The empirical formula and molar mass of several compounds...

The empirical formula and molar mass of several compounds are listed here. Find the molecular formula of each compound. a. $\mathrm{C}_6 \mathrm{H}_7 \mathrm{~N}, 186.24 \mathrm{~g} / \mathrm{mol}$ b. $\mathrm{C}_2 \mathrm{HCl}, 181.44 \mathrm{~g} / \mathrm{mol}$ c. $\mathrm{C}_5 \mathrm{H}_{10} \mathrm{NS}_2, 296.54 \mathrm{~g} / \mathrm{mol}$

The empirical formula and molar mass of several compounds are listed here. Find the molecular formula of each compound.
a. $\mathrm{C}_6 \mathrm{H}_7 \mathrm{~N}, 186.24 \mathrm{~g} / \mathrm{mol}$
b. $\mathrm{C}_2 \mathrm{HCl}, 181.44 \mathrm{~g} / \mathrm{mol}$
c. $\mathrm{C}_5 \mathrm{H}_{10} \mathrm{NS}_2, 296.54 \mathrm{~g} / \mathrm{mol}$

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Key Concepts

Determination of Molecular Formula

To determine a molecular formula, one calculates the mass of the empirical formula, compares it to the given molar mass, and finds the ratio (multiplier) between them. This multiplier, when applied to the subscripts of the empirical formula, yields the molecular formula.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole. It allows for the conversion between the mass of a sample and the number of moles and is essential for comparing with the mass of an empirical formula.

Empirical Formula

The empirical formula represents the simplest whole-number ratio of atoms of each element in a compound. It provides the proportions of the elements but not the actual number of atoms in the molecule.

Molecular Formula

The molecular formula indicates the actual number of atoms of each element in a molecule. Unlike the empirical formula, it provides the precise numbers, which are determined using the empirical formula and the compound’s molar mass.

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