A compound (60 g) on analysis gave C = 24 g, H = 4 g, O = 32 g. Its empirical formula is:
Correct answer: D. CH₂O
- A. C₂H₄O₂
- B. CH₂O₂
- C. C₂H₂O₂
- D. CH₂O
Explanation
Convert the mass of each element to moles: Moles C = 24/12 = 2; Moles H = 4/1 = 4; Moles O = 32/16 = 2. The mole ratio C:H:O is 2:4:2. Dividing by the smallest number (2) gives the simplest ratio, 1:2:1, so the empirical formula is CH₂O.
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Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.
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