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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown - Chemistry: The Central Science 14th Edition
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Capitolo 3, Problema 46c

Determine the empirical formula of each of the following compounds if a sample contains (c) 89.14% Au and 10.86% O by mass.

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Determine the mass of each element in a 100 g sample based on the given percentages. For Au (gold), it would be 89.14 g, and for O (oxygen), it would be 10.86 g.
Convert the mass of each element to moles by using the atomic masses from the periodic table (Au = 197 g/mol, O = 16 g/mol).
Calculate the mole ratio of Au to O by dividing the moles of each element by the smallest number of moles obtained in the previous step.
If the mole ratio is not a whole number, multiply both ratios by the smallest number that will convert them into whole numbers.
The whole number mole ratios obtained will give the subscripts for each element in the empirical formula. Write the empirical formula by placing these subscripts as the indices of the respective elements.

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Empirical Formula

The empirical formula of a compound represents the simplest whole-number ratio of the elements present in that compound. It is derived from the percentage composition of each element, allowing chemists to understand the basic composition without detailing the molecular structure.
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Empirical vs Molecular Formula

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting the mass percentages of elements into moles, which are then used to determine the empirical formula by finding the simplest ratio of the elements.
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Molar Mass Concept

Conversion from Mass Percent to Moles

To find the empirical formula, the mass percent of each element must be converted to moles. This is done by dividing the mass of each element by its molar mass. The resulting values are then simplified to the smallest whole-number ratio, which gives the empirical formula.
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Mass Percent Conversion
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