Final answer:
The empirical formula for a compound with the molecular formula C6H12Br202 is found by dividing the subscripts by the greatest common divisor, resulting in the empirical formula C2H4Br101.
Step-by-step explanation:
The empirical formula for a compound is the simplest whole-number ratio of elements in that compound. Given the molecular formula C6H12O6, the simplest whole-number ratio of C to H to O atoms in glucose is 1:2:1, which means the empirical formula is CH2O. To determine the empirical formula from a molecular formula such as C6H12Br202, you divide the subscripts by the greatest common divisor for each element. In this case, dividing each subscript of C6H12Br202 by 6 yields C1H2Br1O1, which simplifies to CH2BrO, making option A) CHBrO the incorrect empirical formulae. The correct empirical formula is C2H4Br101, which is simplified from the molecular formula by dividing each element's subscript by the smallest integer possible that still leaves a whole number.