Write a balanced chemical equation to represent decomposition of lead nitrate onheating. What are brown fumes due to?

Balanced Chemical Equation for Decomposition of Lead Nitrate

When lead(II) nitrate $(\text{Pb(NO}_3\text{)}_2)$ is heated, it decomposes into lead(II) oxide $(\text{PbO})$, nitrogen dioxide $(\text{NO}_2)$, and oxygen gas $(\text{O}_2)$. The balanced chemical equation for this reaction is:

$2 \text{Pb(NO}_3\text{)}_2 \rightarrow 2 \text{PbO} + 4 \text{NO}_2 + \text{O}_2$

Explanation of Brown Fumes

The brown fumes observed during the decomposition of lead(II) nitrate are primarily due to the formation of nitrogen dioxide ($\text{NO}_2$). Nitrogen dioxide is a reddish-brown gas, which is a characteristic feature of the decomposition process. It indicates the presence of nitrogen oxides, which are formed when the nitrate ions decompose upon heating. The reaction not only produces solid lead(II) oxide but also generates these hazardous gases, emphasizing the need for caution when conducting this reaction in a laboratory setting.