Question

In the following reaction:
\[ \text{MnO}_4^{-} \xrightarrow{\text{H}^+} \text{MnO}_2 + \text{MnO}_4^{2-} \] Mangante ion undergoes disproportionation in acidic medium to form:

• A. \(\text{MnO}_2, \text{MnO}_4^{2-}\)
• B. \(\text{MnO}_4, \text{MnO}_2\)
• C. \(\text{MnO}_2, \text{Mn}_2\text{O}_3\)
• D. \(\text{MnO}_4, \text{MnO}\)

Hint:

In acidic medium, the manganate ion (\(\text{MnO}_4^{-}\)) disproportionates into manganese dioxide (\(\text{MnO}_2\)) and manganese tetraoxide (\(\text{MnO}_4^{2-}\)).

Answer 1

The Correct Option is A

Step 1: Understanding the reaction.
The manganate ion \(\text{MnO}_4^{-}\) undergoes a disproportionation reaction in acidic medium, meaning it breaks into two different species: \(\text{MnO}_2\) and \(\text{MnO}_4^{2-}\).
Step 2: Conclusion.
The correct answer is (1) \(\text{MnO}_2, \text{MnO}_4^{2-}\) as per the given reaction sequence.