A colourless inorganic salt `(A)` decomposes completely at about `250^@ C` to give only two products `(B)` and `( C)`, leaving no residue. The oxide `( C)` is a liquid at room temperature and neutral to litmus paper while the gas `(B)` is a neutral oxide. White phosphorous burns in excess of `(B)` to produce a strong white dehydrating agent. Write balanced equations for the reactions involved in this process.

Explanation

Given,
`underset (colourl ess)((A)) overset (250^@ C)rarr (B)_((g)) + underset (Ox ide)((C)_((1)))`
inorganic compound
Liquid `( C)` is neutral oxide at room temperature and neutral to litmus paper.
Gas `(B)` is neutral oxide.
`underset (Express) ((B)) + underset (White) (P_4) rarr` strong white dehydrating agent.
Both `(B)` and `( C)` are neutral oxides, `(B)` helps in combustion of white phosphorous, hence `(B)` can be nitrons oxide, `N_2 O. ( C)` is liquid at room temperature, hence it can be `H_2 O`.
`underset ((A)) (NH_4 NO_3) rarr underset ((B)) (N_2 O) + underset ((C))(2 H_2 O)`
`10 N_2 O + P_4O_10 + 10 N_2`
`P_4 O_10` is strong white dehydrating agent.
`(A)` is ammonium nitrate, `NH_4 NO_3, (B)` nitrous oxides, `N_2 O( C)` is water, `H_2 O`.