Question

A colorless inorganic salt (A) decomposes completely at about ${250}^o$C to give only two products (B) and (C) leaving no residue. The (C) is a liquid at room temperature and neutral to moist litmus paper while the gas (B) is a neutral oxide. White phosphorus burns in excess of (B) to produce a strong dehydrating agent (D).
(A), (B), (C) and (D) are identified as

• A. $N{H}_{4}N{O}_3$, $N_{2}O$, $H_{2}O$ and $P_4{O}_{10}$.
• B. $N{H}_{4}N{O}_3$, $P_4{O}_{10}$, $N_{2}O$, and $H_{2}O$.
• C. $H_{2}O$, $N{H}_{4}N{O}_3$, $P_4{O}_{10}$, and $N_{2}O$.
• D. $P_4{O}_{10}$, $N{H}_{4}N{O}_3$, $N_{2}O$ and $H_{2}O$.

Answer 1

The correct option is A $N{H}_{4}N{O}_3$, $N_{2}O$, $H_{2}O$ and $P_4{O}_{10}$.

A colourless inorgnic salt $N{H}_{4}N{O}_3$ decomposes completely at about ${250}^o$C to give only two products $N_{2}O$ and $H_{2}O$ leaving no residue

$N{H}_{4}N{O}_3\stackrel{heat}{\to }{N}_{2}O+2H_{2}O$

The oxide $H_{2}O$ is a liquid at room temperature and neutral to moist litmus paper while the gas $N_{2}O$ is a neutral oxide. White phosphorus burns in excess of $N_{2}O$ to produce a strong while dehydrating agent $P_4{O}_{10}$.

$P_4+10N_{2}O\to P_4{O}_{10}+10N_2$.

Hence, option $A$ is correct.