Final answer:
To find the molecular formula of a compound with a molar mass of 183.2 g/mol, the empirical formula and elemental composition are needed. The molecular formula is determined by how many times the empirical formula's mass fits into the actual molar mass.
Step-by-step explanation:
To determine the molecular formula of a compound with a given molar mass, we first need to know the compound's empirical formula and its molar mass. The empirical formula provides the simplest whole number ratio of the atoms in the compound, while the molar mass is the weight of one mole of that same compound.
For example, if a compound has an empirical formula of C2H5 and a molar mass of 58.12 g/mol, by comparing the molar mass of the empirical formula with the actual molar mass, we can determine how many times the empirical formula must be multiplied to get the molecular formula. If, for instance, the molar mass of the empirical formula is half of the given molar mass, then the molecular formula would be a multiple of two of the empirical formula (C4H10).
However, to provide an answer to a specific compound's molecular formula with a given molar mass of 183.2 g/mol, additional details such as the empirical formula or the percentages of the constituent elements by mass are required. If this information were provided, we could use the molar mass to deduce the molecular formula by determining how many times the empirical formula mass fits into the molecular mass.