A sample of ammonium nitrate when heated yields 8.96 litres of steam (measured at S.T.P.)
`NH_(4)NO_(3)toN_(2)O+2H_(2)O`
Determine the percentage of oxygen in ammonium nitrate (O = 16).

Explanation

To determine the percentage of oxygen in ammonium nitrate (NH₄NO₃), we will follow these steps:

### Step 1: Write down the balanced chemical equation
The decomposition of ammonium nitrate can be represented as:
\[ \text{NH}_4\text{NO}_3 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O} \]

### Step 2: Calculate the volume of water produced
From the balanced equation, we see that 1 mole of ammonium nitrate produces 2 moles of water (H₂O). At standard temperature and pressure (S.T.P.), 1 mole of any gas occupies 22.4 liters.
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