The empirical formula is \( \text{CH}_2\text{O} \). Its molar mass is calculated as follows:\[\text{Molar mass of } \text{CH}_2\text{O} = 12 + 2(1) + 16 = 30 \, \text{g/mol}\]Comparing the compound's molar mass (90 g/mol) to the empirical formula's molar mass (30 g/mol) yields:\[\frac{\text{Molar mass of compound}}{\text{Molar mass of empirical formula}} = \frac{90}{30} = 3\]This indicates the molecular formula is three times the empirical formula. Consequently, the molecular formula is:\[\text{Molecular formula} = 3 \times \text{CH}_2\text{O} = \text{C}_3\text{H}_6\text{O}_3\]Therefore, the molecular formula of the compound is \( \text{C}_3\text{H}_6\text{O}_3 \).