`MnO_(2)+NaCl+H_(2)SO_(4)(Conc.) to MnSO_(4)+Cl_(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 type of reaction represented by the equation:

\[ \text{MnO}_2 + \text{NaCl} + \text{H}_2\text{SO}_4 \text{(Conc.)} \rightarrow \text{MnSO}_4 + \text{Cl}_2 \uparrow \]

we will analyze the oxidation states of the elements involved in the reaction.

### Step-by-Step Solution:

1. **Identify the oxidation states of reactants:**
- In \( \text{MnO}_2 \), manganese (Mn) has an oxidation state of +4.
- In \( \text{NaCl} \), chlorine (Cl) has an oxidation state of -1.
- In \( \text{H}_2\text{SO}_4 \), sulfur (S) has an oxidation state of +6.

2. **Identify the oxidation states of products:**
- In \( \text{MnSO}_4 \), manganese (Mn) has an oxidation state of +2.
- In \( \text{Cl}_2 \), chlorine (Cl) has an oxidation state of 0.

3. **Determine changes in oxidation states:**
- Manganese is reduced from +4 in \( \text{MnO}_2 \) to +2 in \( \text{MnSO}_4 \) (reduction).
- Chlorine is oxidized from -1 in \( \text{NaCl} \) to 0 in \( \text{Cl}_2 \) (oxidation).

4. **Identify the type of reaction:**
- Since there is simultaneous oxidation and reduction occurring in different compounds, this reaction is classified as an **intermolecular redox reaction**.

5. **Eliminate other options:**
- The reaction does not involve thermal conditions (no temperature indicated), so it cannot be a thermal combination or thermal decomposition redox reaction.
- There is no indication that the reaction involves the same species undergoing both oxidation and reduction (which would indicate a disproportionation or comproportionation reaction).

### Conclusion:
The type of reaction is an **intermolecular redox reaction**.

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