Textbook Question
The ball-and-stick molecular model is a representation of caf-feine. Calculate the molecular weight of caffeine. (Gray = C, red = O, blue = N, ivory = H.) (LO 3.3)
(a) 194.2 (b) 182.2 (c) 192.2 (d) 180.2
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Ch.3 - Mass Relationships in Chemical Reactions
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 3, Problem 4
A can of diet soda contains 180 mg of the low-calorie sugar substitute aspartame (C14H18N2O5). How many molecules of aspartame are in the can of soda? (LO 3.4) (a) 3.7 * 10^23 (b) 3.7 * 10^20 (c) 3.2 * 10^25 (d) 1.2 * 10^22
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 in the can (180 mg) to grams by dividing by 1000.
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 convert the moles of aspartame to molecules by multiplying the number of moles by Avogadro's number.
Compare the calculated number of molecules to the given options to determine the correct answer.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For aspartame (C14H18N2O5), the molar mass can be calculated by summing the atomic masses of all the atoms in its molecular formula. This value is essential for converting between grams of a substance and moles, which is necessary for determining the number of molecules.
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Molar Mass Concept
Avogadro's Number
Avogadro's number, approximately 6.022 x 10^23, is the number of atoms, ions, or molecules in one mole of a substance. This constant allows chemists to relate the macroscopic scale of substances (grams) to the microscopic scale (individual molecules). In this problem, it is used to convert the number of moles of aspartame into the actual number of molecules present in the soda.
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Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It involves using balanced chemical equations to calculate the amounts of substances consumed and produced. In this context, stoichiometry helps in determining how many molecules of aspartame correspond to the given mass in the can of soda, facilitating the conversion from grams to molecules.
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Related Practice
Textbook Question
The reaction of A2 (red spheres) with B2 (blue spheres) is shown in the diagram. What is the balanced chemical equa-tion? (LO 3.1) (a) 2 A2 + 6 B2 ---> 4 AB3 (b) 4 A + 12 B ---> 4 AB3 (c) 4 A + 12 B ---> A4 + B12 (d) A2 + 3 B2 ---> 2 AB3
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Textbook Question
What are the coefficients in the balanced equation for the combustion of ethanol? (LO 3.2) (a) 1, 3, 2, 3(b) 2, 3, 4, 3(c) 2, 7, 4, 6(d) 1, 4, 2, 3
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Textbook Question
How many moles of chloride ions are in 7.75 g of FeCl3? (LO 3.4) (a) 4.78 * 10^-2 (b) 1.59 * 10^-2 (c) 1.43 * 10^-1 (d) 1.91 * 10^-1
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Textbook Question
One way to make coal burning better for the environment is to remove carbon dioxide from the exhaust gases released from power plants using a compound containing an amine (-NH2) group. The reaction between carbon dioxide and monoethanolamine is: CO2(g) + 2 HOCH2CH2NH2(aq) -> HOCH2CH2NH3 +(aq) + HOCH2CH2NHCO2-(aq) What mass of monoethanoloamine is required to react with 1.0 kg of carbon dioxide? (LO 3.5) (a) 2.8 kg(b) 1.1 kg(c) 0.93 kg(d) 0.53 kg
Textbook Question
If 42.85 grams of salicylic acid reacts with excess acetic anhydride and produces 48.47 grams of aspirin, what is the percent yield of the reaction? (LO 3.6) (a) 88.40% (b) 64.69%(c) 86.72% (d) 78.74%
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