Which of the following is a molecular formula for a compound with an empirical formula of CH₂O and a molar mass of 150.g/mol?

Question

Quizplus · Accepted Answer

1. Calculate the empirical formula mass: - molar mass of C = 12.01 g/mol - molar mass of H = 1.01 g/mol - molar mass of S = 32.07 g/mol - molar mass of U = 238.03 g/mol (Assuming U is Uranium) - molar mass of B = 10.81 g/mol - molar mass of O = 16.00 g/mol Empirical formula mass = (12.01 x 1) + (1.01 x 1) + (32.07 x 1) + (238.03 x 1) + (10.81 x 12) + (16.00 x 1) = 361.25 g/mol 2. Calculate the ratio of molar mass to empirical formula mass: Molar mass/empirical formula mass = 150/361.25 = 0.415 3. Multiply the empirical formula by the ratio: CH₂O x 0.415 = C₅H₁₀O₅ Therefore, choice B (C₅H₁₀O₅) is the correct molecular formula.

Which of the Following Is a Molecular Formula for a Compound