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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 26f
Capitolo 3, Problema 26f

Calculate the percentage by mass of the indicated element in the following compounds: (f) carbon in sucrose, C12H22O11, the compound that is responsible for the sweet taste of table sugar.

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Identify the molecular formula of sucrose, which is \( \text{C}_{12}\text{H}_{22}\text{O}_{11} \).
Calculate the molar mass of sucrose by adding the atomic masses of all the atoms in the formula: \( 12 \times \text{C} + 22 \times \text{H} + 11 \times \text{O} \).
Calculate the total mass of carbon in sucrose by multiplying the number of carbon atoms (12) by the atomic mass of carbon (approximately 12.01 g/mol).
Determine the percentage by mass of carbon by dividing the total mass of carbon by the molar mass of sucrose and then multiplying by 100.
Express the final result as a percentage to indicate the mass percentage of carbon in sucrose.

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Molar Mass Calculation

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To calculate the molar mass of a compound, sum the molar masses of all the atoms in its chemical formula. For sucrose (C12H22O11), this involves calculating the contributions from carbon, hydrogen, and oxygen based on their respective atomic masses.
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Molar Mass Calculation Example

Percentage by Mass

Percentage by mass is a way to express the concentration of an element in a compound. It is calculated by dividing the mass of the element in one mole of the compound by the total molar mass of the compound, then multiplying by 100. This provides a clear understanding of how much of the compound's mass is due to a specific element.
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Empirical and Molecular Formulas

The empirical formula represents the simplest whole-number ratio of elements in a compound, while the molecular formula shows the actual number of atoms of each element in a molecule. Understanding these formulas is crucial for determining the composition of compounds like sucrose, as it helps in identifying the number of carbon atoms needed for the mass percentage calculation.
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Empirical vs Molecular Formula
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