Since the molar mass is provided, it is safe to assume that the empirical formula is not equal to the molecular formula.
We need to get the empirical weight to determine the multiple needed to arrive to the correct molecular formula.
Atom Number in Molecule Atomic Weight Total Mass C 1 12.0107 12.0107 Cl 1 35.453 <u> 35.453</u> total empirical weight 47.4637
Molecular weight / Empirical Weight 284.77 g/mol / 47.46 g/mol = 6 - the multiple needed to be multiplied with the empirical formula to get the molecular formula.
C has a molecular number of 1 => 1 * 6 = 6 Thus C₆ Cl has a molecular number of 1 => 1 * 6 = 6 Thus Cl₆
Jill and Susan violated safety procedures by not properly listening and/or reading over the instructions to know all the materials, steps, and equipment they need for the lab. Hope this helps!
