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Q. A colourless inorganic salt $(A)$ decomposes completely at about $250^{\circ} C$ to give only two products $(B)$ and $(C)$, leaving no residue. The oxide $(C)$ is a liquid at room temperature and neutral to moist litmus paper, while the gas $(B)$ is a neutral oxide.
White phosphorus bums in excess of $(B)$ to produce a strong white dehydrating agent. Write balanced equations for the reactions involved in the above process.

IIT JEEIIT JEE 1996Organic Chemistry – Some Basic Principles and Techniques

Solution:

$\underset {\text{Inorganic salt}}{A} \xrightarrow {250^\circ C} \underset{\text{Neutral oxide}}{B} + \underset{\text{Neutral oxide (liquid)}}{C}$
Oxide $C$ is liquid and neutral to litmus, so it is $H_2 O$. White phosphorus burns in excess of $B$ to give $P_4 O_{10}.$
Therefore, $B$ is $N_2 0.$
$ NH_4 NO_3 (A) \xrightarrow{\Delta} N_2 O + 2H_2 O (l)$
$ P_4 + 10N_2 O \longrightarrow P_4 O_{10} + 10N_2$