Then it's molecular formula is what?

Step 1: Calculate the empirical formula mass. The empirical formula is $\text{C}_2H_6\text{O}$. Atomic masses: C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol. $Empirical formula mass = (2 \times 12.01) + (6 \times 1.008) + (1 \times 16.00)$ $Empirical formula mass = 24.02 + 6.048 + 16.00$ $Empirical formula mass = 46.068 g/mol$

Step 2: Determine the ratio ($n$) between the relative molecular mass and the empirical formula mass. Given relative molecular mass = 92. $n = \frac{Relative molecular mass}{Empirical formula mass}$ $n = \frac{92}{46.068}$ $n \approx 1.997 \approx 2$

Step 3: Multiply the subscripts in the empirical formula by $n$ to find the molecular formula. Empirical formula = $\text{C}_2H_6\text{O}$ Molecular formula = $(C_2H_6O)_n = (C_2H_6O)_2$ $Molecular formula = C_{2 \times 2}H_{6 \times 2}O_{1 \times 2}$ $Molecular formula = C_4H_{12}O_2$

The molecular formula is $\boxed{C_4H_{12}O_2}$.