Consider 100.0-g samples of two different compounds...

Consider $100.0-\mathrm{g}$ samples of two different compounds consisting only of carbon and oxygen. One compound contains $27.2 \mathrm{~g}$ of carbon and the other has $42.9 \mathrm{~g}$ of carbon. How can these data support the law of multiple proportions if $42.9$ is not a multiple of $27.2$ ? Show that these data support the law of multiple proportions.

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Key Concepts

Mass Percent Composition

Mass percent composition refers to the percentage by mass of each element in a compound. By knowing the percent composition, one can calculate the actual grams of each element present in a given mass sample. This is crucial for comparing the relative amounts of each element in different compounds, which is key in verifying the law of multiple proportions.

Stoichiometry

Stoichiometry involves using the relative quantities of reactants and products, determined by balanced chemical equations and molar masses, to draw conclusions about the composition of compounds. It allows for the conversion of mass measurements into mole ratios, highlighting the simple whole number ratios expected by the law of multiple proportions.

Law of Multiple Proportions

This law states that when two elements form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other are small whole numbers. It underpins the idea that compounds are made of atoms in fixed, discrete ratios and that these ratios reflect the simple integer multiples of the masses of the elements involved.

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