + C l_{2} + 2 O_{2} + H_{2} O,$
the equivalent mass of the oxidizing agent is (molar mass of $H Cl O_{3} = 84.45$ )

16.89

32.22

84.45

28.15

29.7