A 1.50 g sample of a pure organic compound containing only carbon, hydrogen, and oxygen is completely burned in excess oxygen gas. All of the carbon in the compound is converted to \(\text{CO}_2\text{(g)}\) and all of the hydrogen is converted to \(\text{H}_2\text{O(g)}\). The masses of the products collected are shown in the table below.

Product	Mass (g)
\(\text{CO}_2\text{(g)}\)	2.20
\(\text{H}_2\text{O(g)}\)	0.90

Based on these data, what is the empirical formula of the compound?