Domanda del libro di testo
Calculate the empirical formula for each natural flavor based on its elemental mass percent composition. a. methyl butyrate (component of apple taste and smell): C 58.80%, H 9.87%, O 31.33%
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Ch.3 - Molecules and Compounds
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
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Capitolo 3, Problema 97a
Calculate the empirical formula for each stimulant based on its elemental mass percent composition.
a. nicotine (found in tobacco leaves): C 74.03%, H 8.70%, N 17.27%
b. caffeine (found in coffee beans): C 49.48%, H 5.19%, N 28.85%, O 16.48%
Guida verificata passo dopo passo1
Step 1: Assume you have 100 grams of nicotine, which makes the mass of each element equal to its percentage.
Step 2: Convert the mass of each element to moles by dividing by its atomic mass: C (12.01 g/mol), H (1.008 g/mol), N (14.01 g/mol).
Step 3: Determine the mole ratio by dividing each element's mole value by the smallest number of moles calculated in Step 2.
Step 4: If necessary, multiply the mole ratios by a whole number to get whole numbers for each element.
Step 5: Write the empirical formula using the whole number mole ratios as subscripts for each element.
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Empirical Formula
The empirical formula represents the simplest whole-number ratio of the elements in a compound. It is derived from the percent composition of each element, which indicates how much of each element is present in a sample. For example, if a compound contains 50% carbon and 50% oxygen, its empirical formula would be CO, reflecting the 1:1 ratio.
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Percorso guidato
02:26
Empirical vs Molecular Formula
Mass Percent Composition
Mass percent composition is the percentage by mass of each element in a compound relative to the total mass of the compound. It is calculated by dividing the mass of each element by the total mass and multiplying by 100. This information is crucial for determining the empirical formula, as it provides the necessary data to find the ratio of elements.
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Percorso guidato
00:38Mass Percent Calculation
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 essential for converting mass percent compositions into moles, which are then used to derive the empirical formula.
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01:25Mole Concept
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