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To determine the empirical formula of the compound that contains only iron (Fe) and oxygen (O) and is 22.27% oxygen by mass, follow these steps:

1. **Assume a 100 g sample**: In this case, 22.27 g of the sample is oxygen, and the remaining 77.73 g is iron.

2. **Convert the masses to moles**:
   - Moles of oxygen: \( \frac{22.27 \, \text{g}}{16.00 \, \text{g/mol}} = 1.392 \, \text{mol} \)
   - Moles of iron: \( \frac{77.73 \, \text{g}}{55.85 \, \text{g/mol}} = 1.392 \, \text{mol} \)

3. **Determine the mole ratio**: The ratio of iron to oxygen is approximately 1:1, as both have about 1.392 moles.

4. **Empirical formula**: Since the mole ratio is 1:1, the empirical formula of the compound is **FeO**.

So, the correct answer is **A**: FeO.

Would you like more details or have any questions?

Here are 5 related questions:
1. How do you calculate empirical formulas for compounds with more elements?
2. Why is the empirical formula important in chemistry?
3. What is the difference between empirical and molecular formulas?
4. Can you explain how to deal with decimal mole ratios in empirical formula calculations?
5. How is the percent composition used to determine empirical formulas in more complex compounds?

**Tip**: Always remember to simplify mole ratios by dividing by the smallest number of moles to get the simplest whole-number ratio.

What is the empirical formula of a compound that contains only iron and oxygen and is 22.27% oxygen?

Discover how to calculate the empirical formula of a compound that contains only iron and oxygen with 22.27% oxygen by mass. This detailed step-by-step solution covers concepts such as stoichiometry, mole calculations, and determining the empirical formula. Ideal for high school students in Grades 10-12.

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