A compound has an empirical (simple) formula, C2H2O. If the experimental molecular weight is found to be in the range 160-170, the molecular formula of this compound is: (Atomic weight: C = 12.1, H = 1.008, O = 16).
Correct answer: C. C8H8O4
- A. C3H6O3
- B. C4H4O2
- C. C8H8O4
- D. C6H6O3
Explanation
The empirical mass formula is 42, i.e., [2(12) + 2(1) + 16]. Multiplying the empirical formula mass by 4 will result in a molecular mass of 168, which is between 160 and 170, and would give us the molecular mass of C8H8O4.
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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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