`Pb_(3)O_(4)+HCl (dil.)overset(warm) to PbCl_(2)darr+Cl_(2)+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 analyze the reaction \( \text{Pb}_3\text{O}_4 + \text{HCl (dil.)} \overset{\text{warm}}{\rightarrow} \text{PbCl}_2 + \text{Cl}_2 + \text{H}_2\text{O} \), we will determine the oxidation states of the elements involved and identify the type of reaction.

### Step 1: Determine Oxidation States
1. **Lead in \( \text{Pb}_3\text{O}_4 \)**: Let the oxidation state of lead be \( x \).
- The equation for the oxidation states is:
\[ 3x + 4(-2) = 0 \]
\[ 3x - 8 = 0 \implies 3x = 8 \implies x = \frac{8}{3} \]
- Therefore, the oxidation state of lead in \( \text{Pb}_3\text{O}_4 \) is \( +\frac{8}{3} \).

2. **Oxygen in \( \text{Pb}_3\text{O}_4 \)**: The oxidation state of oxygen is \( -2 \).

3. **Hydrogen in \( \text{HCl} \)**: The oxidation state of hydrogen is \( +1 \).

4. **Chlorine in \( \text{HCl} \)**: The oxidation state of chlorine is \( -1 \).

5. **Lead in \( \text{PbCl}_2 \)**: The oxidation state of lead here is \( +2 \).

6. **Chlorine in \( \text{Cl}_2 \)**: The oxidation state of chlorine is \( 0 \).

7. **Oxygen in \( \text{H}_2\text{O} \)**: The oxidation state of oxygen is \( -2 \).

### Step 2: Analyze Changes in Oxidation States
- **Lead**: Changes from \( +\frac{8}{3} \) to \( +2 \) (Reduction).
- **Chlorine**: Changes from \( -1 \) in \( \text{HCl} \) to \( 0 \) in \( \text{Cl}_2 \) (Oxidation).

### Step 3: Identify the Type of Reaction
- Since one species (lead) is being reduced (gaining electrons) and another species (chlorine) is being oxidized (losing electrons), this reaction is classified as a redox reaction.
- Specifically, since the oxidation and reduction are occurring between two different species, this is an **intermolecular redox reaction**.

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