Question

Which of the following equations depict the oxidizing nature of $H_{2}O$?

• A. $2MnO_{4}^{-} + 6H^{+} + 5H_{2}O_{2} \rightarrow 2Mn^{2 +} + 8H_{2}O + 5O_{2}$
• B. $2Fe^{3 +} + 2H^{+} + H_{2}O_{2} \rightarrow 2Fe^{2 +} + H_{2}O + O_{2}$
• C. $2I^{-} + 2H^{+} + H_{2}O_{2} \rightarrow I_{2} + 2H_{2}O$
• D. $KIO_{4} + H_{2}O_{2} \rightarrow KIO_{3} + H_{2}O + O_{2}$

Answer 1

Answer: (C)

$2I^{-} + 2H^{+} + H_{2}O_{2} \rightarrow I_{2} + 2H_{2}O$

Answer 2

: Oxidising nature of $H_{2}O_{2}$means it oxidizes other substance and itself gets reduced. In such reactions $O_{2}$is not evolved.

In (1) $MnO_{4}^{-}$gets reduced from $Mn^{7 +}toMn^{2 +}$

In (2) $Fe^{3 +}$gets reduced to $Fe^{2 +}$

In (3), $I^{-}$gets oxidised to $I_{2}$

In (4), $KIO_{4}$gets reduced from $I^{7 +}toI^{5 +}$