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Ch.3 - Molecules and Compounds
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.3 - Molecules and CompoundsProblema 108
Capitolo 3, Problema 108

Tartaric acid is the white, powdery substance that coats tart candies such as Sour Patch Kids. Combustion analysis of a 12.01-g sample of tartaric acid—which contains only carbon, hydrogen, and oxygen—produces 14.08 g CO2 and 4.32 g H2O. Determine the empirical formula of tartaric acid.

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1
Calculate the moles of carbon in the CO2 produced using the molar mass of CO2.
Calculate the moles of hydrogen in the H2O produced using the molar mass of H2O.
Determine the mass of carbon and hydrogen in the original sample using their respective moles and atomic masses.
Subtract the mass of carbon and hydrogen from the total mass of the sample to find the mass of oxygen.
Convert the masses of carbon, hydrogen, and oxygen to moles, then find the simplest whole number ratio to determine the empirical formula.

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Combustion Analysis

Combustion analysis is a technique used to determine the elemental composition of organic compounds. In this process, a sample is burned in excess oxygen, and the products, typically carbon dioxide (CO2) and water (H2O), are measured. The masses of these products allow for the calculation of the amounts of carbon, hydrogen, and oxygen in the original sample, which is essential for determining the empirical formula.
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Combustion of Non-Hydrocarbons

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 moles of each element calculated from the mass of the products obtained during combustion analysis. This formula does not provide information about the actual number of atoms in a molecule but is crucial for understanding the basic composition of the substance.
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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 10^23) of entities, whether they are atoms, molecules, or ions. This concept is vital for converting the mass of carbon, hydrogen, and oxygen obtained from combustion into moles, which are then used to determine the empirical formula.
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