The empirical mass of C\(_6\)H\(_{12}\)O\(_6\) is [H =1, C = 12, O = 16]

The empirical formula is the simplest whole-number ratio of atoms in a compound. The empirical formula mass (sometimes called empirical mass) is the molar mass corresponding to that simplest formula.

The molecular formula given is C₆H₁₂O₆. To find the empirical formula, divide all subscripts by their greatest common factor:

\[\text{GCF of } 6, 12, 6 = 6\]

\[\text{Empirical formula} = \text{C}_1\text{H}_2\text{O}_1 = \text{CH}_2\text{O}\]

Now calculate the empirical formula mass using the given atomic masses (H = 1, C = 12, O = 16):

\[\text{Empirical mass} = 12 + 2(1) + 16 = 30\]

As a check, the molecular mass of C₆H₁₂O₆ is 6(12) + 12(1) + 6(16) = 72 + 12 + 96 = 180. Dividing by the empirical mass: 180 / 30 = 6, confirming that the molecular formula is exactly 6 times the empirical formula.