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
110 Gasohol is a fuel that contains ethanol 1C 2 H 6 O2, which burns in oxygen 1O 2 2 to give carbon dioxide and water. (6, 7) a. Write the balanced equation for the combustion of ethanol. b. How many moles of O 2 are needed to completely react with 4.0 moles of C 2 H 6 O? c. If a car produces 88 g of CO 2, how many grams of O 2 are used up in the reaction? d. If you add 125 g of C 2 H 6 O to your fuel, how many grams of CO 2 and H 2 O can be produced from the ethanol? 111 When ammonia 1NH 3 2 reacts with fluorine, the products are dinitrogen tetrafluoride and hydrogen fluoride. (1, 6, 7) b. How many moles of each reactant are needed to produce 4.00 moles of HF? c. How many grams of F 2 are required to react with 25.5 g of NH 3? d. How many grams of N 2 F 4 can be produced when 3.40 g of NH 3 reacts? 112 When peroxide 1H 2 O 2 2 is used in rocket fuels, it produces water and oxygen 1O 2 2. (1, 6, 7) 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 O 2? d. How many grams of water can be produced when 12.2 g of peroxide reacts? 113 Ethane gas, C 2 H 6, reacts with chlorine gas, Cl 2, to form hexachloroethane gas, C 2 Cl 6, and hydrogen chloride gas. (1, 6, 7) 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? 114 Propane gas, C 3 H 8, 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 Propane is converted to carbon dioxide and water when used as a fuel in a barbecue. b. How many grams of water form when 5.00 L of propane gas completely react? c. How many grams of CO 2 are produced from 18.5 g of oxygen gas and excess propane? d. How many grams of H 2 O can be produced from the reaction of 8.50 * 10 22 molecules of propane gas? 115 Acetylene gas, C 2 H 2, burns in oxygen to produce carbon dioxide and water. If 62.0 g of CO 2 is produced when 22.5 g of C 2 H 2 reacts with sufficient oxygen, what is the percent yield of CO 2 for the reaction? (1, 6, 7, 8) 116 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 2 O 3 1s2 + 3CO1g2 h 2Fe1s2 + 3CO 2 1g2 CHALLENGE QUESTIONS 117 Pentane gas, C 5 H 12, reacts with oxygen to produce carbon dioxide and water. (6, 7, 8) C 5 H 12 1g2 + 8O 2 1g2 h 5CO 2 1g2 + 6H 2 O1g2 Pentane a. How many grams of pentane must react to produce 4.0 moles of water? b. How many grams of CO 2 are produced from 32.0 g of oxygen and excess pentane? c. How many grams of CO 2 are formed if 44.5 g of C 5 H 12 is reacted with 108 g of O 2? 118 When nitrogen dioxide 1NO 2 2 from car exhaust combines with water in the air, it forms nitric acid 1HNO 3 2, which causes acid rain, and nitrogen oxide. (6, 7, 8) 256 3NO 2 1g2 + H 2 O1l2 h 2HNO 3 1aq2 + NO1g2 a. How many molecules of NO 2 are needed to react with 0.250 mole of H 2 O? b. How many grams of HNO 3 are produced when 60.0 g of NO 2 completely reacts? c. How many grams of HNO 3 can be produced if 225 g of NO 2 is reacted with 55.2 g of H 2 O? 119 When a mixture of 12.8 g of Na and 10.2 g of Cl 2 reacts, what is the mass of NaCl that is produced? (6, 7, 8) 2Na1s2 + Cl 2 1g2 h 2NaCl1s2 120 If a mixture of 35.8 g of CH 4 and 75.5 g of S reacts, how many grams of H 2 S are produced? (6, 7, 8) CH 4 1g2 + 4S1g2 h CS 2 1g2 + 2H 2 S1g2 121 The formation of nitrogen oxide, NO, from N 2 1g2 and O 2 1g2, requires 21.6 kcal of heat. (9) N 2 1g2 + O 2 1g2 h 2NO1g2 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 N 2 and O 2? 122 The formation of rust 1Fe 2 O 3 2 from solid iron and oxygen gas releases 1.7 * 10 3 kj. (9) 4Fe1s2 + 3O 2 1g2 h 2Fe 2 O 3 1s2 H = -1.7 * 10 3 kj
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 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. 124 A toothpaste contains 0.24% by mass sodium fluoride 1NaF2 used to prevent dental caries and 0.30% by mass triclosan, C 12 H 7 Cl 3 O 2, a preservative and antigingivitis agent. One tube contains 119 g of toothpaste. (4, 5) Components in toothpaste include triclosan and NaF. 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? 125 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? 126 The gaseous hydrocarbon acetylene, C 2 H 2, used in welders torches, releases a large amount of heat when it burns according to the following equation: (6, 7, 8) 2C 2 H 2 1g2 + 5O 2 1g2 h 4CO 2 1g2 + 2H 2 O1g2 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 CO 2, what is the percent yield of CO 2 for the reaction? 127 Consider the following equation: (1, 2, 6, 7, 8) Al1s2 + O 2 1g2 h Al 2 O 3 1s2 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? 128 Consider the equation for the reaction of sodium and nitrogen to form sodium nitride. (1, 2, 6, 7, 8) Na1s2 + N 2 1g2 h Na 3 N1s2 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? ANSWERS Answers to Study Checks 1 2Al1s2 + 3Cl 2 1g2 h 2AlCl 3 1s2 2 Sb 2 S 3 1s2 + 6HCl1aq2 h 2SbCl 3 1s2 + 3H 2 S1g2 3 0.432 mole of H 2 O 4 0.120 mole of aspirin 5 138.1 g/mole 6 80.9 g of Ag 7 0.945 mole of O 2 8 27.5 g of CO 2 9 84.7% yield 10 14.2 g of SO 2 11 a. endothermic b. 10.5 kj Answers to Selected Questions and Problems 1 a. not balanced b. balanced c. not balanced d. balanced 3 a. N 2 1g2 + O 2 1g2 h 2NO1g2 b. 2HgO1s2 h 2Hg1l2 + O 2 1g2 c. 4Fe1s2 + 3O 2 1g2 h 2Fe 2 O 3 1s2 d. 2Na1s2 + Cl 2 1g2 h 2NaCl1s2 e. 2Cu 2 O1s2 + O 2 1g2 h 4CuO1s2 5 a. Mg1s2 + 2AgNO 3 1aq2 h Mg1NO 3 2 2 1aq2 + 2Ag1s2 b. CuCO 3 1s2 h CuO1s2 + CO 2 1g2 c. C 5 H 12 1g2 + 8O 2 1g2 h 5CO 2 1g2 + 6H 2 O1g2 d. Pb1NO 3 2 2 1aq2 + 2NaCl1aq2 h PbCl 2 1s2 + 2NaNO 3 1aq2 e. 2Al1s2 + 6HCl1aq2 h 2AlCl 3 1aq2 + 3H 2 1g2 257
7 a. decomposition reaction b. single replacement reaction c. combustion reaction d. double replacement reaction 9 a. single replacement reaction b. combination reaction c. decomposition reaction d. combustion reaction e. double replacement reaction f. double replacement reaction 11 a. Mg1s2 + Cl 2 1g2 h MgCl 2 1s2 b. 2HBr1g2 h H 2 1g2 + Br 2 1g2 c. Mg1s2 + Zn1NO 3 2 2 1aq2 h Zn1s2 + Mg1NO 3 2 2 1aq2 d. K 2 S1aq2 + Pb1NO 3 2 2 1aq2 h 2KNO 3 1aq2 + PbS1s2 e. 2C 5 H 10 1l2 + 15O 2 1g2 h 10CO 2 1g2 + 10H 2 O1g2 13 a. reduction b. oxidation c. reduction d. reduction 15 a. Zn is oxidized; Cl 2 is reduced. b. Br - in NaBr is oxidized; Cl 2 is reduced. c. The O 2- in PbO is oxidized; the Pb 2+ is reduced. d. Sn 2+ is oxidized; Fe 3+ is reduced. 17 a. reduction b. oxidation 19 Linoleic acid gains hydrogen atoms and is reduced. 21 a. 1.20 * 10 23 atoms of Ag b. 4.52 * 10 23 molecules of C 3 H 8 O c. 7.53 * 10 23 atoms of Cr 23 a. 5.42 moles of Al b. 14.1 moles of C 2 H 5 OH c. 0.478 mole of Au 25 a. 24 moles of H b. 1.0 * 10 2 moles of C c. 0.040 mole of N 27 a. 3.01 * 10 23 atoms of C b. 7.71 * 10 23 molecules of SO 2 c. 0.0867 mole of Fe 29 a. 6.00 moles of H b. 8.00 moles of O c. 1.20 * 10 24 atoms of P d. 4.82 * 10 24 atoms of O 31 a. 188.2 g/mole b. 159.8 g/mole c. 329.2 g/mole d. 342.3 g/mole e. 58.3 g/mole f. 365.3 g/mole 33 a. 46.0 g b. 112 g c. 14.8 g d. 112 g 35 a. 29.3 g b. 109 g c. 4.05 g d. 194 g 37 a. 602 g b. 11 g 39 a. 0.463 mole of Ag b. 0.0167 mole of C c. 0.882 mole of NH 3 d. 1.17 moles of SO 2 41 a. 0.78 mole of S b. 1.95 moles of S c. 0.601 mole of S 43 a. 165 g of caffeine b. 0.144 mole of caffeine c. 1.15 moles of C d. 8.08 g of N 45 a. 2 moles SO 2 and 1 mole O 2 1 mole O 2 2 moles SO 2 2 moles SO 2 and 2 moles SO 3 2 moles SO 3 2 moles SO 2 2 moles SO 3 and 1 mole O 2 1 mole O 2 2 moles SO 3 4 moles P b. and 5 moles O 2 5 moles O 2 4 moles P 4 moles P and 2 moles P 2O 5 2 moles P 2 O 5 4 moles P 5 moles O 2 and 2 moles P 2O 5 2 moles P 2 O 5 5 moles O 2 47 a. 1.0 mole of O 2 b. 10. moles of H 2 c. 5.0 moles of H 2 O 49 a. 1.25 moles of C b. 0.96 mole of CO c. 1.0 mole of SO 2 d. 0.50 mole of CS 2 51 a. 77.5 g of Na 2 O b. 6.26 g of O 2 c. 19.4 g of O 2 53 a. 19.2 g of O 2 b. 3.79 g of N 2 c. 54.0 g of H 2 O 55 a. 3.65 g of H 2 O b. 3.43 g of NO c. 7.53 g of HNO 3 57 a. 2PbS1s2 + 3O 2 1g2 h 2PbO1s2 + 2SO 2 1g2 b. 6.00 g of O 2 c. 17.4 g of SO 2 d. 137 g of PbS 59 a. 70.9% b. 63.2% 61 70.8 g of Al 2 O 3 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 H 2 b. 4.0 moles of H 2 c. 3.0 moles of N 2 69 a. limiting reactant SO 2 ; 2.00 moles of SO 3 b. limiting reactant H 2 O; 0.500 mole of Fe 3 O 4 c. limiting reactant O 2 ; 1.27 moles of CO 2 71 a. limiting reactant Cl 2 ; 25.1 g of AlCl 3 b. limiting reactant O 2 ; 13.5 g of H 2 O c. limiting reactant O 2 ; 26.7 g of SO 2 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 c. exothermic 77 a. exothermic; H = -890 kj b. endothermic; H = +65.3 kj c. exothermic; H = -205 kcal 79 578 kj are released 258
81 a. 1, 1, 2 combination reaction b. 2, 2, 1 decomposition reaction 83 a. reactants NO, O 2 ; product NO 2 b. 2NO1g2 + O 2 1g2 h 2NO 2 1g2 c. combination reaction 85 a. reactant NI 3 ; products N 2, I 2 b. 2NI 3 1s2 h N 2 1g2 + 3I 2 1g2 c. decomposition reaction 87 a. reactants Cl 2, O 2 ; product OCl 2 b. 2Cl 2 1g2 + O 2 1g2 h 2OCl 2 1g2 c. combination reaction 89 1. a. S 2 Cl 2 b. 135.2 g/mole c. 0.0740 mole 2. a. C 6 H 6 b. 78.1 g/mole c. 0.128 mole 91 a. 252 g/mole b. 0.0991 mole c. 0.991 mole of C 93 a. 66.2 g of propane b. 0.771 mole of propane c. 27.8 g of C d. 2.77 * 10 22 atoms of H 95 a. NH 3 1g2 + HCl1g2 h NH 4 Cl1s2 Combination b. Fe 3 O 4 1s2 + 4H 2 1g2 h 3Fe1s2 + 4H 2 O1g2 Single replacement c. 2Sb1s2 + 3Cl 2 1g2 h 2SbCl 3 1s2 Combination d. C 5 H 12 1g2 + 8O 2 1g2 h 5CO 2 1g2 + 6H 2 O1g2 Combustion e. 2KBr1aq2 + Cl 2 1aq2 h 2KCl1aq2 + Br 2 1l2 Single replacement f. Al 2 1SO 4 2 3 1aq2 + 6NaOH1aq2 h 3Na 2 SO 4 1aq2 + 2Al1OH2 3 1s2 Double replacement 97 a. Zn1s2 + 2HCl1aq2 h ZnCl 2 1aq2 + H 2 1g2 b. BaCO 3 1s2 h BaO1s2 + CO 2 1g2 c. NaOH1aq2 + HCl1aq2 h NaCl1aq2 + H 2 O1l2 d. 2Al1s2 + 3F 2 1g2 h 2AlF 3 1s2 99 a. Cu 0 1s2 is oxidized and H + 1aq2 is reduced. b. Fe 0 1s2 is oxidized and Ni 2+ 1aq2 is reduced. c. Ag 0 1s2 is oxidized and Cu 2+ 1aq2 is reduced. d. Cr 0 1s2 is oxidized and Ni 2+ 1aq2 is reduced. e. Zn 0 1s2 is oxidized and Cu 2+ 1aq2 is reduced. f. Zn 0 1s2 is oxidized and Pb 2+ 1aq2 is reduced. 101 a. 90.1 g/mole b. 3.01 * 10 23 molecules c. 2.71 * 10 24 atoms of C d. 220 g of lactic acid 103 a. 161.5 g/mole 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 111 a. 2NH 3 1g2 + 5F 2 1g2 h N 2 F 4 1g2 + 6HF1g2 b. 1.33 moles of NH 3 and 3.33 moles of F 2 c. 143 g of F 2 d. 10.4 g of N 2 F 4 113 a. C 2 H 6 1g2 + 6Cl 2 1g2 h C 2 Cl 6 1g2 + 6HCl1g2 b. 9.60 moles of chlorine c. 364 g of HCl d. 394 g of hexachloroethane 115 81.4% 117 a. 48 g of C 5 H 12 b. 27.5 g of CO 2 c. 92.8 g of CO 2 119 16.8 g of NaCl 121 a. 1.08 kcal are released b. 2NO1g2 h N 2 1g2 + O 2 1g2 + 21.6 kcal c. 1.80 kcal are required 123 a. 3Pb1NO 3 2 2 1aq2 + 2Na 3 PO 4 1aq2 h Pb 3 1PO 4 2 2 1s2 + 6NaNO 3 1aq2 Double replacement b. 4Ga1s2 + 3O 2 1g2 h 2Ga 2 O 3 1s2 Combination c. 2NaNO 3 1s2 h 2NaNO 2 1s2 + O 2 1g2 Decomposition d. Bi 2 O 3 1s2 + 3C1s2 h 2Bi1s2 + 3CO1g2 Single replacement 125 a. 5.00 g of gold b. 1.53 * 10 22 atoms of Au c. 0.038 mole of oxygen 127 a. 4Al1s2 + 3O 2 1g2 h 2Al 2 O 3 1s2 b. combination reaction c. 3.38 moles of oxygen d. 94.8 g of aluminum oxide e. 17.0 g of aluminum oxide f. 59.5 g of aluminum oxide 259
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