To find the empirical formula, we need to determine the simplest whole number ratio of the elements in the compound.

1. Convert the percentages to grams:

- Carbon: 52.17% = 52.17 g

- Hydrogen: 6.90% = 6.90 g

- Nitrogen: 9.52% = 9.52 g

- Oxygen: 31.41% = 31.41 g

2. Convert the grams of each element to moles:

- Carbon: 52.17 g / 12.01 g/mol = 4.34 mol

- Hydrogen: 6.90 g / 1.01 g/mol = 6.84 mol

- Nitrogen: 9.52 g / 14.01 g/mol = 0.68 mol

- Oxygen: 31.41 g / 16.00 g/mol = 1.96 mol

3. Divide each mole value by the smallest mole value to get the simplest whole number ratio:

- Carbon: 4.34 mol / 0.68 mol ≈ 6.4

- Hydrogen: 6.84 mol / 0.68 mol ≈ 10.1

- Nitrogen: 0.68 mol / 0.68 mol = 1

- Oxygen: 1.96 mol / 0.68 mol ≈ 2.9

4. Round the ratios to the nearest whole numbers:

- Carbon: 6

- Hydrogen: 10

- Nitrogen: 1

- Oxygen: 3

5. Write the empirical formula using the rounded ratios:

C6H10NO3