Question

The products obtained from a reaction of hydrogen peroxide and acidified potassium permanganate are

• A. \(Mn^{4+}, H_2O \;only\)
• B. \(Mn^{2+}, H_2O \;only\)
• C. \(Mn^{4+}, H_2O, O_2 \;only\)
• D. \(Mn^{2+}, H_2O, O_2 \;only\)

Answer 1

The Correct Option is D

The reaction of hydrogen peroxide (\(H_2O_2\)) with acidified potassium permanganate (\(KMnO_4\)) is a redox reaction where \(H_2O_2\) acts as a reducing agent, and \(KMnO_4\) is reduced in an acidic medium. Let's solve this problem step-by-step by understanding the chemical reaction and identifying the products.

Step 1: Understand the Reaction

In acidic conditions, the balanced redox reaction between hydrogen peroxide and potassium permanganate is:

\(2 KMnO_4 + 3 H_2SO_4 + 5 H_2O_2 \rightarrow 2 MnSO_4 + K_2SO_4 + 5 O_2 + 8 H_2O\)

In this reaction:

• Potassium permanganate (\(KMnO_4\)) is reduced to manganese(II) sulfate (\(MnSO_4\)), where manganese goes from a +7 oxidation state to a +2 oxidation state.
• Hydrogen peroxide (\(H_2O_2\)) is oxidized to oxygen gas (\(O_2\)).

Step 2: Identify the Products

From the balanced reaction, the products formed are:

• \(Mn^{2+}\) ions (from \(MnSO_4\))
• Water (\(H_2O\))
• Oxygen gas (\(O_2\))

Step 3: Conclusion

Thus, the correct answer is \(Mn^{2+}, H_2O, O_2 \;only\). Therefore, the option \(Mn^{2+}, H_2O, O_2 \;only\) is correct.

Other options can be ruled out based on the oxidation state changes and the products that could form in this acidic redox reaction.