The empirical formula and molecular mass of a compound are CH₂O and 180 g/mol respectively. The molecular formula of the compound is:
Correct answer: C. C₆H₁₂O₆
- A. C₉H₁₈O₉
- B. CH₂O
- C. C₆H₁₂O₆
- D. C₂H₄O₂
Explanation
The mass of the empirical formula (CH₂O) is 30 g/mol. The ratio of the molecular mass to the empirical mass is 180/30 = 6. Multiplying the subscripts in the empirical formula by 6 gives (CH₂O)₆ = C₆H₁₂O₆.
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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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