On heating lead nitrate forms oxides of nitrogen and lead. The oxides formed are :

Options

A. 1. `N_(2)O, PbO`
B. 2. `NO_(2), PbO`
C. 3. `NO, PbO`
D. 4. `NO, PbO_(2)`

Answer

To solve the question regarding the decomposition of lead nitrate upon heating, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Compound**: The compound in question is lead nitrate, which is represented by the chemical formula \( \text{Pb(NO}_3\text{)}_2 \).

2. **Understand the Decomposition Reaction**: When lead nitrate is heated, it undergoes thermal decomposition. This means it breaks down into simpler substances.

3. **Write the Decomposition Reaction**: The decomposition of lead nitrate can be represented by the following chemical equation:
\[ \text{2 Pb(NO}_3\text{)}_2 \rightarrow \text{2 PbO} + \text{4 NO}_2 + \text{O}_2 \]
Here, lead nitrate decomposes to form lead oxide (\( \text{PbO} \)), nitrogen dioxide (\( \text{NO}_2 \)), and oxygen (\( \text{O}_2 \)).

4. **Balance the Reaction**: To ensure that the equation is balanced, we check the number of atoms of each element on both sides of the equation:
- **Left Side**: 2 Pb, 8 N, 12 O (from 2 Pb(NO3)2)
- **Right Side**: 2 Pb (from 2 PbO), 4 N (from 4 NO2), 2 O (from O2) + 8 O (from 4 NO2) = 10 O
- The equation is balanced as there are equal numbers of each type of atom on both sides.

5. **Identify the Products**: From the balanced equation, the products formed are:
- Lead oxide (\( \text{PbO} \))
- Nitrogen dioxide (\( \text{NO}_2 \))
- Oxygen (\( \text{O}_2 \))

6. **Select the Correct Answer**: Based on the products formed, the correct answer to the question is that the oxides formed are \( \text{PbO} \) and \( \text{NO}_2 \).

### Final Answer:
The oxides formed upon heating lead nitrate are \( \text{PbO} \) (lead oxide) and \( \text{NO}_2 \) (nitrogen dioxide).

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