**Step 1: **We are given 58.55% C, 13.81% H, and 27.40% N by mass.

$\overline{){\mathbf{\%}}{\mathbf{}}{\mathbf{mass}}{\mathbf{=}}\frac{\mathbf{mass}\mathbf{}\mathbf{of}\mathbf{}\mathbf{X}}{\mathbf{total}\mathbf{}\mathbf{mass}}{\mathbf{\times}}{\mathbf{100}}}$

Assuming we have **100 g** of the compound, this means we have **58.55 g C, 13.81 g H,** and **27.40 g N**.

Determine the empirical and molecular formulas of each of the following substances. For example, butane has an empirical formula of C_{2}H_{5} (lowest whole-number ratio) and a molecular formula of C_{4}H_{10}, where the molecular formula corresponds to the molar mass of 58.12 g/mol.

Cadaverine, a foul-smelling substance produced by the action of bacteria on meat, contains 58.55% C, 13.81% H, and 27.40% N by mass; its molar mass is 102.2 g/mol.

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