From the given empirical formula and molar mass, find the molecular formula of each compound. a. C₆H₇N, 186.24 g/mol

Key Concepts

Empirical Formula

The empirical formula represents the simplest whole-number ratio of atoms of each element in a compound. It provides essential information about the composition of the compound but does not indicate the actual number of atoms present in a molecule. For example, the empirical formula for glucose (C6H12O6) is CH2O, reflecting the ratio of carbon, hydrogen, and oxygen.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in the molecular formula. Knowing the molar mass is crucial for converting between grams and moles, and it helps in determining the molecular formula from the empirical formula when combined with the empirical formula's mass.

Molecular Formula

The molecular formula indicates the actual number of atoms of each element in a molecule of a compound. It can be derived from the empirical formula by multiplying the subscripts by a whole number, which is determined by the ratio of the compound's molar mass to the empirical formula mass. For instance, if the empirical formula is CH2 and the molar mass is 86 g/mol, the molecular formula would be C6H12.