`Pb(NO_(3))_(2) overset(Delta)to PbO+NO_(2)+O_(2)`

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 question regarding the reaction of lead(II) nitrate decomposing into lead(II) oxide, nitrogen dioxide, and oxygen, we will analyze the reaction step by step.

### Step-by-Step Solution:

1. **Identify the Reaction Type**:
The given reaction is:
\[ \text{Pb(NO}_3\text{)}_2 \overset{\Delta}{\rightarrow} \text{PbO} + \text{NO}_2 + \text{O}_2 \]
This indicates that lead(II) nitrate is breaking down into lead(II) oxide, nitrogen dioxide, and oxygen gas.

2. **Understanding Decomposition Reaction**:
A decomposition reaction is characterized by a single compound breaking down into two or more products. In this case, lead(II) nitrate (Pb(NO3)2) is decomposing into three different products.

3. **Thermal Decomposition**:
The reaction occurs upon heating (indicated by the Δ symbol). This suggests that thermal energy is required to break the bonds in lead(II) nitrate, leading to the formation of the products.

4. **Redox Process**:
During the decomposition, oxidation and reduction processes occur. Lead(II) nitrate decomposes, where lead is reduced to lead(II) oxide, and nitrogen in the nitrate is oxidized to nitrogen dioxide. Oxygen is released as a byproduct.

5. **Conclusion**:
Since the reaction involves the breakdown of a single compound into multiple products due to heat, it is classified as a **thermal decomposition redox reaction**.

### Final Answer:
The reaction \( \text{Pb(NO}_3\text{)}_2 \overset{\Delta}{\rightarrow} \text{PbO} + \text{NO}_2 + \text{O}_2 \) is a **thermal decomposition redox reaction**.

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