Question

missed this? watch kcv: calculating empirical formulas for compounds, section in your etext. a 2.241 g sample of zinc reacts with oxygen to form 2.789 g of the metal oxide part a calculate the empirical formula of the oxide. express your answer as a chemical formula. a chemical reaction does not occur for this question. submit request answer

Explanation:

Step1: Find mass of oxygen

Mass of oxide = 2.789 g, mass of Zn = 2.241 g. So mass of O = 2.789 - 2.241 = 0.548 g.

Step2: Moles of Zn and O

Molar mass of Zn = 65.38 g/mol, moles of Zn = $\frac{2.241}{65.38}$ ≈ 0.03428 mol. Molar mass of O = 16.00 g/mol, moles of O = $\frac{0.548}{16.00}$ ≈ 0.03425 mol.

Step3: Mole ratio

Divide moles by smallest (≈0.03425). Ratio Zn:O ≈ 1:1.

Answer:

ZnO