1. Convert Mass Percentages to Grams:

* Assume you have 100 g of the compound. This means you have:

* 53.31 g Carbon

* 11.18 g Hydrogen

* 35.51 g Oxygen

2. Convert Grams to Moles:

* Divide the mass of each element by its molar mass:

* Carbon: 53.31 g / 12.01 g/mol = 4.44 mol

* Hydrogen: 11.18 g / 1.01 g/mol = 11.07 mol

* Oxygen: 35.51 g / 16.00 g/mol = 2.22 mol

3. Find the Simplest Mole Ratio:

* Divide each mole value by the smallest mole value (2.22 mol in this case):

* Carbon: 4.44 mol / 2.22 mol = 2

* Hydrogen: 11.07 mol / 2.22 mol = 5

* Oxygen: 2.22 mol / 2.22 mol = 1

4. Determine the Empirical Formula:

* The simplest whole-number ratio of the elements is C₂H₅O.

5. Calculate the Empirical Formula Mass:

* C₂H₅O: (2 x 12.01) + (5 x 1.01) + (1 x 16.00) = 45.07 g/mol

6. Find the Molecular Formula:

* Divide the given molar mass by the empirical formula mass:

* 90.122 g/mol / 45.07 g/mol ≈ 2

* Multiply the subscripts in the empirical formula by this factor (2):

* C₂H₅O x 2 = C₄H₁₀O₂

Therefore, the molecular formula of the compound is C₄H₁₀O₂.