`PbO_(2)+HCl(dil.) overset(warm) to PbCl_(2)darr+Cl_(2)uarr+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 determine the type of reaction represented by the equation:

\[ \text{PbO}_2 + \text{HCl (dil.)} \overset{\text{warm}}{\rightarrow} \text{PbCl}_2 + \text{Cl}_2 + \text{H}_2\text{O} \]

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

### Step 1: Identify the oxidation states of the elements in the reactants and products.

- In **PbO₂**:
- Lead (Pb) has an oxidation state of +4 (since O is -2 and there are 2 O atoms, total -4; thus, Pb must be +4 to balance).

- In **HCl**:
- Hydrogen (H) has an oxidation state of +1 and Chlorine (Cl) has -1.

- In **PbCl₂**:
- Lead (Pb) has an oxidation state of +2 (since Cl is -1 and there are 2 Cl atoms, total -2; thus, Pb must be +2 to balance).

- In **Cl₂**:
- Chlorine (Cl) has an oxidation state of 0 (elemental state).

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

### Step 2: Determine the changes in oxidation states.

- Lead (Pb) changes from +4 in PbO₂ to +2 in PbCl₂. This indicates a **reduction** (gain of electrons).
- Chlorine (Cl) changes from -1 in HCl to 0 in Cl₂. This indicates an **oxidation** (loss of electrons).

### Step 3: Classify the reaction.

Since one species (lead) is being reduced while another species (chlorine) is being oxidized, this reaction qualifies as a **redox reaction** (reduction-oxidation reaction).

### Step 4: Identify the type of redox reaction.

This specific reaction can be classified as an **intermolecular redox reaction** because it involves two different reactant molecules (PbO₂ and HCl) participating in the electron transfer process.

### Conclusion:

The reaction is classified as an **intermolecular redox reaction**.

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