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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 45a
Capitolo 3, Problema 45a

Give the empirical formula of each of the following compounds if a sample contains (a) 0.052 mol C, 0.103 mol H, and 0.017 mol O

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Identify the number of moles of each element in the compound: 0.052 mol C, 0.103 mol H, and 0.017 mol O.
Divide the number of moles of each element by the smallest number of moles present among the elements to find the simplest whole number ratio. In this case, divide each by 0.017 mol.
Calculate the resulting ratios: \( \frac{0.052}{0.017} \) for C, \( \frac{0.103}{0.017} \) for H, and \( \frac{0.017}{0.017} \) for O.
Round the ratios to the nearest whole number to determine the subscripts for each element in the empirical formula.
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 mole quantities of each element, providing a basic understanding of the composition without indicating the actual number of atoms in a molecule.
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Empirical vs Molecular Formula

Mole Concept

The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole corresponds to approximately 6.022 x 10²³ entities (atoms, molecules, etc.). Understanding the mole concept is essential for converting between mass, number of particles, and volume in chemical calculations.
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Mole Concept

Mole Ratio

Mole ratio refers to the proportional relationship between the amounts of different substances involved in a chemical reaction or composition. It is calculated by dividing the number of moles of each element by the smallest number of moles present, which helps in determining the empirical formula of a compound.
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Neutron-Proton Ratio
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