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

To solve the problem step by step, we need to identify the compounds involved and write the balanced equations for the reactions.

### Step 1: Identify the inorganic salt (A)
The inorganic salt (A) is colorless and decomposes at about 250°C. Given the properties of the products (B and C), we can deduce that (A) is likely **ammonium nitrate (NH₄NO₃)**.

### Step 2: Write the decomposition reaction for (A)
When ammonium nitrate decomposes, it produces nitrous oxide (B) and water (C). The balanced equation for this decomposition is:

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