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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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 8
The diagram represents a mixture of AB2 and B2 before it reacts to form AB3. (Red spheres = A, blue spheres = B.) Which reactant is limiting, and how many AB3 molecules are formed? (LO 3.7) 
(a) B2 is limiting, and 10 molecules of AB3 are formed. (b) B2 is limiting, and 4 molecules of AB3 are formed. (c) AB2 is limiting, and 6 molecules of AB3 are formed. (d) AB2 is limiting, and 4 molecules of AB3 are formed
Verified step by step guidance1
Count the number of AB2 molecules in the diagram. Each AB2 molecule consists of one yellow sphere (A) and two blue spheres (B).
Count the number of B2 molecules in the diagram. Each B2 molecule consists of two blue spheres (B).
Determine the number of B atoms available from the B2 molecules by multiplying the number of B2 molecules by 2.
Determine the number of AB3 molecules that can be formed by using the available B atoms from both AB2 and B2 molecules. Each AB3 molecule requires one A atom and three B atoms.
Identify the limiting reactant by comparing the number of AB3 molecules that can be formed with the available A and B atoms. The reactant that runs out first is the limiting reactant.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Limiting Reactant
The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. In this scenario, identifying which reactant (AB2 or B2) is limiting is crucial for calculating the number of AB3 molecules produced.
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01:30
Limiting Reagent Concept
Stoichiometry
Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced chemical equations. Understanding the stoichiometric ratios between AB2 and B2 is essential to determine how many molecules of AB3 can be formed from the available reactants.
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01:16Stoichiometry Concept
Molecular Representation
Molecular representation uses symbols or diagrams to illustrate the composition and structure of molecules. In this question, the diagram shows the arrangement of A and B atoms, which helps visualize the reactants and their proportions, aiding in the identification of the limiting reactant and the amount of product formed.
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02:38Molecular Polarity
Related Practice
Textbook Question
What is the percent composition by mass of Mn in potas-sium permanganate, KMnO4? (LO 3.10) (a) 22.6%(b) 34.8%(c) 49.9% (d) 54.9%
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Textbook Question
Silver sulfide, the tarnish on silverware, comes from the reaction of silver metal with hydrogen sulfide (H2S).The unbalanced equation is: Ag + H2S + O2 --> Ag2S + H2O Unbalanced If the reaction was used intentionally to prepare Ag2S, how many grams would be formed from 496 g of Ag, 80.0 g of H2S, and excess O2 if the reaction takes place in 90% yield? (LO 3.9) (a) 525 g (b) 1139 g (c) 583 g (d) 1025
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Textbook Question
If 2.00 moles of nitrogen and 5.50 moles of hydrogen are placed in a reaction vessel and react to form ammonia, what is the theoretical yield of ammonia (NH3)? (LO 3.8) N2(g) + 3 H2(g) --> 2 NH3(g)(a) 31.2 g (b) 62.3 g(c) 93.7 g (d) 34.1
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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
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