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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.pearsoned.co.uk © Pearson Education Limited 2014 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 licence 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: 1-292-02062-8 ISBN 13: 978-1-292-02062-4 British Library Cataloguing-in-Publication Data A catalogue record for this book is available from the British Library Printed in the United States of America CHEMICAL REACTIONS AND QUANTITIES 111 112 113 Gasohol is a fuel that contains ethanol 1C2H6O2, which burns in oxygen 1O22 to give carbon dioxide and water. (6, 7) a. Write the balanced equation for the combustion of ethanol. b. How many moles of O2 are needed to completely react with 4.0 moles of C2H6O? c. If a car produces 88 g of CO2, how many grams of O2 are used up in the reaction? d. If you add 125 g of C2H6O to your fuel, how many grams of CO2 and H2O can be produced from the ethanol? 114 When ammonia 1NH32 reacts with fluorine, the products are dinitrogen tetrafluoride and hydrogen fluoride. (1, 6, 7) a. Write the balanced equation for the reaction. b. How many moles of each reactant are needed to produce 4.00 moles of HF? c. How many grams of F2 are required to react with 25.5 g of NH3? d. How many grams of N2F4 can be produced when 3.40 g of NH3 reacts? When peroxide 1H2O22 is used in rocket fuels, it produces water and oxygen 1O22. (1, 6, 7) a. Write the balanced equation for the reaction. b. How many moles of peroxide are needed to produce 3.00 moles of water? c. How many grams of peroxide are required to produce 36.5 g of O2? d. How many grams of water can be produced when 12.2 g of peroxide reacts? Ethane gas, C2H6, reacts with chlorine gas, Cl2, to form hexachloroethane gas, C2Cl6, and hydrogen chloride gas. (1, 6, 7) a. Write the balanced equation for the reaction. b. How many moles of chlorine gas must react to produce 1.60 moles of hexachloroethane? c. How many grams of hydrogen chloride are produced when 50.0 g of ethane reacts? d. How many grams of hexachloroethane are produced when 50.0 g of ethane reacts? Propane gas, C3H8, a fuel for many barbecues, reacts with oxygen to produce water and carbon dioxide. Propane has a density of 2.02 g/L at room temperature. (1, 4, 6, 7) Pearson Education 110 Propane is converted to carbon dioxide and water when used as a fuel in a barbecue. 115 116 a. Write the balanced equation for the reaction. b. How many grams of water form when 5.00 L of propane gas completely react? c. How many grams of CO2 are produced from 18.5 g of oxygen gas and excess propane? d. How many grams of H2O can be produced from the reaction of 8.50 * 1022 molecules of propane gas? Acetylene gas, C2H2, burns in oxygen to produce carbon dioxide and water. If 62.0 g of CO2 is produced when 22.5 g of C2H2 reacts with sufficient oxygen, what is the percent yield of CO2 for the reaction? (1, 6, 7, 8) When 50.0 g of iron(III) oxide reacts with carbon monoxide, 32.8 g of iron is produced. What is the percent yield of Fe for the reaction? (6, 7, 8) Fe 2O31s2 + 3CO1g2 h 2Fe1s2 + 3CO21g2 C HA LLE NG E Q UES TIO NS 117 Pentane gas, C5H12, reacts with oxygen to produce carbon dioxide and water. (6, 7, 8) 119 C5H121g2 + 8O21g2 h 5CO21g2 + 6H2O1g2 Pentane 118 a. How many grams of pentane must react to produce 4.0 moles of water? b. How many grams of CO2 are produced from 32.0 g of oxygen and excess pentane? c. How many grams of CO2 are formed if 44.5 g of C5H12 is reacted with 108 g of O2? 120 121 3NO21g2 + H2O1l2 h 2HNO31aq2 + NO1g2 256 2Na1s2 + Cl21g2 h 2NaCl1s2 If a mixture of 35.8 g of CH4 and 75.5 g of S reacts, how many grams of H2S are produced? (6, 7, 8) CH41g2 + 4S1g2 h CS21g2 + 2H2S1g2 The formation of nitrogen oxide, NO, from N21g2 and O21g2, requires 21.6 kcal of heat. (9) N21g2 + O21g2 h 2NO1g2 When nitrogen dioxide 1NO22 from car exhaust combines with water in the air, it forms nitric acid 1HNO32, which causes acid rain, and nitrogen oxide. (6, 7, 8) a. How many molecules of NO2 are needed to react with 0.250 mole of H2O? b. How many grams of HNO3 are produced when 60.0 g of NO2 completely reacts? c. How many grams of HNO3 can be produced if 225 g of NO2 is reacted with 55.2 g of H2O? When a mixture of 12.8 g of Na and 10.2 g of Cl2 reacts, what is the mass of NaCl that is produced? (6, 7, 8) 122 H = +21.6 kcal a. How many kilocalories are required to form 3.00 g of NO? b. What is the complete equation (including heat) for the decomposition of NO? c. How many kilocalories are released when 5.00 g of NO decomposes to N2 and O2? The formation of rust 1Fe 2O32 from solid iron and oxygen gas releases 1.7 * 103 kJ. (9) 4Fe1s2 + 3O21g2 h 2Fe 2O31s2 H = - 1.7 * 103 kJ CHEMICAL REACTIONS AND QUANTITIES a. How many kilojoules are released when 2.00 g of Fe reacts? b. How many grams of rust form when 150 kcal are released? c. What is the complete equation (including heat) for the formation of rust? 123 124 Write a balanced equation for each of the following reaction descriptions and identify each type of reaction: (1, 2) a. An aqueous solution of lead(II) nitrate is mixed with aqueous sodium phosphate to produce solid lead(II) phosphate and aqueous sodium nitrate. b. Gallium metal heated in oxygen gas forms solid gallium(III) oxide. c. When solid sodium nitrate is heated, solid sodium nitrite and oxygen gas are produced. d. Solid bismuth(III) oxide and solid carbon react to form bismuth metal and carbon monoxide gas. 126 2C2H21g2 + 5O21g2 h 4CO21g2 + 2H2O1g2 127 A gold bar is 2.31 cm long, 1.48 cm wide, and 0.0758 cm thick. (4, 5) a. If gold has a density of 19.3 g/mL, what is the mass, in grams, of the gold bar? b. How many atoms of gold are in the bar? c. When the same mass of gold combines with oxygen, the oxide product has a mass of 5.61 g. How many moles of O are combined with the gold? Consider the following equation: (1, 2, 6, 7, 8) a. Balance the equation. b. Identify the type of reaction. c. How many moles of oxygen are needed to react with 4.50 moles of Al? d. How many grams of aluminum oxide are produced when 50.2 g of aluminum reacts? e. When 13.5 g of aluminum is reacted with 8.00 g of oxygen, how many grams of aluminum oxide can form? f. If 45.0 g of aluminum and 62.0 g of oxygen undergo a reaction that has a 70.0% yield, what mass of aluminum oxide forms? Components in toothpaste include triclosan and NaF. 125 a. How many moles of water are produced from the complete reaction of 2.50 moles of oxygen? b. How many grams of oxygen are needed to react completely with 2.25 g of acetylene? c. How many grams of carbon dioxide are produced from the complete reaction of 78.0 g of acetylene? d. If the reaction in part c produces 186 g of CO2, what is the percent yield of CO2 for the reaction? Al1s2 + O21g2 h Al2O31s2 A toothpaste contains 0.24% by mass sodium fluoride 1NaF2 used to prevent dental caries and 0.30% by mass triclosan, C12H7Cl3O2, a preservative and antigingivitis agent. One tube contains 119 g of toothpaste. (4, 5) Pearson Education a. How many moles of NaF are in the tube of toothpaste? b. How many fluoride ions 1F -2 are in the tube of toothpaste? c. How many grams of sodium ion 1Na+2 are in 1.50 g of toothpaste? d. How many molecules of triclosan are in the tube of toothpaste? The gaseous hydrocarbon acetylene, C2H2, used in welders’ torches, releases a large amount of heat when it burns according to the following equation: (6, 7, 8) 128 Consider the equation for the reaction of sodium and nitrogen to form sodium nitride. (1, 2, 6, 7, 8) Na1s2 + N21g2 h Na 3N1s2 a. Balance the equation. b. If 80.0 g of sodium is reacted with 20.0 g of nitrogen gas, what mass of sodium nitride forms? c. If the reaction in part b has a percent yield of 75.0%, how many grams of sodium nitride are actually produced? AN SW ER S Answers to Study Checks Answers to Selected Questions and Problems 1 2Al1s2 + 3Cl21g2 h 2AlCl31s2 2 Sb 2S31s2 + 6HCl1aq2 h 2SbCl31s2 + 3H2S1g2 3 0.432 mole of H2O 4 0.120 mole of aspirin 5 138.1 g/mole 6 80.9 g of Ag 3 a. b. c. d. e. b. balanced d. balanced N21g2 + O21g2 h 2NO1g2 2HgO1s2 h 2Hg1l2 + O21g2 4Fe1s2 + 3O21g2 h 2Fe 2O31s2 2Na1s2 + Cl21g2 h 2NaCl1s2 2Cu2O1s2 + O21g2 h 4CuO1s2 5 a. Mg1s2 + 2AgNO31aq2 h Mg1NO3221aq2 + 2Ag1s2 b. CuCO31s2 h CuO1s2 + CO21g2 7 0.945 mole of O2 c. C5H121g2 + 8O21g2 h 5CO21g2 + 6H2O1g2 d. Pb1NO3221aq2 + 2NaCl1aq2 h PbCl21s2 + 2NaNO31aq2 e. 2Al1s2 + 6HCl1aq2 h 2AlCl31aq2 + 3H21g2 8 27.5 g of CO2 9 84.7% yield 10 14.2 g of SO2 11 a. endothermic 1 a. not balanced c. not balanced b. 10.5 kJ 257 CHEMICAL REACTIONS AND QUANTITIES 7 a. b. c. d. decomposition reaction single replacement reaction combustion reaction double replacement reaction 9 a. b. c. d. e. f. single replacement reaction combination reaction decomposition reaction combustion reaction double replacement reaction double replacement reaction 11 a. Mg1s2 + Cl21g2 h MgCl21s2 b. 2HBr1g2 h H21g2 + Br21g2 c. Mg1s2 + Zn1NO3221aq2 h Zn1s2 + Mg1NO3221aq2 d. K2S1aq2 + Pb1NO3221aq2 h 2KNO31aq2 + PbS1s2 e. 2C5H101l2 + 15O21g2 h 10CO21g2 + 10H2O1g2 13 a. reduction c. reduction 15 a. b. c. d. b. oxidation d. reduction Zn is oxidized; Cl2 is reduced. Br - in NaBr is oxidized; Cl2 is reduced. The O2- in PbO is oxidized; the Pb2+ is reduced. Sn2+ is oxidized; Fe3+ is reduced. 17 a. reduction b. oxidation 19 Linoleic acid gains hydrogen atoms and is reduced. 21 a. 1.20 * 1023 atoms of Ag b. 4.52 * 1023 molecules of C3H8O c. 7.53 * 1023 atoms of Cr 23 a. 5.42 moles of Al c. 0.478 mole of Au b. 14.1 moles of C2H5OH 25 a. 24 moles of H c. 0.040 mole of N b. 1.0 * 102 moles of C 27 a. 3.01 * 1023 atoms of C b. 7.71 * 1023 molecules of SO2 c. 0.0867 mole of Fe 258 1 mole O2 2 moles SO2 and 1 mole O2 2 moles SO2 2 moles SO3 2 moles SO2 and 2 moles SO3 2 moles SO2 2 moles SO3 1 mole O2 and 1 mole O2 2 moles SO3 5 moles O2 4 moles P b. and 5 moles O2 4 moles P 2 moles P2O5 4 moles P and 2 moles P2O5 4 moles P 2 moles P2O5 5 moles O2 and 2 moles P2O5 5 moles O2 45 a. 29 a. 6.00 moles of H c. 1.20 * 1024 atoms of P b. 8.00 moles of O d. 4.82 * 1024 atoms of O 31 a. 188.2 g/mole c. 329.2 g/mole e. 58.3 g/mole b. 159.8 g/mole d. 342.3 g/mole f. 365.3 g/mole 33 a. 46.0 g c. 14.8 g b. 112 g d. 112 g 35 a. 29.3 g c. 4.05 g b. 109 g d. 194 g 37 a. 602 g b. 11 g 39 a. 0.463 mole of Ag c. 0.882 mole of NH3 b. 0.0167 mole of C d. 1.17 moles of SO2 41 a. 0.78 mole of S c. 0.601 mole of S b. 1.95 moles of S 43 a. 165 g of caffeine c. 1.15 moles of C b. 0.144 mole of caffeine d. 8.08 g of N 47 a. 1.0 mole of O2 b. 10. moles of H2 c. 5.0 moles of H2O 49 a. 1.25 moles of C c. 1.0 mole of SO2 b. 0.96 mole of CO d. 0.50 mole of CS2 51 a. 77.5 g of Na 2O b. 6.26 g of O2 c. 19.4 g of O2 53 a. 19.2 g of O2 b. 3.79 g of N2 c. 54.0 g of H2O 55 a. 3.65 g of H2O b. 3.43 g of NO c. 7.53 g of HNO3 57 a. b. c. d. 2PbS1s2 + 3O21g2 h 2PbO1s2 + 2SO21g2 6.00 g of O2 17.4 g of SO2 137 g of PbS 59 a. 70.9% b. 63.2% 61 70.8 g of Al2O3 63 60.4% 65 a. Eight taxis can be used to pick up passengers. b. Seven taxis can be driven. 67 a. 5.0 moles of H2 b. 4.0 moles of H2 c. 3.0 moles of N2 69 a. limiting reactant SO2; 2.00 moles of SO3 b. limiting reactant H2O; 0.500 mole of Fe 3O4 c. limiting reactant O2; 1.27 moles of CO2 71 a. limiting reactant Cl2; 25.1 g of AlCl3 b. limiting reactant O2; 13.5 g of H2O c. limiting reactant O2; 26.7 g of SO2 73 a. The activation energy is the energy required to break the bonds of the reacting molecules. b. In exothermic reactions, the energy of the products is lower than that of the reactants. c. Energy Reactants Products Reaction progress 75 a. exothermic b. endothermic 77 a. exothermic; H = -890 kJ b. endothermic; H = +65.3 kJ c. exothermic; H = -205 kcal 79 578 kJ are released c. exothermic CHEMICAL REACTIONS AND QUANTITIES 81 a. 1, 1, 2 combination reaction b. 2, 2, 1 decomposition reaction 83 a. reactants NO, O2; product NO2 b. 2NO1g2 + O21g2 h 2NO21g2 c. combination reaction 89 1. a. S2Cl2 2. a. C6H6 b. 135.2 g/mole b. 78.1 g/mole c. 0.0740 mole c. 0.128 mole 91 a. 252 g/mole b. 0.0991 mole c. 0.991 mole of C 93 a. b. c. d. 66.2 g of propane 0.771 mole of propane 27.8 g of C 2.77 * 1022 atoms of H 95 a. NH31g2 + HCl1g2 h NH4Cl1s2 Combination b. Fe 3O41s2 + 4H21g2 h 3Fe1s2 + 4H2O1g2 Single replacement c. 2Sb1s2 + 3Cl21g2 h 2SbCl31s2 Combination d. C5H121g2 + 8O21g2 h 5CO21g2 + 6H2O1g2 Combustion e. 2KBr1aq2 + Cl21aq2 h 2KCl1aq2 + Br21l2 Single replacement f. Al21SO4231aq2 + 6NaOH1aq2 h 3Na 2SO41aq2 + 2Al1OH231s2 Double replacement 97 a. b. c. d. 99 a. b. c. d. e. f. 101 a. b. c. d. b. 389.9 g/mole c. 169.1 g/mole 105 a. 5.87 g b. 10.7 g c. 15.9 g 107 a. 0.568 mole b. 0.321 mole c. 0.262 mole 109 a. 242 g of glucose b. 123 g of ethanol 85 a. reactant NI 3; products N2, I 2 b. 2NI 31s2 h N21g2 + 3I 21g2 c. decomposition reaction 87 a. reactants Cl2, O2; product OCl2 b. 2Cl21g2 + O21g2 h 2OCl21g2 c. combination reaction 103 a. 161.5 g/mole Zn1s2 + 2HCl1aq2 h ZnCl21aq2 + H21g2 BaCO31s2 h BaO1s2 + CO21g2 NaOH1aq2 + HCl1aq2 h NaCl1aq2 + H2O1l2 2Al1s2 + 3F21g2 h 2AlF31s2 Cu01s2 is oxidized and H +1aq2 is reduced. Fe01s2 is oxidized and Ni2+1aq2 is reduced. Ag 01s2 is oxidized and Cu2+1aq2 is reduced. Cr01s2 is oxidized and Ni2+1aq2 is reduced. Zn01s2 is oxidized and Cu2+1aq2 is reduced. Zn01s2 is oxidized and Pb2+1aq2 is reduced. 111 a. b. c. d. 2NH31g2 + 5F21g2 h N2F41g2 + 6HF1g2 1.33 moles of NH3 and 3.33 moles of F2 143 g of F2 10.4 g of N2F4 113 a. b. c. d. C2H61g2 + 6Cl21g2 h C2Cl61g2 + 6HCl1g2 9.60 moles of chlorine 364 g of HCl 394 g of hexachloroethane 115 81.4% 117 a. 48 g of C5H12 b. 27.5 g of CO2 c. 92.8 g of CO2 119 16.8 g of NaCl 121 a. 1.08 kcal are released b. 2NO1g2 h N21g2 + O21g2 + 21.6 kcal c. 1.80 kcal are required 123 a. 3Pb1NO3221aq2 + 2Na 3PO41aq2 h Pb 31PO4221s2 + 6NaNO31aq2 Double replacement b. 4Ga1s2 + 3O21g2 h 2Ga 2O31s2 Combination c. 2NaNO31s2 h 2NaNO21s2 + O21g2 Decomposition d. Bi2O31s2 + 3C1s2 h 2Bi1s2 + 3CO1g2 Single replacement 125 a. 5.00 g of gold b. 1.53 * 1022 atoms of Au c. 0.038 mole of oxygen 127 a. b. c. d. e. f. 4Al1s2 + 3O21g2 h 2Al2O31s2 combination reaction 3.38 moles of oxygen 94.8 g of aluminum oxide 17.0 g of aluminum oxide 59.5 g of aluminum oxide 90.1 g/mole 3.01 * 1023 molecules 2.71 * 1024 atoms of C 220 g of lactic acid 259 This page intentionally left blank