`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 solve the given question regarding the reaction:

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

we will follow these steps:

### Step 1: Identify Oxidation States
First, we need to determine the oxidation states of all the elements involved in the reaction.

- For \(\text{MnO}_4^{-}\):
- Let the oxidation state of Mn be \(X\).
- The oxidation state of O is \(-2\).
- Therefore, the equation becomes:
\[ X + 4(-2) = -1 \implies X - 8 = -1 \implies X = +7 \]

- For \(\text{H}^{+}\):
- The oxidation state is \(+1\).

- For \(\text{Br}^{-}\):
- The oxidation state is \(-1\).

- For \(\text{Mn}^{3+}\):
- The oxidation state is \(+3\).

- For \(\text{Br}_2\):
- The oxidation state is \(0\) (as it is in its elemental form).

### Step 2: Determine Changes in Oxidation States
Next, we analyze the changes in oxidation states:

- Manganese changes from \(+7\) in \(\text{MnO}_4^{-}\) to \(+3\) in \(\text{Mn}^{3+}\). This is a reduction (gain of electrons).

- Bromine changes from \(-1\) in \(\text{Br}^{-}\) to \(0\) in \(\text{Br}_2\). This is an oxidation (loss of electrons).

### Step 3: Classify the Reaction
Since we have both oxidation and reduction occurring simultaneously, this reaction is classified as a redox reaction.

### Step 4: Identify the Type of Redox Reaction
In this case, the reaction is an intermolecular redox reaction because it involves different species (MnO4- and Br-). It is not a disproportionation reaction (where a single species undergoes both oxidation and reduction) or a comproportionation reaction (where a single species is present in two different oxidation states).

### Conclusion
Thus, the correct classification of the reaction is that it is an intermolecular redox reaction.

### Final Answer
The answer to the question is that the reaction is an **intermolecular redox reaction**.

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