question_answer

In the disproportionation reaction \[3HCl{{O}_{3}}\xrightarrow{{}}HCl{{O}_{4}}+C{{l}_{2}}+2{{O}_{2}}+{{H}_{2}}O,\]the equivalent mass of the oxidizing agent is (molar mass of \[HCl{{O}_{3}}=84.45\])

A)  16.89                   

B)         32.22

C)  84.45                   

D)         28.15

E)  29.7

Correct Answer: A

Solution :

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\[HCl{{O}_{4}}\]. Thus, \[HCl{{O}_{3}}\]acts as oxidizing as well as reducing agent. Equivalent mass of oxidizing agent (i.e.,\[HCl{{O}_{3}}\]) \[=\frac{molar\,mass}{Change\,in\,oxidation\,number}\] \[=\frac{84.45}{(5-0)}=16.89\]