1. Determine the mass of oxygen:

* Mass of oxygen = Mass of oxide - Mass of phosphorus

* Mass of oxygen = 0.142 g - 0.062 g = 0.080 g

2. Convert masses to moles:

* Moles of phosphorus = Mass of phosphorus / Molar mass of phosphorus

* Moles of phosphorus = 0.062 g / 30.97 g/mol ≈ 0.002 mol

* Moles of oxygen = Mass of oxygen / Molar mass of oxygen

* Moles of oxygen = 0.080 g / 16.00 g/mol ≈ 0.005 mol

3. Find the simplest whole-number ratio of moles:

* Divide both mole values by the smaller one (0.002 mol):

* Phosphorus: 0.002 mol / 0.002 mol = 1

* Oxygen: 0.005 mol / 0.002 mol = 2.5

4. Adjust to whole numbers (if necessary):

* Since we have a 1:2.5 ratio, multiply both by 2 to get whole numbers:

* Phosphorus: 1 * 2 = 2

* Oxygen: 2.5 * 2 = 5

5. Write the empirical formula:

* The empirical formula is P₂O₅.