Question

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.

Answer 1

$\underset{\text{Inorganic salt}}{A}\stackrel{250^{\circ }C}{\to }\underset{\text{Neutral oxide}}{B}+\underset{\text{Neutral oxide (liquid)}}{C}$
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 $N_{2}0.$
$N{H}_{4}N{O}_3(A)\stackrel{\Delta }{\to }{N}_{2}O+2H_{2}O(l)$
$P_4+10N_{2}O⟶P_4{O}_{10}+10N_2$