What is the empirical formula of a compound with 5.02g of C, .42g of H, and 1.33g of O?

Molar masses in g/mol: C = 12.0, H = 1.0, O = 16.0

Number of moles of C = (5.02 g) / (12.0 g/mol) = 0.418 mol
Number of moles of H = (0.42 g) / (1.0 g/mol) = 0.42 mol
Number of moles of O = (1.33 g) / (16.0 g/mol) = 0.0831 mol

Mole ratio C : H : O
= 0.418 : 0.42 : 0.0831
= 0.418/0.0831 : 0.42/0.0831 : 0.0831/0.0831
= 5 : 5 : 1

Empirical formula = C₅H₅O

(The molecular mass given is redundant because it is used to calculate the molecular formula.)
(324.38 / (12.0×5 + 1.0×5 + 16.0) = 4)
(The molecular formula = C₂₀H₂₀O₄)