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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown - Chemistry: The Central Science 15th Edition
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Capitolo 3, Problema 47a

Determine the empirical formulas of the compounds with the following compositions by mass: a. 10.4% C, 27.8% S, and 61.7% Cl

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Convert the percentage of each element to grams, assuming you have 100 grams of the compound. This means you have 10.4 grams of C, 27.8 grams of S, and 61.7 grams of Cl.
Convert the mass of each element to moles by dividing by their respective molar masses: C (12.01 g/mol), S (32.07 g/mol), and Cl (35.45 g/mol).
Determine the mole ratio of the elements by dividing each element's mole value by the smallest number of moles calculated in the previous step.
If necessary, multiply the ratios by a whole number to get whole numbers for each element in the compound.
Write the empirical formula using the whole number ratios as subscripts for each element.

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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

Mole Concept

The mole concept is a fundamental principle in chemistry that relates the mass of a substance to the number of particles it contains. One mole of any substance contains Avogadro's number (approximately 6.022 x 10²³) of entities, whether they are atoms, molecules, or ions, facilitating conversions between mass and number of particles.
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Mole Concept

Mass Percent Composition

Mass percent composition is the percentage by mass of each element in a compound. It is calculated by dividing the mass of each element by the total mass of the compound and multiplying by 100. This information is crucial for determining the empirical formula, as it provides the necessary data to find the mole ratios of the elements.
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