What is the molecular formula for a compound that is 40.0% C, 6.6% H, and 53.4% O and the molar mass is 120.0g/mol?

molecular formula of the compound is C₄H₈O₄

Explanation:

First the empirical formula of the compound is determined:

Divide the percentage masses by the molar mass of each element to determine the mole ratio;

Carbon, C: 40/12 = 3.33

Hydrogen, H: 6.6/1 = 6.6

Oxygen, O: 53.4 / 16 = 3.3

dividing through with the smallest ratio to obtain the simplest whole number mole ratios

C = 3.3/3.3 = 1

H = 6.6/3.3 = 2

O = 3.3/3.3 = 1

Therefore, the empirical formula is CHO

molecular formula/mass = n (empirical formula/mass)

120 g/mol = n( 12 + 1 * 2 + 16)

30n = 120

n = 4 therefore, the molecular formula = 4(CH₂O)

molecular formula of the compound is C₄H₈O₄

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