Hexamethylene diamine is used to make nylon. If the molar mass is 115 g / mol and the empirical

step 1 We're given the empirical formula here, and we want to find the molecular formula. So we have to

Hexamethylene diamine is used to make nylon. If the molar...

Hexamethylene diamine is used to make nylon. If the molar mass is $115 \mathrm{~g} / \mathrm{mol}$ and the empirical formula is $\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{~N}$, what is the molecular formula of the compound?

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Key Concepts

Empirical Formula

The empirical formula of a compound represents the simplest whole-number ratio of the atoms of each element present. It provides the basic composition of the substance but does not necessarily reflect the actual number of atoms in a molecule.

Molar Mass

Molar mass is the mass of one mole of a substance, given in grams per mole. It is used to relate the physical mass of a compound to the number of moles, which is essential for quantitative chemical analysis and calculations.

Molecular Formula Determination

Determining the molecular formula involves using the empirical formula and the compound's molar mass. The process requires calculating the mass of the empirical unit, then dividing the given molar mass by this empirical mass to find a multiplication factor. Multiplying the subscripts in the empirical formula by this factor yields the molecular formula.

Calculation of the Multiplication Factor

This concept involves obtaining an integer or approximate integer value by dividing the molar mass of the compound by the molar mass of its empirical formula. The multiplication factor indicates how many times the empirical formula must be repeated to arrive at the true molecular formula.

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