Textbook Question
The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet®, is C14H18N2O5. (a) What is the molar mass of aspartame?
Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 3, Problem 40d
The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet®, is C14H18N2O5. (d) How many hydrogen atoms are present in 1.00 mg of aspartame?
Verified step by step guidance1
Determine the molar mass of aspartame (C_{14}H_{18}N_{2}O_{5}) by adding the atomic masses of all the atoms in the formula.
Convert the mass of aspartame from milligrams to grams, since molar mass is typically in grams per mole.
Calculate the number of moles of aspartame using the formula: \( \text{moles} = \frac{\text{mass in grams}}{\text{molar mass}} \).
Use Avogadro's number (6.022 \(\times\) 10^{23} molecules/mol) to find the number of molecules of aspartame in the calculated moles.
Multiply the number of molecules of aspartame by the number of hydrogen atoms per molecule (18) to find the total number of hydrogen atoms.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Formula
A molecular formula indicates the number and types of atoms in a molecule. For aspartame, C14H18N2O5 means it contains 14 carbon atoms, 18 hydrogen atoms, 2 nitrogen atoms, and 5 oxygen atoms. Understanding the molecular formula is essential for determining the composition of a compound and calculating quantities such as mass or number of atoms.
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Determining Molecular Formulas
Molar Mass
The molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find the number of hydrogen atoms in a given mass of aspartame, one must first calculate its molar mass by summing the atomic masses of all atoms in the molecular formula. This allows for conversions between mass and the number of molecules or atoms.
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Avogadro's Number
Avogadro's number, approximately 6.022 x 10^23, is the number of particles (atoms, molecules, etc.) in one mole of a substance. This concept is crucial for converting between moles and the actual number of molecules or atoms. In the context of aspartame, it helps determine how many hydrogen atoms are present in a specific mass of the compound by relating moles to individual atoms.
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Related Practice
Textbook Question
The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet®, is C14H18N2O5. (c) How many molecules of aspartame are present in 1.00 mg of aspartame?
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