An empirical formula specifies a ratio, not the number of atoms in one molecule. Reducing subscripts discards information about molecular size.
Recover the integer multiplier
For a molecular substance, divide the measured molar mass by the empirical-formula mass:
multiplier = molar mass ÷ empirical-formula mass
Multiply every empirical subscript by that same positive integer. Allow for measurement precision; a ratio far from an integer is a reason to recheck the data, not to round blindly.
A different example
NO₂ has an empirical-formula mass of approximately 46.01 g/mol. A molecular species with that ratio and molar mass 92.02 g/mol has multiplier 2, giving N₂O₄. The 1:2 atom ratio alone cannot distinguish NO₂ from N₂O₄.
What remains unknown
Even a molecular formula does not normally determine connectivity or three-dimensional structure. Empirical composition, molecular size, and structure answer different questions; obtain the evidence needed for each instead of treating one formula as a complete identification.
Related question
Apply this knowledge
Use the concept guide to understand the reasoning, then return to the complete question and worked answer.
Of the Following, the Only Empirical Formula Is: C₁₂H₂₂O₁₁Sources
These references support the core concepts and interpretation boundaries explained above.