question_answer

\[{{\text{H}}_{\text{2}}}{{\text{O}}_{\text{2}}}\]oxidizes \[\text{Mn}{{\text{O}}_{\text{2}}}\]is \[\text{MnO}_{4}^{-}\]in basic  medium, \[{{\text{H}}_{\text{2}}}{{\text{O}}_{\text{2}}}\]and \[\text{Mn}{{\text{O}}_{\text{2}}}\]react in the molar ratio of

A) 1 : 1     

B)                        2 : 1       

C)        2 : 3       

D)        3 : 2

Correct Answer: D

Solution :

(Oxidation number two O atoms taken) On balancing of oxidation number                 \[3{{H}_{2}}{{O}_{2}}+2Mn{{O}_{2}}\xrightarrow{{}}2MnO_{4}^{-}+6{{H}_{2}}O\] Thus,   \[{{H}_{2}}{{O}_{2}}:Mn{{O}_{2}}=3:2\]