Preview General, Organic, and Biological Chemistry Structures of Life, 5th Edition by Karen C. Timberlake (2014)

Preview General, Organic, and Biological Chemistry Structures of Life, 5th Edition by Karen C. Timberlake (2014) Preview General, Organic, and Biological Chemistry Structures of Life, 5th Edition by Karen C. Timberlake (2014) Preview General, Organic, and Biological Chemistry Structures of Life, 5th Edition by Karen C. Timberlake (2014) Preview General, Organic, and Biological Chemistry Structures of Life, 5th Edition by Karen C. Timberlake (2014) Preview General, Organic, and Biological Chemistry Structures of Life, 5th Edition by Karen C. Timberlake (2014)

General, Organic, and Biological Chemistry Structures of Life Fifth Edition GLOBAL EDITION Karen C Timberlake Contributions by Laura Frost, Ph.D Director, Whitaker Center for STEM Education Professor of Chemistry Florida Gulf Coast University Editor in Chief: Jeanne Zalesky Senior Acquisitions Editor: Terry Haugen Program Manager: Coleen Morrison Editorial Assistant: Caitlin Falco Assistant Acquisitions Editor, Global Edition: Murchana Borthakur Associate Project Editor, Global Edition: Binita Roy Director of Development: Jennifer Hart Product Marketing Manager: Will Moore Field Marketing Manager: Chris Barker Program Management Team Lead: Kristen Flathman Project Management Team Lead: David Zielonka Senior Project Manager: Jenna Vittorioso, Lumina Datamatics, Inc Copyeditor: Lumina Datamatics, Inc Compositor: Lumina Datamatics, Inc Art Coordinator: Wynne Au Yeung Design Manager: Derek Bacchus Interior Designer: Jerilyn Bockorick Cover Designer: Lumina Datamatics, Inc Illustrator: Imagineering Text Permissions Manager: William Opaluch Rights & Permissions Management: Rachel Youdelman Photo Researchers: Steve Merland and Jennifer Simmons Senior Specialist, Manufacturing: Maura Zaldivar-Garcia Senior Manufacturing Controller, Production, Global Edition: Trudy Kimber Cover Photo Credit: ©Iaryna Turchyniak >Shutterstock.com Acknowledgements of third party content appear on page 933, which constitutes an extension of this copyright page MasteringChemistry, is an exclusive trademark in the U.S and >or other countries owned by Pearson Education, Inc or its affiliates Unless otherwise indicated herein, any third-party trademarks that may appear in this work are the property of their respective owners and any references to third-party trademarks, logos or other trade dress are for demonstrative or descriptive purposes only Such references are not intended to imply any sponsorship, endorsement, authorization, or promotion of Pearson's products by the owners of such marks, or any relationship between the owner and Pearson Education, Inc or its affiliates, authors, licensees or distributors Pearson Education Limited Edinburgh Gate Harlow Essex CM20 2JE England and Associated Companies throughout the world Visit us on the World Wide Web at: www.pearsonglobaleditions.com © Pearson Education Limited 2016 The rights of Karen C Timberlake to be identified as the author of this work have been asserted by her in accordance with the Copyright, Designs and Patents Act 1988 Authorized adaptation from the United States edition, entitled General, Organic, and Biological Chemistry: Structures of Life, 5th edition, ISBN 978-0-321-96746-6, by Karen C Timberlake, published by Pearson Education © 2015 All rights reserved No part of this publication may be reproduced, stored in a retrieval system, or transmitted in any form or by any means, electronic, mechanical, photocopying, recording or otherwise, without either the prior written permission of the publisher or a license permitting restricted copying in the United Kingdom issued by the Copyright Licensing Agency Ltd, Saffron House, 6–10 Kirby Street, London EC1N 8TS All trademarks used herein are the property of their respective owners The use of any trademark in this text does not vest in the author or publisher any trademark ownership rights in such trademarks, nor does the use of such trademarks imply any affiliation with or endorsement of this book by such owners ISBN 10: 1-292-09619-5 ISBN 13: 978-1-292-09619-3 British Library Cataloguing-in-Publication Data A catalogue record for this book is available from the British Library 10 Typeset in 10 Times LT Std by Lumina Datamatics, Inc Printed and bound by CTPS in China Brief Contents Chemistry in Our Lives 33 Chemistry and Measurements 57 Matter and Energy 94 Atoms 133 Nuclear Chemistry 183 Ionic and Molecular Compounds 215 Chemical Reactions and Quantities 267 Gases 320 Solutions 356 10 Reaction Rates and Chemical Equilibrium 402 11 Acids and Bases 431 12 Introduction to Organic Chemistry: Hydrocarbons 475 13 Alcohols, Phenols, Thiols, and Ethers 520 14 Aldehydes, Ketones, and Chiral Molecules 548 15 Carbohydrates 582 16 Carboxylic Acids and Esters 612 17 Lipids 640 18 Amines and Amides 681 19 Amino Acids and Proteins 720 20 Enzymes and Vitamins 754 21 Nucleic Acids and Protein Synthesis 785 22 Metabolic Pathways for Carbohydrates 829 23 Metabolism and Energy Production 868 24 Metabolic Pathways for Lipids and Amino Acids 893  3 Contents Chemistry in Our Lives 33 Career: Forensic Scientist 33 1.1 Chemistry and Chemicals 34 1.2 Scientific Method: Thinking Like a Scientist 36 Explore Your World  Nobel Prize Winners in Chemistry 36 Chemistry Link to Health  Early Chemist: Paracelsus 37 1.3 Learning Chemistry: A Study Plan 38 1.4 Key Math Skills for Chemistry 41 Guide to Writing a Number in Scientific Notation  49 Clinical Applications  36, 38, 51 Clinical Update  Forensic Evidence Solves the Murder 51 Concept Map  51 Chapter Review  52 Key Terms  52 Key Math Skills  52 Understanding the Concepts  54 Additional Questions and Problems  54 Challenge Questions  55 Answers 56 Chemistry and Measure­ments 57 Career: Registered Nurse 57 2.1 Units of Measurement 58 Explore Your World  Units Listed on Labels 61 2.2 Measured Numbers and Significant Figures 62 2.3 Significant Figures in Calculations 64 2.4 Prefixes and Equalities 68 2.5 Writing Conversion Factors 71 Explore Your World  SI and Metric Equalities on Product Labels  72 2.6 Problem Solving Using Unit Conversion 76 Guide to Problem Solving Using Conversion Factors 76 Chemistry Link to Health  Toxicology and Risk–Benefit Assessment 79 2.7 Density 81 Explore Your World  Sink or Float 82 Chemistry Link to Health  Bone Density 83 Guide to Using Density  83 Clinical Applications  61, 64, 76, 80, 85, 91 Clinical Update  Greg’s Follow-Up Visit with His Doctor 85 Concept Map  86 Chapter Review  86 Key Terms  87 Key Math Skill  88 Core Chemistry Skills  88 Understanding the Concepts  89 Additional Questions and Problems  90 Challenge Questions  91 Answers 92 Matter and Energy 94 Career: Dietitian 94 3.1 Classification of Matter 95 Chemistry Link to Health  Breathing Mixtures 98 3.2 States and Properties of Matter 99 3.3 Temperature 101 Guide to Calculating Temperature  103 Chemistry Link to Health  Variation in Body Temperature 104 3.4 Energy 105 Contents  Chemistry Link to the Environment  Carbon Dioxide and Climate Change 107 3.5 Energy and Nutrition 108 Guide to Calculating the Energy from a Food  110 Explore Your World  Counting Calories 110 Chemistry Link to Health  Losing and Gaining Weight 110 3.6 Specific Heat 112 Guide to Calculations Using Specific Heat  113 3.7 Changes of State 113 Guide to Using a Heat Conversion Factor  115 Chemistry Link to Health  Steam Burns 118 Clinical Applications  105, 111, 122, 127, 128 Clinical Update  A Diet and Exercise Program for Charles 122 Concept Map  123 Chapter Review  123 Key Terms  124 Core Chemistry Skills  125 Understanding the Concepts  126 Additional Questions and Problems  127 Challenge Questions  129 Answers 129 Combining Ideas from Chapters to 3  131 Answers 132 Chemistry Link to the Environment  EnergySaving Fluorescent Bulbs 155 4.7 Electron Configurations 159 Guide to Drawing Orbital Diagrams  161 Guide to Writing Electron Configurations Using Sublevel Blocks  164 4.8 Trends in Periodic Properties 167 Clinical Applications  136, 142, 149, 173 Clinical Update  Improving Crop Production 173 Concept Map  174 Chapter Review  174 Key Terms  176 Core Chemistry Skills  177 Understanding the Concepts  178 Additional Questions and Problems  179 Challenge Questions  180 Answers 181 Nuclear Chemistry 183 Career: Nuclear Medicine Technologist 183 Atoms 133 5.1 Natural Radioactivity 184 5.2 Nuclear Reactions 188 Guide to Completing a Nuclear Equation  189 Chemistry Link to Health  Radon in Our Homes 189 5.3 Radiation Measurement 194 Career: Farmer 133 4.1 Elements and Symbols 134 Chemistry Link to Health  Latin Names for Elements in Clinical Usage 136 Chemistry Link to Health  Toxicity of Mercury 136 4.2 The Periodic Table 137 Chemistry Link to Health  Elements Essential to Health 140 4.3 The Atom 142 Explore Your World  Repulsion and Attraction 145 4.4 Atomic Number and Mass Number 146 Chemistry Link to the Environment  Many Forms of Carbon 148 4.5 Isotopes and Atomic Mass 149 Guide to Calculating Atomic Mass  152 4.6 Electron Energy Levels 153 Chemistry Link to Health  Biological Reactions to UV Light 154 Chemistry Link to Health  Radiation and Food 195 5.4 Half-Life of a Radioisotope 197 Guide to Using Half-Lives  198 Chemistry Link to the Environment  Dating Ancient Objects 199 5.5 Medical Applications Using Radioactivity 201 Chemistry Link to Health  Brachytherapy 203 5.6 Nuclear Fission and Fusion 204 Chemistry Link to the Environment  Nuclear Power Plants 207 Clinical Applications  187, 197, 201, 204, 208, 212, 213 Clinical Update  Cardiac Imaging Using a Radioisotope  208 Concept Map  208 Chapter Review  209 Key Terms  209 6 Contents Core Chemistry Skills  210 Understanding the Concepts  210 Additional Questions and Problems  211 Challenge Questions  212 Answers 213 Understanding the Concepts  259 Additional Questions and Problems  260 Challenge Questions  261 Answers 262 Combining Ideas from Chapters to 6  265 Answers 266 Ionic and Molecular Compounds 215 Career: Pharmacy Technician 215 6.1 Ions: Transfer of Electrons 216 Chemistry Link to Health  Some Important Ions in the Body 220 6.2 Writing Formulas for Ionic Compounds 221 6.3 Naming and Writing Ionic Formulas 224 Guide to Naming Ionic Compounds with Metals that Form a Single Ion  224 Guide to Naming Ionic Compounds with Variable Charge Metals  226 Guide to Writing Formulas from the Name of an Ionic Compound  227 6.4 Polyatomic Ions 228 Guide to Writing Formulas with Polyatomic Ions  230 Guide to Naming Ionic Compounds with Polyatomic Ions  231 6.5 Molecular Compounds: Sharing Electrons 232 Guide to Naming Molecular Compounds  233 Guide to Writing Formulas for Molecular Compounds  234 6.6 Lewis Structures for Molecules and Polyatomic Ions 236 Guide to Drawing Lewis Structures  238 6.7 Electronegativity and Bond Polarity 241 6.8 Shapes and Polarity of Molecules 244 Guide to Predicting Shape 1Vsepr Theory2  247 Guide to Determining the Polarity of a Molecule  249 6.9 Attractive Forces in Compounds 250 Chemistry Link to Health  Attractive Forces in Biological Compounds 252 Clinical Applications  221, 228, 232, 236, 254 Clinical Update  Compounds at the Pharmacy 254 Concept Map  255 Chapter Review  255 Key Terms  257 Core Chemistry Skills  257 Chemical Reactions and Quantities 267 Career: Dental Hygienist 267 7.1 Equations for Chemical Reactions 268 Guide to Balancing a Chemical Equation  272 7.2 Types of Reactions 275 Chemistry Link to Health  Incomplete Combustion: Toxicity of Carbon Monoxide 279 7.3 Oxidation–Reduction Reactions 280 Explore Your World  Oxidation of Fruits and Vegetables 282 7.4 The Mole 283 Guide to Calculating the Atoms or Molecules of a Substance  285 Guide to Calculating the Moles of an Element in a Compound  286 7.5 Molar Mass and Calculations 287 Guide to Calculating Molar Mass  288 Explore Your World  Calculating Moles in the Kitchen 288 Guide to Calculating the Moles 1or Grams2 of a Substance from Grams 1or Moles2  290 7.6 Mole Relationships in Chemical Equations 292 Guide to Calculating the Quantities of Reactants and Products in a Chemical Reaction  294 7.7 Mass Calculations for Reactions 295 7.8 Limiting Reactants and Percent Yield 297 Guide to Calculating the Moles of Product from a Limiting Reactant  298 Guide to Calculating the Grams of Product from a Limiting Reactant  299 Guide to Calculations for Percent Yield  301 7.9 Energy in Chemical Reactions 303 Guide to Calculating Using the Heat of Reaction  305 Chemistry Link to Health  Cold Packs and Hot Packs 305 Clinical Applications  275, 283, 287, 291, 297, 306, 307, 316 Clinical Update  Whitening of Tooth Enamel 307 Contents  Concept Map  308 Chapter Review  308 Key Terms  309 Core Chemistry Skills  310 Understanding the Concepts  312 Additional Questions and Problems  315 Challenge Questions  317 Answers 318 Solutions 356 Career: Dialysis Nurse 356 9.1 Solutions 357 Gases 320 Career: Respiratory Therapist 320 8.1 Properties of Gases 321 Explore Your World  Forming a Gas 323 Chemistry Link to Health  Measuring Blood Pressure 326 8.2 Pressure and Volume 1Boyle’s Law2 327 Guide to Using the Gas Laws  328 Chemistry Link to Health  Pressure–Volume Relationship in Breathing 328 Temperature and Volume 1Charles’s Law2 330 Temperature and Pressure 1Gay-Lussac’s Law2 332 The Combined Gas Law 335 Volume and Moles 1Avogadro’s Law2 336 Guide to Using Molar Volume  339 8.7 The Ideal Gas Law 340 Guide to Using the Ideal Gas Law  341 8.3 8.4 8.5 8.6 Chemistry Link to Health  Hyperbaric Chambers 342 Guide to Using the Ideal Gas Law for Reactions  343 8.8 Partial Pressures 1Dalton’s Law2 344 Guide to Calculating Partial Pressure  345 Chemistry Link to Health  Blood Gases 346 Clinical Applications  326, 329, 334, 344, 346, 347, 352 Clinical Update  Exercise-Induced Asthma 347 Concept Map  347 Chapter Review  348 Key Terms  349 Core Chemistry Skills  349 Understanding the Concepts  350 Additional Questions and Problems  351 Challenge Questions  352 Answers 352 Combining Ideas from Chapters and 8  354 Answers 355 Chemistry Link to Health  Water in the Body 359 Explore Your World  Live Dissolves Like 360 9.2 Electrolytes and Nonelectrolytes 361 Chemistry Link to Health  Electrolytes in Body Fluids 363 9.3 Solubility 365 Chemistry Link to Health  Gout and Kidney Stones: A Problem of Saturation in Body Fluids 366 Explore Your World  Preparing Rock Candy 367 Explore Your World  Preparing Solutions 368 Guide to Writing an Equation for the Formation of an Insoluble Ionic Compound  370 9.4 Solution Concentrations and Reactions 371 Guide to Calculating Solution Concentration  372 Guide to Using Concentration to Calculate Mass or Volume  376 Guide to Calculations Involving Solutions in Chemical Reactions  377 9.5 Dilution of Solutions 381 Guide to Calculating Dilution Quantities  382 9.6 Properties of Solutions 384 Chemistry Link to Health  Colloids and Solutions in the Body 385 Guide to Calculating Freezing Point Lowering>Boiling Point Elevation  387 Explore Your World  Everyday Osmosis 388 Guide to Calculating Osmolarity  389 Chemistry Link to Health  Dialysis by the Kidneys and the Artificial Kidney 391 Clinical Applications  361, 365, 380, 383, 393, 399, 400 Clinical Update  Using Dialysis for Renal Failure 393 Concept Map  394 Chapter Review  394 Key Terms  395 Core Chemistry Skills  396 Understanding the Concepts  397 Additional Questions and Problems  398 Challenge Questions  399 Answers 400 8 Contents 10 Reaction Rates and Chemical Equilibrium 402 Career: Neonatal Nurse 402 10.1 Rates of Reactions 404 Chemistry Link to the Environment  Catalytic Converters 407 10.2 Chemical Equilibrium 409 10.3 Equilibrium Constants 412 Guide to Writing the Equilibrium Constant Expression  413 Guide to Calculating the Kc Value  414 10.4 Using Equilibrium Constants 415 Guide to Using the Equilibrium Constant  417 10.5 Changing Equilibrium Conditions: Le Châtelier’s Principle 419 Chemistry Link to Health  Oxygen– Hemoglobin Equilibrium and Hypoxia 421 Chemistry Link to Health  Homeostasis: Regulation of Body Temperature 424 Clinical Applications  425 Clinical Update  An Iron-Rich Diet for Children’s Anemia 425 Concept Map  426 Chapter Review  426 Key Terms  427 Core Chemistry Skills  427 Understanding the Concepts  428 Additional Questions and Problems  428 Challenge Questions  429 Answers 430 11 Acids and Bases 431 Career: Clinical Laboratory Technician 431 11.1 Acids and Bases 432 11.2 Brønsted–Lowry Acids and Bases 435 Guide to Writing Conjugate Acid–Base Pairs  437 11.3 Strengths of Acids and Bases 438 11.4 Dissociation Constants for Acids and Bases 443 11.5 Dissociation of Water 445 Guide to Calculating 3H3O+4 and 3OH-4 in Aqueous Solutions  447 11.6 The pH Scale 448 guide to Calculating pH of an Aqueous Solution  451 Guide to Calculating 3H3O+4 from pH  453 Chemistry Link to Health  Stomach Acid, HCI 454 11.7 Reactions of Acids and Bases 455 Guide to Balancing an Equation for Neutralization  456 Chemistry Link to Health  Antacids 456 11.8 Acid–Base Titration 457 Guide to Calculations for an Acid–Base Titration  458 11.9 Buffers 459 Guide to Calculating pH of a Buffer  461 Chemistry Link to Health  Buffers in the Blood Plasma 462 Clinical Applications  448, 454, 464, 469, 470, 473 Clinical Update  Acid Reflux Disease 464 Concept Map  465 Chapter Review  465 Key Terms  466 Key Math Skills  467 Core Chemistry Skills  467 Understanding the Concepts  468 Additional Questions and Problems  469 Challenge Questions  470 Answers 471 Combining Ideas from Chapters to 11  473 Answers 474 12 Introduction to Organic Chemistry: Hydrocarbons 475 Career: Firefighter>Emergency Medical Technician 475 12.1 Organic Compounds  476 12.2 Alkanes 479 Guide to Drawing Structural Formulas for Alkanes  480 12.3 Alkanes with Substituents 483 Guide to Naming Alkanes with Substituents  486 Guide to Drawing Structural Formulas for Alkanes with Substituents  487 Contents  12.4 Properties of Alkanes 489 12.5 Alkenes and Alkynes 492 Explore Your World  Ripening Fruit 493 Guide to Naming Alkenes and Alkynes  493 Chemistry Link to the Environment  Fragrant Alkenes 495 12.6 Cis–Trans Isomers 496 Explore Your World  Modeling Cis–Trans Isomers 497 Chemistry Link to the Environment  Pheromones in Insect Communication 498 Chemistry Link to Health  Cis-Trans Isomers for Night Vision 499 12.7 Addition Reactions for Alkenes 500 Explore Your World  Unsaturation in Fats and Oils 500 Chemistry Link to Health  Hydrogenation of Unsaturated Fats 501 Explore Your World  Polymers and Recycling Plastics 504 12.8 Aromatic Compounds 505 Chemistry Link to Health  Some Common Aromatic Compounds in Nature and Medicine 507 Chemistry Link to Health  Polycyclic Aromatic Hydrocarbons 1PAHs2 509 Clinical Applications  509 Clinical Update  Diane’s Treatment in the Burn Unit 509 Concept Map  510 Chapter Review  511 Summary of Naming  512 Summary of Reactions  512 Key Terms  513 Core Chemistry Skills  513 Understanding the Concepts  514 Additional Questions and Problems  515 Challenge Questions  517 Answers 517 13 Alcohols, Phenols, Thiols, and Ethers 520 Career: Nurse Anesthetist 520 13.1 Alcohols, Phenols, and Thiols 521 Guide to Naming Alcohols and Phenols  523 Explore Your World  Alcohols in Household Products 523 Chemistry Link to Health  Some Important Alcohols and Phenols 524 13.2 Ethers 527 Guide to Writing Iupac Names for Ethers  528 Chemistry Link to Health  Ethers as Anesthetics 528 13.3 Physical Properties of Alcohols, Phenols, and Ethers 529 Chemistry Link to Health  Hand Sanitizers and Ethanol 532 13.4 Reactions of Alcohols and Thiols 533 Chemistry Link to Health  Methanol Poisoning 535 Chemistry Link to Health  Oxidation of Alcohol in the Body 537 Clinical Applications  539, 544 Clinical Update  Janet’s New Diet Plan 539 Concept Map  540 Chapter Review  540 Summary of Naming  541 Summary of Reactions  541 Key Terms  541 Core Chemistry Skills  542 Understanding the Concepts  542 Additional Questions and Problems  543 Challenge Questions  545 Answers 545 14 Aldehydes, Ketones, and Chiral Molecules 548 Career: Dermatology Nurse 548 14.1 Aldehydes and Ketones 549 Guide to Naming Aldehydes  550 Guide to Naming Ketones  552 Chemistry Link to Health  Some Important Aldehydes and Ketones 553 14.2 Physical Properties of Aldehydes and Ketones 555 14.3 Oxidation and Reduction of Aldehydes and Ketones 557 14.4 Hemiacetals and Acetals 559 14.5 Chiral Molecules 563 Explore Your World  Using Gumdrops and Toothpicks to Model Chiral Objects 565 118  Chapter 3  Matter and Energy Step Set up the problem and calculate the needed quantity Three SFs 122 g H2O Three SFs * 2260 J g H2O Exact * Exact kJ 1000 J = Exact 276 kJ Three SFs Study Check 3.9 When steam from a pan of boiling water reaches a cool window, it condenses How much heat, in kilojoules, is released when 25.0 g of steam condenses at 100 °C? Answer 56.5 kJ released Chemistry Link to Health Steam Burns Hot water at 100 °C will cause burns and damage to the skin However, getting steam on the skin is even more dangerous If 25 g of hot water at 100 °C falls on a person’s skin, the temperature of the water will drop to body temperature, 37 °C The heat released during cooling can cause severe burns The amount of heat can be calculated from the mass, the temperature change, 100 °C - 37 °C = 63 °C, and the specific heat of water, 4.184 J>g °C 25 g * 63 °C * 4.184 J = 6600 J of heat released when g °C water cools However, getting steam on the skin is even more damaging The condensation of the same quantity of steam to liquid at 100 °C releases much more heat—almost ten times as much This amount of heat can be calculated using the heat of vaporization, which is 2260 J> g for water at 100 °C 25 g * 2260 J = 57 000 J released when water 1gas2 1g condenses to water 1liquid2 at 100 °C The total heat released is calculated by combining the heat from the condensation at 100 °C and the heat from cooling of the steam from 100 °C to 37 °C 1body temperature2 We can see that most of the heat is from the condensation of steam This large amount of heat ­released on the skin is what causes damage from steam burns Condensation 1100 °C2 = 57 000 J Heat released = 64 000 J 1rounded off2 Cooling 1100 °C to 37 °C2 = 600 J The amount of heat released from steam is almost ten times greater than the heat from the same amount of hot water H2O steam HEAT H2O liquid When g of steam condenses, 2260 J is released 3.7  Changes of State  119 Heating and Cooling Curves All the changes of state during the heating or cooling of a substance can be illustrated visually On a heating curve or cooling curve, the temperature is shown on the vertical axis and the loss or gain of heat is shown on the horizontal axis Steps on a Heating Curve The first diagonal line indicates a warming of a solid as heat is added When the melting temperature is reached, a horizontal line, or plateau, indicates that the solid is melting As melting takes place, the solid is changing to liquid without any change in temperature 1see Figure 3.82 160 120 Boiling Gas Temperature 1°C2 100 80 60 Liquid 40 Melting -20 -40 Solid Heat Absorbed Once all the particles are in the liquid state, heat that is added will increase the temperature of the liquid This increase is drawn as a diagonal line from the melting point temperature to the boiling point temperature Once the liquid reaches its boiling point, a horizontal line indicates that the temperature is constant as liquid changes to gas Because the heat of vaporization is greater than the heat of fusion, the horizontal line at the boiling point is longer than the line at the melting point Once all the liquid becomes gas, adding more heat increases the temperature of the gas Steps on a Cooling Curve A cooling curve is a diagram of the cooling process in which the temperature decreases as heat is removed Initially, a diagonal line to the boiling 1condensation2 point is drawn to show that heat is removed from a gas until it begins to condense At the boiling 1condensation2 point, a horizontal line is drawn that indicates a change of state as gas condenses to form a liquid After all the gas has changed into liquid, further cooling lowers the temperature The decrease in temperature is shown as a diagonal line from the condensation temperature to the freezing temperature At the freezing point, another horizontal line indicates that liquid is changing to solid at the freezing point temperature Once all the substance is frozen, the removal of more heat decreases the temperature of the solid below its freezing point, which is shown as a diagonal line below its freezing point Figure 3.8 ▶ A heating curve diagrams the temperature increases and changes of state as heat is added Q What does the plateau at 100 °C represent on the heating curve for water? 140 Steam 120 Water + steam 100 Condensation 80 Water 60 40 Water + 20 ice Freezing -20 Ice Temperature 1°C2 20 Heat Removed A cooling curve for water illustrates the change in temperature and changes of state as heat is removed 120  Chapter 3  Matter and Energy ▶▶Sample Problem 3.10  Using a Cooling Curve Using the cooling curve for water, identify the state or change of state for water as solid, liquid, gas, condensation, or freezing a at 120 °C b at 100 °C c at 40 °C Solution a A temperature of 120 °C occurs on the diagonal line above the boiling 1condensation2 point, which indicates that water is a gas b A temperature of 100 °C, shown as a horizontal line, indicates that the water vapor is changing to liquid water, or condensing c A temperature of 40 °C occurs on the diagonal line below the boiling point but above the freezing point, which indicates that the water is in the liquid state Study Check 3.10 Using the cooling curve for water, identify the state or change of state for water as solid, liquid, gas, condensation, or freezing a at °C b at -20 °C Answer a freezing b solid Combining Energy Calculations Up to now, we have calculated one step in a heating or cooling curve However, many problems require a combination of steps that include a temperature change as well as a change of state The heat is calculated for each step separately and then added together to find the total energy, as seen in Sample Problem 3.11 ▶▶Sample Problem 3.11  Combining Heat Calculations Charles has increased his activity by doing more exercise After a session of using small weights, he has a sore arm An ice bag is filled with 125 g of ice at 0.0 °C The heat of fusion for ice is 334 J >g How much heat, in kilojoules, is absorbed to melt the ice, and to raise the temperature of the water to body temperature, 37.0 °C? Solution Step State the given and needed quantities Analyze the Problem Given Need 125 g of ice at 0.0 °C, heat of fusion of ice = 334 J>g total kilojoules to melt ice at 0.0 °C and to raise temperature of water to 37.0 °C Step Write a plan to convert the given quantity to the needed quantity Total heat = kilojoules needed to melt the ice and heat the water from 0.0 °C 1freezing point2 to 37.0 °C Step Write the heat conversion factor and any metric factor g of H2O1s 334 J g H 2O and l2 = 334 J g H2O 334 J SHwater = 4.184 J g °C 4.184 J g °C and g °C 4.184 J kJ = 1000 J 1000 J kJ and kJ 1000 J 3.7  Changes of State  121 Step Set up the problem and calculate the needed quantity ∆T = 37.0 °C - 0.0 °C = 37.0 °C Heat needed to change ice 1solid2 to water 1liquid2 at 0.0 °C: Exact Three SFs 334 J g ice 125 g ice * Three SFs kJ 1000 J * = 41.8 kJ Exact Exact Three SFs Heat needed to warm water 1liquid2 from 0.0 °C to water 1liquid2 at 37.0 °C: Exact 125 g * 37.0 °C * Three SFs Three SFs 4.184 J g °C Calculate the total heat: Melting ice at 0.0 °C Heating water 10.0 °C to 37.0 °C2 Total heat needed Exact kJ 1000 J * Exact = 19.4 kJ Three SFs 41.8 kJ 19.4 kJ 61.2 kJ Study Check 3.11 How many kilojoules are released when 75.0 g of steam at 100 °C condenses, cools to °C, and freezes at °C? 1Hint: The solution will require three energy calculations.2 Answer 226 kJ Questions and Problems 3.7 Changes of State Learning Goal  Describe the changes of state between solids, liquids, and gases; calculate the energy involved 3.41 Identify each of the following changes of state as melting, freezing, sublimation, or deposition: a The solid structure of a substance breaks down as liquid forms b Coffee is freeze-dried c Water on the street turns to ice during a cold wintry night d Ice crystals form on a package of frozen corn 3.42 Identify each of the following changes of state as melting, freezing, sublimation, or deposition: a Dry ice in an ice-cream cart disappears b Snow on the ground turns to liquid water c Heat is removed from 125 g of liquid water at °C d Frost 1ice2 forms on the walls of a freezer unit of a refrigerator 3.43 Calculate the heat change at °C for each of the following, and indicate whether heat was absorbed or released: a calories to melt 65 g of ice b joules to melt 17.0 g of ice c kilocalories to freeze 225 g of water d kilojoules to freeze 50.0 g of water 3.44 Calculate the heat change at °C for each of the following, and indicate whether heat was absorbed or released: a calories to freeze 35 g of water b joules to freeze 275 g of water c kilocalories to melt 140 g of ice d kilojoules to melt 5.00 g of ice 3.45 Identify each of the following changes of state as evaporation, boiling, or condensation: a The water vapor in the clouds changes to rain b Wet clothes dry on a clothesline c Lava flows into the ocean and steam forms d After a hot shower, your bathroom mirror is covered with water 3.46 Identify each of the following changes of state as evaporation, boiling, or condensation: a At 100 °C, the water in a pan changes to steam b On a cool morning, the windows in your car fog up c A shallow pond dries up in the summer d Your teakettle whistles when the water is ready for tea 3.47 Calculate the heat change at 100 °C for each of the following, and indicate whether heat was absorbed or released: a calories to vaporize 10.0 g of water b joules to vaporize 5.00 g of water c kilocalories to condense 8.0 kg of steam d kilojoules to condense 175 g of steam 3.48 Calculate the heat change at 100 °C for each of the following, and indicate whether heat was absorbed or released: a calories to condense 10.0 g of steam b joules to condense 7.60 g of steam c kilocalories to vaporize 44 g of water d kilojoules to vaporize 5.00 kg of water 122  Chapter 3  Matter and Energy 3.49 Draw a heating curve for a sample of ice that is heated from - 20 °C to 150 °C Indicate the segment of the graph that corresponds to each of the following: a solid b melting c liquid e gas d boiling 3.50 Draw a cooling curve for a sample of steam that cools from 110 °C to - 10 °C Indicate the segment of the graph that corresponds to each of the following: a solid b freezing c liquid e gas d condensation 3.51 Using the values for the heat of fusion, specific heat of water, and>or heat of vaporization, calculate the amount of heat energy in each of the following: a joules needed to melt 50.0 g of ice at °C and to warm the liquid to 65.0 °C b kilocalories released when 15.0 g of steam condenses at 100 °C and the liquid cools to °C c kilojoules needed to melt 24.0 g of ice at °C, warm the liquid to 100 °C, and change it to steam at 100 °C Px 3.52 Using the values for the heat of fusion, specific heat of water, and>or heat of vaporization, calculate the amount of heat energy in each of the following: a joules released when 125 g of steam at 100 °C condenses and cools to liquid at 15.0 °C b kilocalories needed to melt a 525-g ice sculpture at °C and to warm the liquid to 15.0 °C c kilojoules released when 85.0 g of steam condenses at 100 °C, cools, and freezes at °C Px Clinical Applications 3.53 A patient arrives in the emergency room with a burn caused by steam Calculate the heat, in kilocalories, that is released when 18.0 g of steam at 100 °C hits the skin, condenses, and cools to body temperature of 37.0 °C 3.54 A sports trainer applies an ice bag to the back of an injured athlete Calculate the heat, in kilocalories, that is absorbed if 145 g of ice at 0.0 °C is placed in an ice bag, melts, and rises to body temperature of 37.0 °C Clinical Update A Diet and Exercise Program for Charles It has been two weeks since Charles met with Daniel, a dietitian, who provided Charles with a menu for weight loss Charles and his mother are going back to see Daniel again with a chart of the food Charles has eaten The following is what Charles ate in one day: Breakfast banana, cup of nonfat milk, egg Lunch cup of carrots, oz of ground beef, apple, cup of nonfat milk Dinner oz of skinless chicken, baked potato, oz of broccoli, cup of nonfat milk Px Clinical Applications 3.55 Using energy values from Table 3.8, determine each of the following: a the total kilocalories for each meal b the total kilocalories for one day c If Charles consumes 1800 kcal per day, he will maintain his weight Would he lose weight on his new diet? d If the loss of 3500 kcal is equal to a loss of 1.0 lb, how many days will it take Charles to lose 5.0 lb? 3.56 a During one week, Charles swam for a total of 2.5 h and walked for a total of 8.0 h If Charles expends 340 kcal>h swimming and 160 kcal>h walking, how many total kilocalories did he expend for one week? b For the amount of exercise that Charles did for one week in part a, how much weight, in pounds, did he lose? c How many hours would Charles have to walk to lose 1.0 lb? d H  ow many hours would Charles have to swim to lose 1.0 lb? Concept Map MATTER AND ENERGY Solid Matter Energy has states of affects Liquid can be Gas Particle Motion undergo as Pure Substances Mixtures Changes of State Heat that are that are gain>loss of heat during measured in Elements Homogeneous Melting or Freezing Calories or Joules or or Compounds Heterogeneous using Boiling or Condensation require Temperature Change Specific Heat Heat of Fusion Mass Heat of Vaporization are drawn as a Heating or Cooling Curve Chapter Review 3.1 Classification of Matter Learning Goal  Classify exam- 3.2 States and Properties of Matter Learning Goal  Identify the ples of matter as pure substances or mixtures • Matter is anything that has mass and ­occupies space • Matter is classified as pure substances or mixtures • Pure substances, which are elements or compounds, have fixed compositions, and mixtures have variable compositions • The substances in mixtures can be separated using physical methods states and the physical and chemical properties of matter • The three states of matter are solid, liquid, and gas • A physical property is a characteristic of a substance in that it can be observed or measured without ­affecting the identity of the substance • A physical change occurs when physical properties change, but not the composition of the substance • A chemical property indicates the ability of a substance to change into another substance • A chemical change occurs when one or more substances react to form a substance with new physical and chemical properties 124  Chapter 3  Matter and Energy 3.3 Temperature Learning Goal  Given a temperature, °C 3.6 Specific Heat Learning Goal  Use spe- °F calculate a corresponding temperature on another scale • In science, temperature is measured in degrees Celsius 1°C2 or kelvins 1K2 • On the Celsius scale, there are 100 units ­between the freezing point 10 °C2 and the boiling point 1100 °C2 of water • On the Fahrenheit scale, there are 180 units ­between the freezing point 132 °F2 and the boiling point 1212 °F2 of water A Fahrenheit temperature is related to its Celsius temperature by the equation TF = 1.81TC2 + 32 • The SI unit, kelvin, is related to the Celsius temperature by the equation TK = TC + 273 42.0 107.6 41.0 105.8 40.0 104.0 39.0 102.2 38.0 100.4 37.0 98.6 36.0 96.8 35.0 95.0 34.0 93.2 Death Hyperthermia Fever Normal Average range Hypothermia 3.4 Energy Learning Goal  Identify energy as potential or kinetic; convert between units of ­energy • Energy is the ability to work • Potential energy is stored ­energy; kinetic energy is the ­energy of motion • Common units of energy are the calorie 1cal2, kilocalorie 1kcal2, joule 1J2, and kilojoule 1kJ2 • One calorie is equal to 4.184 J 3.5 Energy and Nutrition Learning Goal  Use the ­ nergy values to calculate the e ­kilocalories 1kcal2 or kilojoules 1kJ2 for a food • The nutritional Calorie is the same amount of energy as kcal or 1000 calories • The energy of a food is the sum of ­kilocalories or kilojoules from ­carbohydrate, fat, and protein Snack Snack Crackers Crackers Nutrition Facts Serving Size 14 crackers 131g2 Servings Per Container About Amount Per Serving Calories 130 Calories from Fat 40 150 Kilojoules 500 kJ from Fat cific heat to calculate heat loss or gain • Specific heat is the amount of ­energy required to raise the ­temperature of exactly g of a substance by exactly °C • The heat lost or gained by a ­substance is determined by ­multiplying its mass, the temperature change, and its specific heat 3.7 Changes of State Learning Goal  Describe Solid + Heat Liquid Melting the changes of state between solids, liquids, and gases; calculate the energy involved F r e e zi n g • Melting occurs when the particles - Heat in a solid absorb enough energy to break apart and form a liquid • The amount of energy required to convert exactly g of solid to liquid is called the heat of fusion • For water, 80 cal 1334 J2 is needed to melt g of ice or must be ­removed to freeze g of water • Evaporation occurs when particles in a liquid state absorb enough energy to break apart and form gaseous particles • Boiling is the vaporization of liquid at its boiling point The heat of vaporization is the amount of heat needed to convert exactly g of liquid to vapor • For water, 540 cal 12260 J2 is needed to vaporize g of water or must be removed to condense g of steam • A heating or cooling curve illustrates the changes in temperature and state as heat is added to or removed from a substance Plateaus on the graph indicate changes of state • The total heat absorbed or removed from a substance undergoing temperature changes and changes of state is the sum of energy calculations for change1s2 of state and change1s2 in temperature • Sublimation is a process whereby a solid changes directly to a gas Key Terms boiling  The formation of bubbles of gas throughout a liquid boiling point 1bp2   The temperature at which a liquid changes to gas 1boils2 and gas changes to liquid 1condenses2 calorie 1cal2   The amount of heat energy that raises the temperature of exactly g of water by exactly °C change of state  The transformation of one state of matter to another; for example, solid to liquid, liquid to solid, liquid to gas chemical change  A change during which the original substance is converted into a new substance that has a different composition and new physical and chemical properties chemical properties  The properties that indicate the ability of a ­substance to change into a new substance compound  A pure substance consisting of two or more elements, with a definite composition, that can be broken down into simpler substances only by chemical methods condensation  The change of state from a gas to a liquid cooling curve  A diagram that illustrates temperature changes and changes of state for a substance as heat is removed deposition  The change of a gas directly into a solid; the reverse of sublimation element  A pure substance containing only one type of matter, which cannot be broken down by chemical methods energy  The ability to work energy value  The kilocalories 1or kilojoules2 obtained per gram of the food types: carbohydrate, fat, and protein evaporation  The formation of a gas 1vapor2 by the escape of high- energy molecules from the surface of a liquid freezing  The change of state from liquid to solid freezing point 1fp2   The temperature at which a liquid changes to a solid 1freezes2, a solid changes to a liquid 1melts2 gas  A state of matter that does not have a definite shape or volume heat  The energy associated with the motion of particles in a substance heat of fusion  The energy required to melt exactly g of a substance at its melting point For water, 80 cal 1334 J2 is needed to melt g of ice; 80 cal 1334 J2 is released when g of water freezes Core Chemistry Skills  heat of vaporization  The energy required to vaporize exactly g of a substance at its boiling point For water, 540 cal 12260 J2 is needed to vaporize g of liquid; g of steam gives off 540 cal 12260 J2 when it condenses heating curve  A diagram that illustrates the temperature changes and changes of state of a substance as it is heated joule 1J2   The SI unit of heat energy; 4.184 J = cal kinetic energy  The energy of moving particles liquid  A state of matter that takes the shape of its container but has a definite volume matter  The material that makes up a substance and has mass and ­occupies space melting  The change of state from a solid to a liquid melting point 1mp2   The temperature at which a solid becomes a liquid 1melts2 It is the same temperature as the freezing point 125 mixture  The physical combination of two or more substances that does not change the identities of the mixed substances physical change  A change in which the physical properties of a sub- stance change but its identity stays the same physical properties  The properties that can be observed or measured without affecting the identity of a substance potential energy  A type of energy related to position or composition of a substance pure substance  A type of matter that has a definite composition solid  A state of matter that has its own shape and volume specific heat 1SH2   A quantity of heat that changes the temperature of exactly g of a substance by exactly °C states of matter  Three forms of matter: solid, liquid, and gas sublimation  The change of state in which a solid is transformed ­directly to a gas without forming a liquid first Core Chemistry Skills b.  When methane burns, it changes to different substances with new properties, which is a chemical property c.  The odor of hydrogen sulfide is a physical property The chapter section containing each Core Chemistry Skill is shown in parentheses at the end of each heading Classifying Matter 13.12 • A pure substance is matter that has a fixed or constant composition • An element, the simplest type of a pure substance, is composed of only one type of matter, such as silver, iron, or aluminum • A compound is also a pure substance, but it consists of two or more elements chemically combined in the same proportion • In a homogeneous mixture, also called a solution, the composition of the substances in the mixture is uniform • In a heterogeneous mixture, the components are visible and not have a uniform composition throughout the sample Example: Classify each of the following as a pure substance 1element or compound2 or a mixture 1homogeneous or heterogeneous2: a.  iron in a nail b.  black coffee c.  carbon dioxide, a greenhouse gas Answer: a.  Iron is a pure substance, which is an element b.  Black coffee contains different substances with uniform composition, which makes it a homogeneous mixture c. The gas carbon dioxide, which is a pure substance that contains two elements chemically combined, is a compound Identifying Physical and Chemical Changes 13.22 • When matter undergoes a physical change, its state or its appearance changes, but its composition remains the same • When a chemical change takes place, the original substance is converted into a new substance, which has different physical and chemical properties Example: Classify each of the following as a physical or chemical property: a.  Helium in a balloon is a gas b.  Methane, in natural gas, burns c.  Hydrogen sulfide smells like rotten eggs Answer: a.  A gas is a state of matter, which makes it a physical property Converting between Temperature Scales 13.32 • The temperature equation TF = 1.81TC2 + 32 is used to convert from Celsius to Fahrenheit and can be rearranged to convert from Fahrenheit to Celsius • The temperature equation TK = TC + 273 is used to convert from Celsius to Kelvin and can be rearranged to convert from Kelvin to Celsius Example: Convert 75.0 °C to degrees Fahrenheit Answer: TF = 1.81TC2 + 32 TF = 1.8175.02 + 32 = 135 + 32 = 167 °F Example: Convert 355 K to degrees Celsius Answer: TK = TC + 273 To solve the equation for TC, subtract 273 from both sides TK - 273 = TC + 273 - 273 TC = TK - 273 TC = 355 - 273 = 82 °C Using Energy Units 13.42 • Equalities for energy units include cal = 4.184 J, kcal = 1000 cal, and kJ = 1000 J • Each equality for energy units can be written as two conversion factors: 4.184 J cal and cal 4.184 J 1000 cal kcal and kcal 1000 cal 1000 J kJ and kJ 1000 J • The energy unit conversion factors are used to cancel given units of energy and to obtain the needed unit of energy Example: Convert 45 000 J to kilocalories Answer: Using the conversion factors above, we start with the given 45 000 J and convert it to kilocalories 45 000 J * cal kcal * = 11 kcal 4.184 J 1000 cal 126  Chapter 3  Matter and Energy Example: How many joules are required to heat 5.25 g of titanium Using the Heat Equation 13.62 • The quantity of heat absorbed or lost by a substance is calculated using the heat equation Heat = m * ∆T * SH • Heat, in joules, is obtained when the specific heat of a substance in J>g °C is used • To cancel, the unit grams is used for mass, and the unit °C is used for temperature change from 85.5 °C to 132.5 °C? Answer: m = 5.25 g, ∆T = 132.5 °C - 85.5 °C = 47.0 °C SH for titanium = 0.523 J>g °C The known values are substituted into the heat equation making sure units cancel Heat = m * ∆T * SH = 5.25 g * 47.0 °C * 0.523 J g °C = 129 J Understanding the Concepts The chapter sections to review are shown in parentheses at the end of each question 3.57 Identify each of the following as an element, a compound, or a mixture Explain your choice 13.12 a b 3.61 State the temperature on the Celsius thermometer and convert to Fahrenheit 13.32 70 60 50 3.62 State the temperature on the Celsius thermometer and convert to Fahrenheit 13.32 c 54 3.58 Identify each of the following as a homogeneous or heterogeneous mixture Explain your choice 13.12 a b 52 3.63 Compost can be made at home from grass clippings, some kitchen scraps, and dry leaves As microbes break down organic matter, heat is generated and the compost can reach a temperature of 155 °F, which kills most pathogens What is this temperature in degrees Celsius? In kelvins? 13.32    c 3.59 Classify each of the following as a homogeneous or heterogeneous mixture: 13.12 a pulpy orange juice b cereal in milk c copper sulphate in water 3.60 Classify each of the following as a homogeneous or heterogeneous mixture: 13.12 a noodle soup   b.  pizza           c.  ketchup    53        Compost produced from decayed plant material is used to enrich the soil 3.64 In a chemical reaction, a mixture of salicylic acid and methanol was heated at 90 °C for two hours After completion of the reaction, the mixture is cooled to 30 °C What is this temperature in degrees Fahrenheit? In kelvins? 13.32 3.65 Calculate the energy to heat two cubes 1gold and aluminum2 each with a volume of 20.0 cm3 from 25 °C to 35 °C Refer to Tables 2.9 and 3.11 13.62 Additional Questions and Problems  3.66 Calculate the energy to heat two cubes 1silver and copper2, each with a volume of 10.0 cm3 from 15 °C to 25 °C Refer to Tables 2.9 and 3.11 13.62 Px Clinical Applications 3.67 A 70.0-kg person had a quarter-pound cheeseburger, french fries, and a chocolate shake 13.52 Carbohydrate 1g2 46 Fat 1g2 40 Protein 1g2 47 French fries 47 16  4 Chocolate shake 76 10 10 Item Cheeseburger 127 a Using Table 3.7, calculate the total kilocalories for each food type in this meal 1round off the kilocalories to the tens place2 b Determine the total kilocalories for the meal 1round off to the tens place2 c Using Table 3.10, determine the number of hours of sleep needed to burn off the kilocalories in this meal d Using Table 3.10, determine the number of hours of running needed to burn off the kilocalories in this meal 3.68 Your friend, who has a mass of 70.0 kg, has a slice of pizza, a cola soft drink, and ice cream 13.52 Pizza Carbohydrate 1g2 29 Fat 1g2 10 Protein 1g2 Cola 51  0  0 Ice cream 44 28  8 Item 13 a Using Table 3.7, calculate the total kilocalories for each food type in this meal 1round off the kilocalories to the tens place2 b Determine the total kilocalories for the meal 1round off to the tens place2 c Using Table 3.10, determine the number of hours of sitting needed to burn off the kilocalories in this meal d Using Table 3.10, determine the number of hours of swimming needed to burn off the kilocalories in this meal Additional Questions and Problems 3.69 Classify each of the following as an element, a compound, or a mixture: 13.12 a iron filings in concrete b sodium carbonate in soap c air in the atmosphere 3.70 Classify each of the following as an element, a compound, or a mixture: 13.12 a copper 1Cu2 in wiring b chromium oxide in paint c disinfectant in mouthwash 3.71 Classify each of the following mixtures as homogeneous or heterogeneous: 13.12 a powdered iron and powdered sulfur b vinegar c toothpaste 3.72 Classify each of the following mixtures as homogeneous or heterogeneous: 13.12 a dishwashing detergent b ice in soda c vinegar and oil mixture 3.73 Identify each of the following as solid, liquid, or gas: 13.22 a calcium tablets in a bottle b alcohol in water c compressed air in a spray bottle d dust in the air e apple juice in a bottle 3.74 Identify each of the following as solid, liquid, or gas: 13.22 a pencil in a box b oil paint in a container c ice cubes in a bowl d salad dressing in a bowl e air filled in a balloon 3.75 Identify each of the following as a physical or chemical property: 13.22 a Gold is shiny b Gold melts at 1064 °C c Gold is a good conductor of electricity d When gold reacts with yellow sulfur, a black sulfide compound forms 3.76 Identify each of the following as a physical or chemical property: 13.22 a burning of gasoline to give CO2 and water vapor b souring of milk c magnetizing a compass needle d dicing potatoes into small pieces 3.77 Identify each of the following as a physical or chemical change: 13.22 a A plant grows a new leaf b Chocolate is melted for a dessert c Wood is chopped for the fireplace d Wood burns in a woodstove 3.78 Identify each of the following as a physical or chemical change: 13.22 a Aspirin tablets are broken in half b Carrots are grated for use in a salad c Malt undergoes fermentation to make beer d A copper pipe reacts with air and turns green 128  Chapter 3  Matter and Energy 3.79 Calculate each of the following temperatures in degrees Celsius and kelvins: 13.32 a The highest recorded temperature in the continental United States was 134 °F in Death Valley, California, on July 10, 1913 b The lowest recorded temperature in the continental United States was - 69.7 °F in Rodgers Pass, Montana, on January 20, 1954 3.80 Calculate each of the following temperatures in kelvins and degrees Fahrenheit: 13.32 a The highest recorded temperature in the world was 58.0 °C in El Azizia, Libya, on September 13, 1922 b The lowest recorded temperature in the world was -89.2 °C in Vostok, Antarctica, on July 21, 1983 3.81 What is - 20 °F in degrees Celsius and in kelvins? 13.32 3.82 On a hot sunny day, you get out of the swimming pool and sit in a metal chair, which is very hot Would you predict that the specific heat of the metal is higher or lower than that of water? ­Explain 13.62 3.83 On a hot day, the beach sand gets hot but the water stays cool Would you predict that the specific heat of sand is higher or lower than that of water? Explain 13.62 On a sunny day, the sand gets hot but the water stays cool c On the heating curve, identify the segments A, B, C, D, and E as solid, liquid, gas, melting, or boiling d At the following temperatures, is chloroform a solid, liquid, or gas? -80 °C; -40 °C; 25 °C; 80 °C 3.88 Associate the contents of the beakers 11 to 52 with segments 1A to E2 on the following heating curve for water: 13.72 120 D 100 80 60 T °C C 40 20 B A -20 Heat Added 3.84 A large bottle containing 883 g of water at °C is removed from the refrigerator How many kilojoules are absorbed to warm the water to room temperature of 22 °C? 13.62 3.85 A 0.50-g sample of vegetable oil is placed in a calorimeter When the sample is burned, 18.9 kJ is given off What is the energy value 1kcal>g2 for the oil? 13.52 3.86 A 1.3-g sample of rice is placed in a calorimeter When the sample is burned, 22 kJ is given off What is the energy value 1kcal>g2 for the rice? 13.52 3.87 The following graph is a heating curve for chloroform, a solvent for fats, oils, and waxes: 13.72 100 D 60 E 20 C T °C -20 -60 B A E 3.89 The melting point of dibromomethane is - 53 °C and its boiling point is 97 °C Sketch a heating curve for dibromomethane from -100 °C to 120 °C 13.72 a What is the state of dibromomethane at - 75 °C? b What happens on the curve at -53 °C? c What is the state of dibromomethane at - 18 °C? d What is the state of dibromomethane at 110 °C? e At what temperature will both solid and liquid be present? 3.90 The melting point of benzene is 5.5 °C and its boiling point is 80.1 °C Sketch a heating curve for benzene from °C to 100 °C 13.72 a What is the state of benzene at 15 °C? b What happens on the curve at 5.5 °C? c What is the state of benzene at 63 °C? d What is the state of benzene at 98 °C? e At what temperature will both liquid and gas be present? Px Clinical Applications -100 Heat Added a What is the approximate melting point of chloroform? b What is the approximate boiling point of chloroform? 3.91 If you want to lose lb of “body fat,” which is 15% water, how many kilocalories you need to expend? 13.52 3.92 The highest recorded body temperature that a person has survived is 46.5 °C Calculate that temperature in degrees Fahrenheit and in kelvins 13.32 Answers  3.93 A hot-water bottle for a patient contains 725 g of water at 65 °C If the water cools to body temperature 137 °C2, how many kilojoules of heat could be transferred to sore muscles? 13.62 129 3.94 A young patient drinks whole milk as part of her diet Calculate the total kilocalories if the glass of milk contains 12 g of carbohydrate, g of fat, and g of protein 1Round off answers for each food type to the tens place.2 13.52 Challenge Questions The following groups of questions are related to the topics in this chapter However, they not all follow the chapter order, and they require you to combine concepts and skills from several sections These questions will help you increase your critical thinking skills and prepare for your next exam 3.95 When a 0.66-g sample of olive oil is burned in a calorimeter, the heat released increases the temperature of 370 g of water from 22.7 °C to 38.8 °C What is the energy value for the olive oil in kcal>g? 13.5, 3.62 3.96 A 45-g piece of ice at 0.0 °C is added to a sample of water at 8.0 °C All of the ice melts and the temperature of the water decreases to 0.0 °C How many grams of water were in the sample? 13.6, 3.72 3.97 In a large building, oil is used in a steam boiler heating system The combustion of 1.0 lb of oil provides 2.4 * 107 J 13.4, 3.62 a How many kilograms of oil are needed to heat 150 kg of water from 22 °C to 100 °C? b How many kilograms of oil are needed to change 150 kg of water to steam at 100 °C? 3.98 When 1.0 g of gasoline burns, it releases 11 kcal of heat The density of gasoline is 0.74 g>mL 13.4, 3.62 a How many megajoules are released when 1.0 gal of gasoline burns? b If a television requires 150 kJ>h to run, how many hours can the television run on the energy provided by 1.0 gal of gasoline? 3.99 An ice bag containing 225 g of ice at °C was used to treat sore muscles When the bag was removed, the ice had melted and the liquid water had a temperature of 32.0 °C How many kilojoules of heat were absorbed? 13.6, 3.72 3.100 A 115-g sample of steam at 100 °C is emitted from a volcano It condenses, cools, and falls as snow at °C How many kilojoules of heat were released? 13.6, 3.72 3.101 A 70.0-g piece of copper metal at 54.0 °C is placed in 50.0 g of water at 26.0 °C If the final temperature of the water and metal is 29.2 °C, what is the specific heat 1J>g °C2 of copper? 13.62 3.102 A 125-g piece of metal is heated to 288 °C and dropped into 85.0 g of water at 12.0 °C The metal and water come to the same temperature of 24.0 °C What is the specific heat, in J>g °C, of the metal? 13.62 3.103 A metal is thought to be silver or iron When 8.0 g of the metal absorbs 23.50 J, its temperature rises by 6.5 °C 13.62 a What is the specific heat 1J>g °C2 of the metal? b Would you identify the metal as silver or iron 1see Table 3.112? 3.104 A metal is thought to gold or titanium When 20 g of the metal absorbs 30.8 cal, its temperature rises by 50 °C 13.62 a What is the specific heat, in cal>g °C, of the metal? b Would you identify the metal as gold or titanium 1see Table 3.112? Answers Answers to Selected Questions and Problems 3.1 a pure substance c pure substance e mixture b mixture d pure substance 3.3 a element c element e compound b compound d compound 3.5 a heterogeneous c homogeneous e heterogeneous b homogeneous d heterogeneous 3.7 a gas c solid b gas 3.9 a physical c physical e chemical b chemical d chemical 3.11 a physical c physical e physical b chemical d physical 3.13 a chemical c physical e physical b physical d chemical 3.15 In the United States, we still use the Fahrenheit temperature scale In °F, normal body temperature is 98.6 On the Celsius scale, her temperature would be 37.7 °C, a mild fever 3.17 a 98.6 °F c 246 K e 46 °C b 18.5 °C d 335 K 3.19 a 41 °C b No The temperature is equivalent to 39 °C 3.21 When the roller-coaster car is at the top of the ramp, it has its maximum potential energy As it descends, potential energy changes to kinetic energy At the bottom, all the energy is kinetic 3.23 a potential c potential b kinetic d potential 3.25 a 8.1 * 105 J b 190 kcal 130  Chapter 3  Matter and Energy 3.27 a 29.9 kcal b 208 kcal 3.29 a 470 kJ c 130 kcal b 18 g d 37 g 3.31 210 kcal, 880 kJ 3.33 640 kcal 3.35 Copper has the lowest specific heat of the samples and will reach the highest temperature 3.71 a heterogeneous c homogeneous b homogeneous 3.73 a solid c gas e liquid b liquid d solid 3.75 a physical c physical b physical d chemical 3.77 a chemical c physical b physical d chemical 3.79 a 56.7 °C, 330 K b - 56.5 °C, 217 K 3.37 a 180 cal c 2600 J b 14 000 J d 10.8 kJ 3.39 a 1380 J, 330 cal c 3780 J, 904 cal b 1810 J, 434 cal d 3600 J, 850 cal 3.81 -29 °C, 244 K 3.41 a melting c freezing b sublimation d deposition 3.43 a 5200 cal absorbed c 18 kcal released b 5680 J absorbed d 16.7 kJ released 3.83 The same amount of heat causes a greater temperature change in the sand than in the water; thus the sand must have a lower specific heat than that of water 3.45 a condensation c boiling b evaporation d condensation 3.47 a 5400 cal absorbed c 4300 kcal released b 11 300 J absorbed d 396 kJ released 3.49 150 Gas 1e2 100 T °C 50 -20 Liquid 1c2 Boiling 1d2 3.85 9.0 kcal>g 3.87 a about -60 °C b about 60 °C c The diagonal line A represents the solid state as temperature increases The horizontal line B represents the change from solid to liquid or melting of the substance The diagonal line C represents the liquid state as temperature increases The horizontal line D represents the change from liquid to gas or boiling of the liquid The diagonal line E represents the gas state as temperature increases d At -80 °C, solid; at -40 °C, liquid; at 25 °C, liquid; at 80 °C, gas 3.89 140 Melting 1b2 Solid 1a2 100 Heat Added 3.51 a 30 300 J c 72.2 kJ b 9.6 kcal 60 T °C 20 3.53 11 kcal -20 3.55 a Breakfast 270 kcal; Lunch 420 kcal; Dinner 440 kcal b 1130 kcal total c Yes Charles should be losing weight d 26 days 3.57 a compound, the molecules have a definite 2:1 ratio of atoms b mixture, has two different kinds of atoms and molecules c element, has a single kind of atom 3.59 a heterogeneous c homogeneous b heterogeneous -60 -100 Heat Added a solid c liquid e -53 °C 3.61 61.4 °C, 143 °F 3.63 68.3 °C, 341 K 3.91 3500 kcal 3.65 Gold, 497.94 J or 118.88 cal; aluminum, 484.38 J or 115.56 cal 3.93 85 kJ 3.67 a carbohydrate, 680 kcal; fat, 590 kcal; protein, 240 kcal b 1510 kcal c 25 h d 2.0 h 3.95 9.0 kcal>g 3.69 a element c mixture b compound 3.97 a 0.93 kg b solid dibromomethane melts d gas b 6.4 kg 3.99 105.3 kJ 3.101 Specific heat = 0.385 J>g °C 3.103 a 0.452 J>g °C b iron Combining Ideas from   Chapters to CI.1 Gold, one of the most sought-after metals in the world, has a density of 19.3 g>cm3, a melting point of 1064 °C, a specific heat of 0.129 J>g °C, and a heat of fusion of 63.6 J>g A gold nugget found in Alaska in 1998 weighs 20.17 lb 12.4, 2.6, 2.7, 3.3, 3.6, 3.72 a In which sample 1A or B2 does the water have its own shape? b Which diagram 11 or or 32 represents the arrangement of particles in water sample A? c Which diagram 11 or or 32 represents the arrangement of particles in water sample B? Gold nuggets, also called native gold, can be found in streams and mines a How many significant figures are in the measurement of the weight of the nugget? b Which is the mass of the nugget in kilograms? c If the nugget were pure gold, what would its volume be in cm3? d What is the melting point of gold in degrees Fahrenheit and kelvins? e How many kilocalories are required to raise the temperature of the nugget from 500 °C to 1064 °C and melt all the gold to liquid at 1064 °C? f If the price of gold is $45.98 per gram, what is the nugget worth, in dollars? CI.2 The mileage for a motorcycle with a fuel-tank capacity of 22 L is 35 mi>gal 12.5, 2.6, 2.7, 3.42 a How long a trip, in kilometers, can be made on one full tank of gasoline? b If the price of gasoline is $3.82 per gallon, what would be the cost of fuel for the trip? c If the average speed dur- When 1.00 g of gasoline ing the trip is 44 mi > h, burns, 47 kJ of energy are how many hours will it released take to reach the destination? d If the density of gasoline is 0.74 g>mL, what is the mass, in grams, of the fuel in the tank? e When 1.00 g of gasoline burns, 47 kJ of energy is released How many kilojoules are produced when the fuel in one full tank is burned? CI.3 Answer the following questions for the water samples A and B shown in the diagrams: 13.1, 3.2, 3.62 A B Answer the following for diagrams 1, 2, and 3: 13.2, 3.32 d The state of matter indicated in diagram is a ; in diagram 2, it is a ; and in diagram 3, it is a e The motion of the particles is slowest in diagram f The arrangement of particles is farthest apart in diagram g The particles fill the volume of the container in diagram h If the water in diagram has a mass of 19 g and a temperature of 45 °C, how much heat, in kilojoules, is removed to cool the liquid to °C? CI.4 The label of a black cherry almond energy bar with a mass of 68 g lists the nutrition facts as 39 g of carbohydrate, g of fat, and 10 g of protein 12.5, 2.6, 3.4, 3.52 a Using the energy values for carbohydrates, fats, and proteins 1see Table 3.72, what are the total kilocalories 1Calories2 listed for a black cherry almond bar? 1Round off answers for each food type to the tens place.2 b What are the kilojoules for the An energy bar conblack cherry almond bar? tains carbohydrate, 1Round off answers for each fat, and protein food type to the tens place.2 c If you obtain 160 kJ, how many grams of the black cherry almond bar did you eat? d If you are walking and using energy at a rate of 840 kJ >h, how many minutes will you need to walk to expend the energy from two black cherry almond bars? 131 132  Chapter 3  Matter and Energy CI.5 In one box of nails, there are 75 iron nails weighing 0.250 lb The density of iron is 7.86 g>cm3 The specific heat of iron is 0.452 J>g °C The melting point of iron is 1535 °C The heat of fusion for iron is 272 J>g.12.5, 2.6, 2.7, 3.4, 3.6, 3.72 Nails made of iron have a density of 7.86 g> cm3 a What is the volume, in cm3, of the iron nails in the box? b If 30 nails are added to a graduated cylinder containing 17.6 mL of water, what is the new level of water, in ­milliliters, in the cylinder? c How much heat, in joules, must be added to the nails in the box to raise their temperature from 16 °C to 125 °C? d How much heat, in joules, is required to heat one nail from 25 °C to its melting point and change it to liquid iron? CI.6 A hot tub is filled with 450 gal of water 12.5, 2.6, 2.7, 3.3, 3.4, 3.62 A hot tub filled with water is heated to 105 °F a What is the volume of water, in liters, in the tub? b What is the mass, in kilograms, of water in the tub? c How many kilocalories are needed to heat the water from 62 °F to 105 °F? d If the hot-tub heater provides 5900 kJ > min, how long, in minutes, will it take to heat the water in the hot tub from 62 °F to 105 °F? Answers CI.1 a significant figures b 9.17 kg c 475 cm3 d 1947 °F; 1337 K e 298 kcal f $422 000 CI.3 a B b A is represented by diagram c B is represented by diagram d solid; liquid; gas e diagram f diagram g diagram h 3.6 kJ CI.5 a 14.4 cm3 b 23.4 mL c 5590 J d 1440 J ... to General, Organic, and Biological Chemistry: Structures of Life, fifth edition, she is also the author of Chemistry: An Introduction to General, Organic, and Biological Chemistry, twelfth edition, ... General, Organic, and Biological Chemistry: Structures of Life, fifth edition, provides an integrated teaching and learning package of support material for both students and professors Name of. .. the fifth edition of General, Organic, and Biological Chemistry: Structures of Life This chemistry text was written and designed to help you prepare for a career in a health-related profession,