an organic compound has relative moleculaf mass of 150 and contains 72.0% carbon, 6.67% hydrogen and 21.33% oxygen.Determine the emphirical formula

To determine the empirical formula, follow these steps:

1. Assume you have 100g of the compound. This means you have 72g of Carbon (C), 6.67g of Hydrogen (H), and 21.33g of Oxygen (O).

2. Convert these amounts into moles. Use the atomic masses of C, H, and O which are approximately 12g/mol, 1g/mol, and 16g/mol respectively.

   Moles of C = 72g / 12g/mol = 6 moles Moles of H = 6.67g / 1g/mol = 6.67 moles Moles of O = 21.33g / 16g/mol = 1.33 moles

3. Divide each of the calculated moles by the smallest number of moles calculated in step 2 to get the ratio of the atoms. In this case, the smallest number of moles is 1.33.

   Ratio of C = 6 / 1.33 = 4.5 ≈ 5 (rounded to the nearest whole number) Ratio of H = 6.67 / 1.33 = 5 Ratio of O = 1.33 / 1.33 = 1

4. The empirical formula of the compound is therefore C5H5O1, or simply C5H5O.