What is the molecular formula of a compound that weighs 46 g/mol and analyzes to 52.2% C, 34.8% O, and 13% H?

Question

Quizplus · Accepted Answer

1) Calculate the empirical formula:
Assuming a 100g sample, there are 52.2g C, 34.8g O, and 13g H.
Convert to moles: 
C: 52.2/12.01 = ~4.35
O: 34.8/16 = ~2.18
H: 13/1.01 = ~12.87
Divide by the smallest number of moles (2.18):
C: ~2
O: ~1
H: ~6
Empirical formula: C2H6O
2) Calculate the molecular formula:
Molecular weight = 46 g/mol ÷ empirical weight (30 g/mol) = 1.53
Round to nearest whole number:
C2H6O x1.53 = C3H9O
The molecular formula is C3H9O, which matches option B.

What Is the Molecular Formula of a Compound That Weighs