`MnO_(2)+2KOH+(1)/(2)O_(2) to K_(2)MnO_(4)+H(2)O`

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 reaction and classify it, we will follow these steps:

### Step 1: Write down the reaction
The reaction provided is:
\[ \text{MnO}_2 + 2 \text{KOH} + \frac{1}{2} \text{O}_2 \rightarrow \text{K}_2\text{MnO}_4 + \text{H}_2\text{O} \]

### Step 2: Determine the oxidation states of each element
1. **For MnO2**:
- Manganese (Mn) has an oxidation state of +4 (since \( X + 2(-2) = 0 \) gives \( X = +4 \)).
- Oxygen (O) has an oxidation state of -2.

2. **For KOH**:
- Potassium (K) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- Hydrogen (H) has an oxidation state of +1.

3. **For O2**:
- Oxygen (O) has an oxidation state of 0 (elemental state).

4. **For K2MnO4**:
- Potassium (K) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- To find Mn, we set up the equation:
\[ 2(+1) + X + 4(-2) = 0 \]
\[ 2 + X - 8 = 0 \]
\[ X = +6 \] (Mn has an oxidation state of +6).

5. **For H2O**:
- Hydrogen (H) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.

### Step 3: Analyze the changes in oxidation states
- **Manganese**: Changes from +4 in MnO2 to +6 in K2MnO4 (oxidation).
- **Oxygen**: Changes from 0 in O2 to -2 in H2O (reduction).

### Step 4: Identify the type of reaction
Since there is a change in oxidation states where Mn is oxidized and O is reduced, this reaction is classified as a **redox reaction** (oxidation-reduction reaction).

### Step 5: Determine if it is a disproportionation or comproportionation reaction
- **Disproportionation**: A single species is both oxidized and reduced. This is not the case here since two different species are involved.
- **Comproportionation**: A single species in two different oxidation states reacts to form a single product. This is also not the case here.

### Conclusion
The reaction is a redox reaction, specifically an intermolecular redox reaction, as different species are involved in oxidation and reduction.

### Final Answer
The correct classification of the reaction is that it is a **redox reaction**.

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