Question

Which of the following equation depicts the oxidizing nature of $H _{2} O _{2} ?$

• A. $KIO _{4}+ H _{2} O _{2} \rightarrow KIO _{3}+ H _{2} O + O _{2}$
• B. $2 I ^{-}+ H _{2} O _{2}+2 H ^{+} \rightarrow I _{2}+2 H _{2} O$
• C. $I _{2}+ H _{2} O _{2}+2 OH ^{-} \rightarrow 2 I ^{-}+2 H _{2} O + O _{2}$
• D. $Cl _{2}+ H _{2} O _{2} \rightarrow 2 HCl + O _{2}$

Answer 1

The Correct Option is B

To determine which equation depicts the oxidizing nature of hydrogen peroxide (H_2O_2), we need to identify the reaction in which H_2O_2 acts as an oxidizing agent. An oxidizing agent is a substance that accepts electrons and gets reduced. Here are the steps and rationale:

1. Analyze Option 1: KIO_4 + H_2O_2 \rightarrow KIO_3 + H_2O + O_2
   • In this reaction, H_2O_2 is decomposing to form oxygen, but the main oxidation state changes are involved in the conversion of IO_4^{-} to IO_3^{-}. H_2O_2 is not reducing any element here; it is just decomposing.
2. Analyze Option 2: 2 I^- + H_2O_2 + 2 H^+ \rightarrow I_2 + 2 H_2O
   • Here, H_2O_2 oxidizes iodide ions (I^-) to iodine (I_2). This shows H_2O_2 acting as an oxidizing agent as it accepts electrons from iodide ions.
   • Thus, this reaction correctly depicts the oxidizing nature of H_2O_2.
3. Analyze Option 3: I_2 + H_2O_2 + 2 OH^- \rightarrow 2 I^- + 2 H_2O + O_2
   • In this reaction, H_2O_2 is reducing iodine (I_2) to iodide ions (I^-), which demonstrates its reductive capability, not its oxidizing nature.
4. Analyze Option 4: Cl_2 + H_2O_2 \rightarrow 2 HCl + O_2
   • Here, chlorine gas (Cl_2) is being reduced to hydrochloric acid (HCl), indicating H_2O_2 is acting as a reducing agent.

Based on the above analysis, Option 2 (2 I^- + H_2O_2 + 2 H^+ \rightarrow I_2 + 2 H_2O) is the correct reaction that depicts the oxidizing nature of H_2O_2, as H_2O_2 oxidizes the iodide ions to iodine.