Hydrazine, ammonia, and hydrogen azide all contain only...

Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of hydrogen that combines with $1.00 \mathrm{g}$ of nitrogen for each compound is $1.44 \times 10^{-1} \mathrm{g}$ $2.16 \times 10^{-1} \mathrm{g},$ and $2.40 \times 10^{-2} \mathrm{g},$ respectively. Show how these data illustrate the law of multiple proportions.

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Key Concepts

Law of Multiple Proportions

This law states that when two elements form more than one compound, the different masses of one element that combine with a fixed mass of the other are in ratios of small whole numbers. It reflects the underlying atomic theory that compounds are formed by atoms combining in fixed, discrete amounts. In the problem, the varying masses of hydrogen that combine with a fixed mass of nitrogen in different compounds exemplify this principle.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in chemical reactions. It provides the framework for understanding how mass ratios, like those given in the problem, correspond to moles and the numbers of atoms within compounds. By comparing the mass ratios, one can deduce the simple whole-number ratios of atoms forming the compounds.

Empirical Formulas

Empirical formulas represent the simplest whole-number ratio of atoms in a compound. Determining an empirical formula from experimental mass data involves converting masses to moles, which then show the relative numbers of atoms. The given data on hydrogen combining with nitrogen illustrates how different compounds of the same elements have empirical formulas that reflect different whole-number ratios of the atoms.

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