Preview ISE General, Organic, Biological Chemistry (ISE HED WCB CHEMISTRY) by Janice Gorzynski Smith Dr. (2021)

Preview ISE General, Organic, Biological Chemistry (ISE HED WCB CHEMISTRY) by Janice Gorzynski Smith Dr. (2021) Preview ISE General, Organic, Biological Chemistry (ISE HED WCB CHEMISTRY) by Janice Gorzynski Smith Dr. (2021) Preview ISE General, Organic, Biological Chemistry (ISE HED WCB CHEMISTRY) by Janice Gorzynski Smith Dr. (2021) Preview ISE General, Organic, Biological Chemistry (ISE HED WCB CHEMISTRY) by Janice Gorzynski Smith Dr. (2021)

page i General, Organic, & Biological CHEMISTRY Fifth Edition Janice Gorzynski Smith University of Hawai‘i at Ma-noa GENERAL, ORGANIC, & BIOLOGICAL CHEMISTRY Published by McGraw Hill LLC, 1325 Avenue of the Americas, New York, NY 10121 Copyright ©2022 by McGraw Hill LLC All rights reserved Printed in the United States of America Previous editions ©2019, 2016, and 2013 No part of this publication may be reproduced or distributed in any form or by any means, or stored in a database or retrieval system, without the prior written consent of McGraw Hill LLC, including, but not limited to, in any network or other electronic storage or transmission, or broadcast for distance learning Some ancillaries, including electronic and print components, may not be available to customers outside the United States This book is printed on acid-free paper LWI 24 23 22 21 ISBN 978-1-264-64741-5 MHID 1-264-64741-7 Cover Image: Douglas Klug/Getty Images All credits appearing on page or at the end of the book are considered to be an extension of the copyright page The Internet addresses listed in the text were accurate at the time of publication The inclusion of a website does not indicate an endorsement by the authors or McGraw Hill LLC, and McGraw Hill LLC does not guarantee the accuracy of the information presented at these sites mheducation.com/highered About the Author page iii Daniel C Smith Janice Gorzynski Smith was born in Schenectady, New York She received an A.B degree summa cum laude in chemistry at Cornell University and a Ph.D in Organic Chemistry from Harvard University under the direction of Nobel Laureate E J Corey During her tenure with the Corey group, she completed the total synthesis of the plant growth hormone gibberellic acid Following her postdoctoral work, Jan joined the faculty of Mount Holyoke College where she was employed for 21 years During this time she was active in teaching chemistry lecture and lab courses, conducting a research program in organic synthesis, and serving as department chair Her organic chemistry class was named one of Mount Holyoke’s “Don’t-miss courses” in a survey by Boston magazine After spending two sabbaticals amidst the natural beauty and diversity in Hawai‘i in the 1990s, Jan and her family moved there permanently in 2000 Most recently, she has served as a faculty member at the University of Hawai‘i at Mānoa In 2003, she received the Chancellor’s Citation for Meritorious Teaching Jan resides in Hawai‘i with her husband Dan, an emergency medicine physician, pictured with her hiking in Laos in 2019 She has four children and nine grandchildren When not teaching, writing, or enjoying her family, Jan bikes, hikes, snorkels, and scuba dives in sunny Hawai‘i, and time permitting, enjoys travel and Hawaiian quilting Dedicated to my family, especially Max, Oliver, Alijah, Koa, Logan, Elliott, Penelope, Otis, and Isabelle About the cover Giant kelp, a type of marine algae that grows in dense forests in cold ocean waters, is a source of atmospheric chloromethane (CH3Cl), a simple organic compound that contains the halogen chlorine Chloromethane, a colorless gas with a faint odor, is also formed in forests by wood-rotting fungi and is released during volcanic eruptions Because it is a key compound in the manufacture of polymers and drugs, chloromethane is extensively produced by the chemical industry, but most of the chloromethane in the atmosphere is natural in origin In General, Organic, & Biological Chemistry, we learn about the chemical properties of compounds like chloromethane Brief Contents Matter and Measurement Atoms and the Periodic Table Ionic Compounds Covalent Compounds Chemical Reactions Energy Changes, Reaction Rates, and Equilibrium Gases, Liquids, and Solids Solutions Acids and Bases 10 Nuclear Chemistry 11 Introduction to Organic Molecules and Functional Groups 12 Alkanes 13 Unsaturated Hydrocarbons 14 Organic Compounds That Contain Oxygen, Halogen, or Sulfur 15 The Three-Dimensional Shape of Molecules 16 Aldehydes and Ketones 17 Carboxylic Acids, Esters, and Amides 18 Amines and Neurotransmitters 19 Lipids 20 Carbohydrates 21 Amino Acids, Proteins, and Enzymes 22 Nucleic Acids and Protein Synthesis 23 Metabolism and Energy Production 24 Carbohydrate, Lipid, and Protein Metabolism Available online only in McGraw-Hill Connect® and CreateTM 25 Body Fluids page iv Contents page v Preface xxi Acknowledgments xxviii Daniel C Smith Matter and Measurement 1.1 Chemistry—The Science of Everyday Experience 1.2 States of Matter 1.3 Classification of Matter 1.4 Measurement 1.5 1.6 1.7 1.4A The Metric System 1.4B Measuring Length 10 1.4C Measuring Mass 10 1.4D Measuring Volume 11 Significant Figures 12 1.5A Determining the Number of Significant Figures 12 1.5B Using Significant Figures in Multiplication and Division 13 1.5C Using Significant Figures in Addition and Subtraction 15 Scientific Notation 16 1.6A Writing Numbers in Scientific Notation 16 1.6B Using a Scientific Calculator for Numbers in Scientific Notation 19 Problem Solving Using Conversion Factors 19 1.7A Conversion Factors 19 1.7B Solving a Problem Using One Conversion Factor 20 1.7C Solving a Problem Using Two or More Conversion Factors 22 1.8 FOCUS ON HEALTH & MEDICINE: Problem Solving Using Clinical Conversion Factors 23 1.9 Temperature 25 1.10 Density and Specific Gravity 26 1.10A Density 26 1.10B Specific Gravity 29 Chapter Review 29 Key Terms 29 Key Concepts 30 Key Equations 30 Key Skills 31 Problems 32 Challenge Problems 35 Answers to Problems 36 Daniel C Smith Atoms and the Periodic Table 38 2.1 Elements 39 2.1A Elements and the Periodic Table 40 2.1B FOCUS ON THE HUMAN BODY: The Elements of Life 41 2.1C Compounds 42 2.2 Structure of the Atom 44 2.3 Isotopes 48 2.4 2.3A Isotopes, Atomic Number, and Mass Number 48 2.3B Atomic Weight 51 2.3C FOCUS ON HEALTH & MEDICINE: Isotopes in Medicine 52 The Periodic Table 52 2.4A Basic Features of the Periodic Table 52 2.4B Characteristics of Groups 1A, 2A, 7A, and 8A 54 2.5 Electronic Structure 56 2.6 Electronic Configurations 59 2.6A First-Row Elements (Period 1) 60 2.6B Second-Row Elements (Period 2) 61 page vi 2.6C 2.7 2.8 Electronic Configurations of Other Elements Using the Periodic Table 62 Valence Electrons 64 2.7A Relating Valence Electrons to Group Number 65 2.7B Electron-Dot Symbols 67 Periodic Trends 67 2.8A Atomic Size 67 2.8B Ionization Energy 68 Chapter Review 70 Key Terms 70 Key Concepts 71 Key Skills 72 Problems 73 Challenge Problems 77 Answers to Problems 77 Mark Dierker/McGraw-Hill Ionic Compounds 79 3.1 Introduction to Bonding 80 3.2 Ions 82 3.3 3.4 3.2A Cations and Anions 82 3.2B Relating Group Number to Ionic Charge for Main Group Elements 85 3.2C Metals with Variable Charge 87 3.2D FOCUS ON THE HUMAN BODY: Important Ions in the Body 88 Ionic Compounds 90 3.3A Formulas for Ionic Compounds 91 3.3B FOCUS ON HEALTH & MEDICINE: Ionic Compounds in Consumer Products 93 Naming Ionic Compounds 93 3.4A Naming Cations 93 3.4B Naming Anions 94 3.4C Naming Ionic Compounds with Cations from Main Group Metals 95 b Al2(SO4)3 (aluminum sulfate), once used as a common antiperspirant c C6H8O6 (vitamin C) 5.52 Calculate the formula weight and molar mass of each compound a MgSO4 (magnesium sulfate), a laxative b Ca3(PO4)2 (calcium phosphate), a calcium supplement c C16H16ClNO2S (Plavix), a drug used to treat coronary artery disease 5.53 l-Dopa is a drug used to treat Parkinson’s disease 5.54 Niacin, vitamin B3, is found in soybeans, which contain it naturally, and cereals, which are fortified with it Moles, Mass, and Avogadro's Number 5.55 Which quantity has the greater mass? a mol of Fe atoms or mol of Sn atoms b mol of C atoms or 6.02 × 1023 N atoms c mol of N atoms or mol of N2 molecules d mol of CO2 molecules or 3.01 × 1023 N2O molecules 5.56 Which quantity has the greater mass? a mol of Si atoms or mol of Ar atoms b mol of He atoms or 6.02 × 1023 H atoms c mol of Cl atoms or mol of Cl2 molecules d mol of C2H4 molecules or 3.01 × 1023 C2H4 molecules 5.57 Mescaline is a hallucinogen in peyote, a cactus native to the southwestern United States and Mexico (a) What is the chemical formula of mescaline? (b) Calculate its molar mass (c) How many moles are contained in 7.50 g of mescaline? page 191 5.58 (a) What is the chemical formula of eugenol, the main contributor to the aroma of cloves? (b) Calculate its molar mass (c) How many moles are contained in 10.50 g of eugenol? 5.59 How many grams are contained in 5.00 mol of each compound? a HCl b Na2SO4 c C2H2 d Al(OH)3 5.60 How many grams are contained in 0.50 mol of each compound? a NaOH b CaSO4 c C3H6 d Mg(OH)2 5.61 A bottle of the pain reliever ibuprofen (C13H18O2, molar mass 206.3 g/mol) contains 500 200.-mg tablets (a) How many moles of ibuprofen does the bottle contain? (b) How many molecules of ibuprofen does the bottle contain? Jill Braaten 5.62 One dose of Maalox contains 500 mg each of Mg(OH)2 and Al(OH)3 How many moles of each compound are contained in a single dose? Jill Braaten/McGraw-Hill 5.63 How many moles are contained in each number of grams of table sugar (C12H22O11, molar mass 342.3 g/mol)? a 0.500 g b 5.00 g c 25.0 g d 0.0250 g 5.64 How many moles are contained in each number of grams of fructose (C6H12O6, molar mass 180.2 g/mol), a carbohydrate that is about twice as sweet as table sugar? “Lite” food products use half as much fructose as table sugar to achieve the same sweet taste but with fewer calories a 0.500 g b 5.00 g c 25.0 g d 0.0250 g 5.65 How many molecules of the cholesterol-lowering drug atorvastatin (C33H35FN2O5, trade name Lipitor) are contained in the following number of moles: (a) 2.00 mol; (b) 0.250 mol; (c) 26.5 mol; (d) 222 mol; (e) 5.00 × 105 mol? 5.66 How many moles of the antidepressant fluoxetine (C17H18F3NO, trade name Prozac) are contained in the following number of molecules? a 5.00 × 1019 molecules b 6.51 × 1028 molecules d 3.10 × 1020 molecules c 8.32 × 1021 molecules 5.67 The average nicotine (C10H14N2, molar mass 162.3 g/mol) content of a Camel cigarette is 1.93 mg Suppose an individual smokes one pack of 20 cigarettes a day a How many moles of nicotine are smoked in a day? b How many molecules of nicotine are smoked in a day? Jetsadaphoto/Shutterstock 5.68 How many moles of sucrose (table sugar, C12H22O11, molar mass 342.3 g/mol) are contained in a 5.0lb bag of sugar? 5.69 What is the mass in grams of each quantity of lactic acid (C3H6O3, molar mass 90.08 g/mol), the compound responsible for the aching feeling of tired muscles during vigorous exercise? page 192 a 3.60 mol b 0.580 mol c 7.3 × 1024 molecules d 6.56 × 1022 molecules 5.70 What is the mass in grams of each quantity of vitamin D (molar mass 384.7 g/mol), which is needed for forming and maintaining healthy bones? a 3.6 mol b 0.58 mol c 7.3 × 1024 molecules d 6.56 × 1022 molecules Mass and Mole Calculations in Chemical Equations 5.71 Using the balanced equation for the combustion of acetylene, answer the following questions a How many moles of O2 are needed to react completely with 5.00 mol of C2H2? b How many moles of CO2 are formed from 6.0 mol of C2H2? c How many moles of H2O are formed from 0.50 mol of C2H2? d How many moles of C2H2 are needed to form 0.80 mol of CO2? 5.72 Sodium metal (Na) reacts violently when added to water according to the following balanced equation Na(s) + H2O(l) NaOH(aq) + H2(g) a How many moles of H2O are needed to react completely with 3.0 mol of Na? b How many moles of H2 are formed from 0.38 mol of Na? c How many moles of H2 are formed from 3.64 mol of H2O? 5.73 Using the balanced equation for the combustion of acetylene in Problem 5.71, answer the following questions a How many grams of CO2 are formed from 2.5 mol of C2H2? b How many grams of CO2 are formed from 0.50 mol of C2H2? c How many grams of H2O are formed from 0.25 mol of C2H2? d How many grams of O2 are needed to react with 3.0 mol of C2H2? 5.74 Using the balanced equation for the reaction of Na with H2O in Problem 5.72, answer the following questions a How many grams of NaOH are formed from 3.0 mol of Na? b How many grams of H2 are formed from 0.30 mol of Na? c How many grams of H2O are needed to react completely with 0.20 mol of Na? Theoretical Yield and Percent Yield 5.75 What is the percent yield of B in a reaction that uses 10.0 g of starting material A, has a theoretical yield of 12.0 g of B, and an actual yield of 9.0 g of B? 5.76 What is the percent yield of B in a reaction that uses 25.0 g of starting material A, has a theoretical yield of 20.0 g of B, and an actual yield of 17.0 g of B? 5.77 The reaction of methane (CH4) with Cl2 forms chloroform (CHCl3) and HCl Although CHCl3 is a general anesthetic, it is no longer used for this purpose because it is also carcinogenic The molar masses for all substances are given under the balanced equation a What is the theoretical yield of CHCl3 in grams from 3.20 g of CH4? b What is the percent yield if 15.0 g of CHCl3 are actually formed in this reaction? 5.78 Methanol (CH4O), which is used as a fuel in high-performance racing cars, burns in the presence of O2 to form CO2 and H2O The molar masses for all substances are given under the balanced equation a What is the theoretical yield of CO2 from 48.0 g of methanol? b What is the percent yield of CO2 if 48.0 g of CO2 are formed? Limiting Reactants 5.79 Consider the given reaction mixture that contains A and B molecules, represented by red and blue spheres, respectively Given each of the following chemical equations, which reactant, A or B, is present in excess? Which reactant is the limiting reactant? 5.80 Consider the reaction of A2 and B2 to form A2B, according to the balanced equation: A2 + B2 A2B Identify the limiting reactant in the molecular art, and draw a representation showing how much product is formed and what reactant molecules are left over 5.81 Consider the reaction with the balanced equation, N2 + O2 NO2 (a) Identify the limiting page 193 reactant under the reaction conditions shown in the molecular art (b) What reactant molecules are left over? (c) Draw a representation showing what the product mixture looks like when the reaction is complete 5.82 Consider the reaction with the balanced equation, N2 + H2 NH3 (a) Identify the limiting reactant under the reaction conditions shown in the molecular art (b) What reactant molecules are left over in this reaction? (c) Draw a representation showing what the product mixture looks like when the reaction is complete 5.83 Using the balanced equation, NO + O2 following conditions a 1.0 mol NO and 1.0 mol O2 b 2.0 mol NO and 0.50 mol O2 NO2, determine the limiting reactant under each of the c 10.0 g NO and 10.0 g O2 d 28.0 g NO and 16.0 g O2 5.84 For each set of reaction conditions in Problem 5.83, calculate how many moles of the product NO2 form Then, calculate the number of grams of product that forms 5.85 Complete the following table using the given balanced equation and the initial quantities of reactants Label the limiting reactant and the reactant used in excess 5.86 Complete the following table using the given balanced equation and the initial quantities of reactants Label the limiting reactant and the reactant used in excess 5.87 The local anesthetic ethyl chloride (C2H5Cl, molar mass 64.51 g/mol) can be prepared by reaction of ethylene (C2H4, molar mass 28.05 g/mol) with HCl (molar mass 36.46 g/mol), according to the balanced equation, C2H4 + HCl C2H5Cl a If 8.00 g of ethylene and 12.0 g of HCl are used, how many moles of each reactant are used? b What is the limiting reactant? c How many moles of product are formed? d How many grams of product are formed? e If 10.6 g of product are formed, what is the percent yield of the reaction? 5.88 The solvent dichloromethane (CH2Cl2, molar mass 84.93 g/mol) can be prepared by reaction of methane (CH4, molar mass 16.04 g/mol) with Cl2 (molar mass 70.90 g/mol), according to the balanced equation, CH4 + Cl2 CH2Cl2 + HCl a If 5.00 g of methane and 15.0 g of Cl2 are used, how many moles of each reactant are used? b What is the limiting reactant? c How many moles of product are formed? d How many grams of product are formed? e If 5.6 g of product are formed, what is the percent yield of the reaction? General Questions and Applications 5.89 Answer the following questions about the conversion of the sucrose (C12H22O11) in sugarcane to ethanol (C2H6O) and CO2 according to the following unbalanced equation In this way sugarcane is a renewable source of ethanol, which is used as a fuel additive in gasoline a What is the molar mass of sucrose? b Balance the given equation c How many moles of ethanol are formed from mol of sucrose? d How many moles of water are needed to react with 10 mol of sucrose? e How many grams of ethanol are formed from 0.550 mol of sucrose? f How many grams of ethanol are formed from 34.2 g of sucrose? g What is the theoretical yield of ethanol in grams from 17.1 g of sucrose? h If 1.25 g of ethanol are formed in the reaction in part (g), what is the percent yield of ethanol? 5.90 Answer the following questions about diethyl ether (C4H10O), the first widely used general anesthetic Diethyl ether can be prepared from ethanol according to the following unbalanced equation page 194 a What is the molar mass of diethyl ether? b Balance the given equation c How many moles of diethyl ether are formed from mol of ethanol? d How many moles of water are formed from 10 mol of ethanol? e How many grams of diethyl ether are formed from 0.55 mol of ethanol? f How many grams of diethyl ether are formed from 4.60 g of ethanol? g What is the theoretical yield of diethyl ether in grams from 2.30 g of ethanol? h If 1.80 g of diethyl ether are formed in the reaction in part (g), what is the percent yield of diethyl ether? 5.91 DDT, a pesticide that kills disease-carrying mosquitoes, is synthesized by the given equation DDT is now banned in the United States because it is a persistent environmental pollutant that only slowly degrades a What is the molar mass of DDT? b How many grams of DDT would be formed from 0.10 mol of chlorobenzene? c What is the theoretical yield of DDT in grams from 11.3 g of chlorobenzene? d If 15.0 g of DDT are formed in the reaction in part (c), what is the percent yield of DDT? 5.92 Fats, such as butter, and oils, such as corn oil, are formed from compounds called fatty acids, one of which is linolenic acid (C18H30O2) Linolenic acid undergoes reactions with hydrogen and oxygen to form the products shown in each equation a Calculate the molar mass of linolenic acid b Balance Equation [1], which shows the reaction with hydrogen c Balance Equation [2], which shows the reaction with oxygen d How many grams of product are formed from 10.0 g of linolenic acid in Equation [1]? CHALLENGE PROBLEMS 5.93 TCDD, also called dioxin (C12H4Cl4O2, molar mass 322.0 g/mol), is a potent poison The average lethal dose in humans is estimated to be 3.0 × 10−2 mg per kg of body weight (a) How many grams constitute a lethal dose for a 70.-kg individual? (b) How many molecules of TCDD does this correspond to? 5.94 A 12-oz can of diet soda contains 180 mg of the artificial sweetener aspartame (trade names NutraSweet and Equal) When aspartame is ingested, it is metabolized to phenylalanine, aspartic acid, and methanol, according to the balanced equation: a Using this equation, determine how much methanol (in mg) is formed on metabolism of the aspartame in each 12-oz can The molar mass of aspartame is 294.2 g/mol, and the molar mass of methanol is 32.04 g/mol b Methanol is a toxic compound, with the average lethal dose in humans estimated at 428 mg/kg of body weight How many cans of soda would a 52-kg individual have to ingest to obtain a lethal dose of methanol? ANSWERS TO PROBLEMS Practice Problems 5.1 5.2 5.3 5.4 5.5 5.6 5.7 The process is a chemical reaction because the reactants contain two gray spheres joined (indicating H2) and two red spheres joined (indicating O2), whereas the product (H2O) contains a red sphere joined to two gray spheres (indicating O—H bonds) 5.8 5.9 a 1.20 × 1024 C atoms b 3.61 × 1024 C atoms c 3.01 × 1023 C atoms d 1.51 × 1025 C atoms 5.10 a 100 mol b 0.0500 mol c 15 mol 5.11 285.33 g/mol 5.12 a 29.2 g b 332 g c 101 g d 26.3 g 5.13 a 1.71 mol b 1.59 mol c 1.39 × 10−3 mol d 1.39 mol 5.14 1.80 × 1021 molecules 5.15 a 6.6 mol b 1.0 mol c 5.16 1.2 mol a 51 g b 22 g c 5.17 90 g a 72.4 g b 24.1 g c 7.24 g 5.18 88.0% 5.19 a 154 g page 195 b 34.7% 5.20 a 111 g b 59.0% 5.21 H2 is the limiting reactant 5.22 a 1.0 mol b 0.67 mol c 1.3 mol d 4.0 mol 5.23 a N2 b O2 5.24 a 26.8 g b 24.4 g Problems 5.1 The process is a physical change (freezing), because the particles in the reactants are the same as the particles in the products 5.3 CO + O2 5.5 a,c: combination b,d: decomposition 5.7 a The reactant is C2H6O and the products are H2CCH2 and H2O CO2 b c decomposition 5.9 a 1.20 x 1024 C atoms b 3.61 x 1024 C atoms c 3.01 x 1023 C atoms d 1.51 x 1025 C atoms 5.11 a,b,c,d: 6.02 × 1023 5.13 a 100.09 amu b 166.0 amu 5.15 5.679 × 10−3 mol vitamin C 5.17 a 44 g b 130 g c 5.19 24 g a 323 g b 37.8% 5.21 a,b,d: H2 c: O2 5.23 CO + O3 5.25 a H, Cl, Ca on both sides; therefore balanced CO2 + O2 (not balanced) b Ti, Cl, H, O on left side, and Ti, Cl, H, O on right side; therefore NOT balanced c Al, P, O, H on both sides; therefore balanced 5.27 H2 + Cl2 HCl 5.29 CH4 + Br2 5.31 a Ni(s) + HCl(aq) CHBr3 + HBr NiCl2(aq) + H2(g) b CH4(g) + Cl2(g) c KClO3 CCl4(g) + HCl(g) KCl + O2 d Al2O3 + HCl AlCl3 + H2O e Al(OH)3 + H2SO4 Al2(SO4)3 + H2O 5.33 5.35 a C6H6 + 15 O2 12 CO2 + H2O b 5.37 a The reactants are CO and O2 and the product is CO2 b CO + O2 CO2 c combination 5.39 a The reactants are N2 and O2 and the product is NO2 b N2 + O2 NO2 c combination 5.41 a decomposition b single replacement c combination d double replacement 5.43 a Na + Cl2 b NI3 5.45 NaCl N2 + I2 c Cl2 + KI KCl + I2 d KOH + HI KI + H2O a Fe (oxidized) Cu2+ (reduced)Fe Fe2+ + e−Cu2+ + e− Cu b Cl2 (reduced) I− (oxidized)2 I− c Na (oxidized) Cl2 (reduced)2 Na I2 + e−Cl2 + e− Na+ + e−Cl2 + e− Cl− Cl− 5.47 5.49 Acetylene is reduced because it gains hydrogen atoms 5.51 a 69.00 amu, 69.00 g/mol b 342.2 amu, 342.2 g/mol c 176.12 amu, 176.12 g/mol 5.53 a C9H11NO4 b 197.2 amu c 197.2 g/mol 5.55 a mol Sn c mol N2 molecules b 6.02 × 1023 N atoms d mol CO2 5.57 a C11H17NO3 b molar mass = 211.3 g/mol c 0.0355 mol 5.59 a 182 g b 710 g c 130 g d 390 g 5.61 a 0.485 mol b 2.92 × 1023 5.63 a 1.46 × 10−3 mol b 0.0146 mol c 0.0730 mol d 7.30 × 10−5 mol 5.65 a 1.20 × 1024 b 1.51 × 1023 d 1.34 × 1026 c 1.60 × 1025 e 3.01 × 1029 5.67 a 2.38 × 10−4 mol b 1.43 × 1020 molecules 5.69 a 324 g b 52.2 g page 196 c 1.1 × 103 g d 9.82 g 5.71 a 12.5 mol b 12 mol c 0.50 mol d 0.40 mol 5.73 a 220 g b 44 g c 4.5 g d 240 g 5.75 75% 5.77 a 23.9 g b 62.8% 5.79 a B limiting reactant A in excess b A limiting reactant B in excess c B limiting reactant A in excess 5.81 a O2 is the limiting reactant b N2 molecules are left over c 5.83 a NO b O2 c NO d NO 5.85 5.87 a 0.285 mol ethylene and 0.329 mol HCl b ethylene c 0.285 mol d 18.4 g e 57.6% 5.89 a 342.3 g/mol b C12H22O11(s) + H2O(l) c mol d 10 mol f 18.4 g h 13.6% C2H6O(l) + CO2(g) e 101 g g 9.21 g 5.91 a 354.5 g/mol b 18 g c 17.8 g d 84.3% 5.93 a 2.1 × 10−3 g b 3.9 × 1018 molecules ...page i General, Organic, & Biological CHEMISTRY Fifth Edition Janice Gorzynski Smith University of Hawai‘i at Ma-noa GENERAL, ORGANIC, & BIOLOGICAL CHEMISTRY Published by McGraw Hill... McGraw-Hill SmartBook for General, Organic, & Biological Chemistry I am also extremely grateful to the authors of the other ancillaries to accompany General, Organic, & Biological Chemistry, Fifth Edition:... page iii Daniel C Smith Janice Gorzynski Smith was born in Schenectady, New York She received an A.B degree summa cum laude in chemistry at Cornell University and a Ph.D in Organic Chemistry from