`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 determine the type of reaction represented by the equation:

\[ \text{Pb}_3\text{O}_4 + \text{HCl (dil.)} \xrightarrow{\text{warm}} \text{PbCl}_2 + \text{Cl}_2 + \text{H}_2\text{O} \]

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

### Step 1: Determine the oxidation states of lead in Pb3O4
Let the oxidation state of lead (Pb) be \( x \).

In the compound \( \text{Pb}_3\text{O}_4 \):
- The oxidation state of oxygen (O) is -2.
- The equation for the oxidation states is:
\[ 3x + 4(-2) = 0 \]
\[ 3x - 8 = 0 \]
\[ 3x = 8 \quad \Rightarrow \quad x = \frac{8}{3} \]
Thus, the oxidation state of lead in \( \text{Pb}_3\text{O}_4 \) is \( +\frac{8}{3} \).

### Step 2: Determine the oxidation states in the products
In the product \( \text{PbCl}_2 \):
- The oxidation state of chlorine (Cl) is -1.
- The oxidation state of lead (Pb) is:
\[ x + 2(-1) = 0 \quad \Rightarrow \quad x - 2 = 0 \quad \Rightarrow \quad x = +2 \]

In \( \text{Cl}_2 \):
- The oxidation state of chlorine is 0 (elemental state).

In \( \text{H}_2\text{O} \):
- The oxidation state of hydrogen (H) is +1 and oxygen is -2.

### Step 3: Analyze the changes in oxidation states
- Lead changes from \( +\frac{8}{3} \) in \( \text{Pb}_3\text{O}_4 \) to \( +2 \) in \( \text{PbCl}_2 \). This indicates a decrease in oxidation state, which means lead is being reduced.
- Chlorine changes from -1 in \( \text{HCl} \) to 0 in \( \text{Cl}_2 \), indicating an increase in oxidation state, which means chlorine is being oxidized.

### Step 4: Identify the type of reaction
Since one species (lead) is being reduced (decrease in oxidation state) and another species (chlorine) is being oxidized (increase in oxidation state), this reaction is classified as a redox reaction.

### Conclusion
The type of reaction depicted here is a **redox reaction**. More specifically, it is an **intermolecular redox reaction** because it involves two different reactant molecules leading to oxidation and reduction.

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