Then it's molecular formula is what?

The empirical formula is $\text{C}_2\text{H}_6\text{O}$.
Atomic masses: C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol.

$$\text{Empirical formula mass} = (2 \times 12.01) + (6 \times 1.008) + (1 \times 16.00)$$ $$\text{Empirical formula mass} = 24.02 + 6.048 + 16.00$$ $$\text{Empirical formula mass} = 46.068 \text{ g/mol}$$

Given relative molecular mass = 92.

$$n = \frac{\text{Relative molecular mass}}{\text{Empirical formula mass}}$$ $$n = \frac{92}{46.068}$$ $$n \approx 1.997 \approx 2$$

Empirical formula = $\text{C}_2\text{H}_6\text{O}$
Molecular formula = $(\text{C}_2\text{H}_6\text{O})_n = (\text{C}_2\text{H}_6\text{O})_2$

$$\text{Molecular formula} = \text{C}_{2 \times 2}\text{H}_{6 \times 2}\text{O}_{1 \times 2}$$ $$\text{Molecular formula} = \text{C}_4\text{H}_{12}\text{O}_2$$

The molecular formula is $\text{C}_4\text{H}_{12}\text{O}_2$.