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On heating lead (II) nitrate gives a brown gas " $A$ ". The gas " $A$ " on cooling changes to colourless solid " $B$ ". Solid " $B$ " on heating with NO changes to a blue solid ' $C$. Identify' $A^{\prime}$ ', ' $B$ ' and ' $C^{\prime}$ and also write reactions involved and draw the structures of ' $B^{\prime}$ and ' $C^{\prime}$.
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$\mathrm{Pb}\left(\mathrm{NO}_3\right)_2$ on heating produces a brown coloured gas which may be $\mathrm{NO}_2 . \mathrm{NO}_2$ on cooling gives $\mathrm{N}_2 \mathrm{O}_4$ which is colourless solid. $\mathrm{N}_2 \mathrm{O}_4$ on reaction with ' $\mathrm{NO}^2$ ' gives $\mathrm{N}_2 \mathrm{O}_3$ which is a blue coloured compound.
Reactions involved are as following :
$$
2 \mathrm{NO}+\mathrm{N}_2 \mathrm{O}_4 \underset{250 \mathrm{~K}}{\stackrel{\Delta}{\longrightarrow}} 2 \underset{(\mathrm{C})}{2 \mathrm{~N}_2 \mathrm{O}_3}
$$
Structures of $\mathrm{N}_2 \mathrm{O}_4$ and $\mathrm{N}_2 \mathrm{O}_3$ are :
$$
\text { (i) } \mathrm{N}_2 \mathrm{O}_4
$$
$$
\text { (ii) } \mathrm{N}_2 \mathrm{O}_3
$$
Reactions involved are as following :
$$
2 \mathrm{NO}+\mathrm{N}_2 \mathrm{O}_4 \underset{250 \mathrm{~K}}{\stackrel{\Delta}{\longrightarrow}} 2 \underset{(\mathrm{C})}{2 \mathrm{~N}_2 \mathrm{O}_3}
$$
Structures of $\mathrm{N}_2 \mathrm{O}_4$ and $\mathrm{N}_2 \mathrm{O}_3$ are :
$$
\text { (i) } \mathrm{N}_2 \mathrm{O}_4
$$
$$
\text { (ii) } \mathrm{N}_2 \mathrm{O}_3
$$
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