`MnO_(4)^(-)+H^(+)+Br^(-) to Mn^(3+)(aq.)+Br_(2)uarr`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To determine the nature of the reaction given by the equation:

\[ \text{MnO}_4^{-} + \text{H}^{+} + \text{Br}^{-} \rightarrow \text{Mn}^{3+} + \text{Br}_2 \]

we will analyze the oxidation states of the reactants and products.

### Step-by-Step Solution:

1. **Identify the Oxidation States:**
- For \(\text{MnO}_4^{-}\):
- Manganese (Mn) has an oxidation state of +7 (since the overall charge is -1 and each oxygen is -2).
- For \(\text{Br}^{-}\):
- Bromine (Br) has an oxidation state of -1.
- For \(\text{Mn}^{3+}\):
- Manganese (Mn) has an oxidation state of +3.
- For \(\text{Br}_2\):
- Bromine (Br) in its elemental form has an oxidation state of 0.

2. **Determine Changes in Oxidation States:**
- Manganese changes from +7 in \(\text{MnO}_4^{-}\) to +3 in \(\text{Mn}^{3+}\). This is a reduction (decrease in oxidation state).
- Bromine changes from -1 in \(\text{Br}^{-}\) to 0 in \(\text{Br}_2\). This is an oxidation (increase in oxidation state).

3. **Classify the Reaction:**
- Since one species (Mn) is being reduced and another species (Br) is being oxidized, this reaction is classified as a **redox reaction** (oxidation-reduction reaction).

4. **Check for Other Types of Reactions:**
- **Disproportionation Reaction:** This would require a species to be oxidized and reduced simultaneously. This is not the case here.
- **Comproportionation Reaction:** This involves two different oxidation states of the same element reacting to form a third state. This does not apply here either.
- **Thermal Reaction:** This would involve heat, which is not relevant in this context.

5. **Conclusion:**
- The reaction is a redox reaction where \(\text{MnO}_4^{-}\) is reduced to \(\text{Mn}^{3+}\) and \(\text{Br}^{-}\) is oxidized to \(\text{Br}_2\).

### Final Answer:
The nature of the reaction is a **redox reaction**.

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