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
Not the one you use?Change textbookSelect a different textbook
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 40c
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?
Verified step by step guidance1
Convert the mass of aspartame from milligrams to grams by using the conversion factor: 1 mg = 0.001 g.
Calculate 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: 14 carbon atoms, 18 hydrogen atoms, 2 nitrogen atoms, and 5 oxygen atoms.
Use the molar mass to convert the mass of aspartame in grams to moles by dividing the mass in grams by the molar mass.
Use Avogadro's number (6.022 \(\times\) 10^{23} molecules/mol) to convert the number of moles of aspartame to the number of molecules by multiplying the moles by Avogadro's number.
The result from the previous step gives the number of molecules of aspartame in 1.00 mg.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
2mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Formula
A molecular formula represents the number and types of atoms in a molecule. For aspartame, C14H18N2O5 indicates it contains 14 carbon atoms, 18 hydrogen atoms, 2 nitrogen atoms, and 5 oxygen atoms. Understanding the molecular formula is essential for calculating the molar mass and determining the number of molecules in a given mass.
Recommended video:
Guided course
02:08
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 molar mass of aspartame, one must sum the atomic masses of all atoms in its molecular formula. This value is crucial for converting between mass and the number of molecules using Avogadro's number.
Recommended video:
Guided course
02:11Molar Mass Concept
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 constant allows for the conversion between the mass of a substance and the number of molecules. In the context of aspartame, it helps determine how many molecules are present in a specified mass, such as 1.00 mg.
Recommended video:
Guided course
02:11Avogadro's Law
Related Practice
Textbook Question
The molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is C6H10OS2. (c) How many molecules of allicin are in 5.00 mg of this substance?
Textbook Question
A sample of glucose, C6H12O6, contains 1.250×1021 carbon atoms. (c) How many moles of glucose does it contain?
Textbook Question
A sample of the male sex hormone testosterone, C19H28O2, contains 3.88×1021 hydrogen atoms. (b) How many molecules of testosterone does it contain?
Textbook Question
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?
Textbook Question
The molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is C6H10OS2. (d) How many S atoms are present in 5.00 mg of allicin?