To determine the chemical formula of the unknown compound \( \text{N}_x\text{O}_x \), you need to find the simplest whole number ratio of nitrogen (N) to oxygen (O) atoms. Here are the steps:
1. **Determine the ratio of moles**:
- You have 4.40 mol of oxygen and 2.9 mol of nitrogen.
2. **Calculate the simplest ratio**:
- To find the simplest ratio, divide each amount by the smaller number of moles:
\[
\text{Ratio of nitrogen (N)} = \frac{2.9}{2.9} = 1
\]
\[
\text{Ratio of oxygen (O)} = \frac{4.4}{2.9} \approx 1.52
\]
3. **Simplify the ratio to whole numbers**:
- The ratio 1:1.52 suggests that there are approximately 1.52 oxygens for every nitrogen.
- To simplify this to the smallest whole numbers, we can multiply both sides by a factor that will convert the decimal into a whole number.
- Here, multiplying by 2 gives:
\[
1.52 \times 2 = 3.04 \approx 3
\]
- So the ratio is approximately 2:3.
Therefore, the simplest and closest whole number ratio of nitrogen to oxygen is 2:3, leading to the chemical formula:
\[
\text{N}_2\text{O}_3
\]
So, the complete chemical formula for the unknown compound is \( \text{N}_2\text{O}_3 \).
An unknown compound has the following chemical formula
N_xO_x
Measurements also show that a certain sample of the unknown compound contains 4.40 mol of oxygen and 2.9 mol of nitrogen.
Write the complete chemical formula for the unknown compound.
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1 answer