`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 solve the reaction \( \text{MnO}_2 + \text{NaCl} + \text{H}_2\text{SO}_4 \text{(Conc.)} \rightarrow \text{MnSO}_4 + \text{Cl}_2 \), we will analyze the oxidation states of each element involved in the reaction.

### Step 1: Assign Oxidation States
1. **Manganese in \( \text{MnO}_2 \)**:
- Oxygen has an oxidation state of -2.
- Since there are 2 oxygen atoms, the total contribution from oxygen is \( 2 \times (-2) = -4 \).
- Let the oxidation state of manganese be \( x \).
- Therefore, \( x - 4 = 0 \) (since the compound is neutral).
- Thus, \( x = +4 \).

2. **Sodium in \( \text{NaCl} \)**:
- Sodium has an oxidation state of +1.
- Chlorine has an oxidation state of -1.

3. **Hydrogen in \( \text{H}_2\text{SO}_4 \)**:
- Each hydrogen has an oxidation state of +1.
- Sulfur has an oxidation state of +6 (calculated as follows: \( 2(+1) + x + 4(-2) = 0 \) leads to \( x = +6 \)).
- Each oxygen has an oxidation state of -2.

4. **Manganese in \( \text{MnSO}_4 \)**:
- The sulfate ion \( \text{SO}_4^{2-} \) has a charge of -2.
- Therefore, manganese must have an oxidation state of +2 to balance the charge.

5. **Chlorine in \( \text{Cl}_2 \)**:
- In its elemental form, chlorine has an oxidation state of 0.

### Step 2: Identify Changes in Oxidation States
- Manganese changes from +4 in \( \text{MnO}_2 \) to +2 in \( \text{MnSO}_4 \). This is a reduction (gain of electrons).
- Chlorine changes from -1 in \( \text{NaCl} \) to 0 in \( \text{Cl}_2 \). This is an oxidation (loss of electrons).

### Step 3: Classify the Reaction
- Since there is both oxidation (of chlorine) and reduction (of manganese) occurring simultaneously, this reaction is classified as a **redox reaction**.
- It is specifically an **intermolecular redox reaction** because it involves multiple reactants.

### Step 4: Eliminate Other Reaction Types
- This is not a disproportionation reaction, as no single species is both oxidized and reduced.
- It is not a comproportionation reaction, as there is no single species present in two different oxidation states.
- It is also not a thermal reaction, as heat is not being applied.

### Conclusion
The correct classification for the reaction \( \text{MnO}_2 + \text{NaCl} + \text{H}_2\text{SO}_4 \text{(Conc.)} \rightarrow \text{MnSO}_4 + \text{Cl}_2 \) is that it is an **intermolecular redox reaction**.

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