Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 4, Problem 4.24PAE
4.22 Generally, an excess of O2 is needed for the reaction
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Chemistry for Engineering Students
Ch. 4 - Describe the chemical composition of gasoline.Ch. 4 - Write balanced chemical equations for the...Ch. 4 - Prob. 3COCh. 4 - Calculate the amounts of reactants needed in a...Ch. 4 - Prob. 5COCh. 4 - Prob. 6COCh. 4 - Prob. 7COCh. 4 - 4.1 List at least two factors that make it...Ch. 4 - 4.2 What is an alkane?Ch. 4 - 4.3 Explain the difference between complete and...
Ch. 4 - 4.4 Automobile exhaust often contains traces of...Ch. 4 - 4.5 Methane, ethane, and propane are also...Ch. 4 - 4.6 Use the web to research prices of gasoline at...Ch. 4 - For the following reactions, write the ratios that...Ch. 4 - 4.8 In an experiment carried out at very low...Ch. 4 - 4.9 Sulfur, S8, combines with oxygen at elevated...Ch. 4 - 4.10 How many moles of oxygen can be obtained by...Ch. 4 - 4.11 MTBE, C5H12O, is one of the additives that...Ch. 4 - 4.12 In petroleum refining, hydrocarbons are often...Ch. 4 - 4.13 For the following reactions, determine the...Ch. 4 - 4.14 The combustion of liquid chloroethylene,...Ch. 4 - 4.15 What mass of the unknown compound is formed...Ch. 4 - 4.16 Many metals react with halogens to give metal...Ch. 4 - 4.17 Phosgene is a highly toxic gas that has been...Ch. 4 - Prob. 4.18PAECh. 4 - 4.19 How many metric tons of carbon are required...Ch. 4 - 4.20 Assuming a charcoal briquette is composed...Ch. 4 - 4.21 Ammonium nitrate, NH4NO3, will decompose...Ch. 4 - If 3.4 mol Al and 6.2 mol Fe2O3 are mixed, what is...Ch. 4 - If 8.4 moles of disilane, Si2H6, is combined with...Ch. 4 - 4.22 Generally, an excess of O2 is needed for the...Ch. 4 - 4.23 In the reaction of arsenic with bromine,...Ch. 4 - 4.24 Ammonia gas can be prepared by the reaction...Ch. 4 - 4.25 When octane is combusted with inadequate...Ch. 4 - 4.26 The equation for one of the reactions in the...Ch. 4 - 4.27 Copper reacts with sulfuric acid according to...Ch. 4 - 4.28 One of the steps in the manufacture of nitric...Ch. 4 - 4.29 When Al(OH)3 reacts with sulfuric acid, the...Ch. 4 - 4.30 Copper reacts with nitric acid via the...Ch. 4 - 4.31 How much HNO3 can be formed in the following...Ch. 4 - 4.32 Hydrogen and oxygen are reacted and the water...Ch. 4 - 4.33 Silicon carbide, an abrasive, is made by the...Ch. 4 - Prob. 4.36PAECh. 4 - Prob. 4.37PAECh. 4 - 4.36 Sometimes students in chemistry labs...Ch. 4 - 4.37 The theoretical yield and the actual yield...Ch. 4 - 4.38 A reaction that produced 4.8 mg of taxol, an...Ch. 4 - Methanol, CH3OH, is used in racing cars because it...Ch. 4 - 4.40 When iron and steam react at high...Ch. 4 - 4.41 The percentage yield of the following...Ch. 4 - 4.42 Sulfur hexafluoride is a very stable gas...Ch. 4 - 4.43 Magnesium nitride forms in a side reaction...Ch. 4 - 4.44 Industrial production of hydrogen gas uses...Ch. 4 - 4.45 If 21 g of H2S is mixed with 38 g of O2 and...Ch. 4 - 4.46 A mixture of 10.0 g of NO and 14.0 g of NO2...Ch. 4 - 4.47 Silicon carbide is, an abrasive used in the...Ch. 4 - 4.48 Elemental phosphorous is used in the...Ch. 4 - 4.49 Small quantities of hydrogen gas can be...Ch. 4 - Prob. 4.52PAECh. 4 - 4.51 What is the role of an indicator in a...Ch. 4 - 4.52 What volume of 0.812 M HCl, in milliliters,...Ch. 4 - Prob. 4.55PAECh. 4 - Prob. 4.56PAECh. 4 - Hydrazine, N2H4, is a weak base and can react with...Ch. 4 - Prob. 4.58PAECh. 4 - Prob. 4.59PAECh. 4 - Prob. 4.60PAECh. 4 - 4.59 Aluminum dissolves in HCI according to the...Ch. 4 - 4.60 Why are fuel additives used?Ch. 4 - 4.61 What is actually measured by the octane...Ch. 4 - Prob. 4.64PAECh. 4 - Prob. 4.65PAECh. 4 - 4.64 Using the web, find information about the...Ch. 4 - 4.65 Using the web, find out how lead “poisons”...Ch. 4 - Prob. 4.68PAECh. 4 - You have 0.954 g of an unknown acid, H2A, which...Ch. 4 - Prob. 4.70PAECh. 4 - 4.79 Phosphoric add (H3PO4) is important in the...Ch. 4 - 4.80 The reaction shown below is used to destroy...Ch. 4 - Prob. 4.73PAECh. 4 - One way of determining blood alcohol levels is by...Ch. 4 - Prob. 4.75PAECh. 4 - The pictures below show a molecular-scale view of...Ch. 4 - The pictures below show a molecular-scale view of...Ch. 4 - 4.84 Aluminum chloride (AlCl3) is used as a...Ch. 4 - 4.85 In the cold vulcanization of rubber, disulfur...Ch. 4 - Prob. 4.80PAECh. 4 - Prob. 4.81PAECh. 4 - 4.88 A quality control technician needs to...Ch. 4 - Prob. 4.83PAECh. 4 - 4.90 Iron metal can be refined (rom the mineral...Ch. 4 - Prob. 4.85PAECh. 4 - Prob. 4.86PAECh. 4 - 4.93 A mixture of methane (CH4) and propane (C3H8)...Ch. 4 - Prob. 4.88PAECh. 4 - Prob. 4.89PAECh. 4 - Prob. 4.90PAECh. 4 - Prob. 4.91PAECh. 4 - Prob. 4.92PAECh. 4 - Prob. 4.93PAECh. 4 - Prob. 4.94PAECh. 4 - Prob. 4.95PAECh. 4 - Prob. 4.96PAECh. 4 - Prob. 4.97PAECh. 4 - 4.104 When 2.750 g of the oxide Pb3O4 is heated to...Ch. 4 - Prob. 4.99PAECh. 4 - 4.106 An ore sample with a mass of 670 kg contains...Ch. 4 - 4.107 Existing stockpiles of the refrigerant...Ch. 4 - 4.108 Elemental analysis is sometimes carried out...Ch. 4 - Prob. 4.103PAECh. 4 - 4.110 Write the balanced chemical equation lot the...Ch. 4 - 4.111 Aluminum metal reacts with sulfuric acid to...Ch. 4 - 4.112 A metallurgical firm wishes to dispose of...
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The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
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One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack emissions is by reaction with ammonia gas, NH3. The products of the reaction, N2 and H2O, are not toxic. Write the balanced equation for this reaction. Assign an oxidation number to each element in the reactants and products, and indicate which element is oxidized and which is reduced.
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Phosphoric acid, H3PO4, can be prepared by the reaction of phosphorus(V) oxide, P4O10, with water. 14P4O10(s)+32H2O(l)H3PO4(aq);H=96.2kJ What is H for the reaction involving 1 mol of P4O10? P4O10(s)+6H2O(l)4H3PO4(aq)
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Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.
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4.19 How many metric tons of carbon are required to react with 7.83 metric tons of Fe2O3 according to the following reaction? 2Fe2O3+3C3CO2+4Fe How many metric tons of iron are produced?
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4.20 Assuming a charcoal briquette is composed entirely of carbon, what mass of oxygen is needed to completely burn a 37.3-g briquette?
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High cost and limited availability of a reactant often dictate which reactant is limiting in a particular process. Identify the limiting reactant when the reactions below are run, and come up with a reason to support your decision. a. Burning charcoal on a grill: C(s)+O2(g)CO2(g) b. Burning a chunk of Mg in water: Mg(s)+2H2O(l)Mg(OH)2(aq)+H2(g) c. The Haber process of ammonia production: 3H2(g)+N2(g)2NH3(g)
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Iron forms a sulfide with the approximate formula Fe7S8. Assume that the oxidation state of sulfur is 2 and that iron atoms exist in both +2 and +3 oxidation states. What is the ratio of Fe(II) atoms to Fe(III) atoms in this compound?
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What is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of mercury, if the fish contains 30 parts per million of mercury by weight? (Assume that all the mercury from the fish ends up as mercury (II) chloride in the body and that a fatal dose is 0.20 g of HgCl2.) How many pounds of fish is this?
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Balance each of the following equations, and then write the net ionic equation. Show states for all reactants and products (s, . g, aq). (a) the reaction of sodium hydroxide and iron(II) chloride to give iron(II) hydroxide and sodium chloride (b) the reaction of barium chloride with sodium carbonate to give barium carbonate and sodium chloride (c) the reaction of ammonia with phosphoric acid
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4.28 One of the steps in the manufacture of nitric acid is the oxidation of ammonia shown in this equation: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) If 43.0 kg of NH3 reacts with 35.4 kg of O2, what mass of NO forms?
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Write balanced chemical equations for the following reactions. (a) The reaction of aluminum and iron(III) oxide to form iron and aluminum oxide (known as the thermite reaction). (b) The reaction of carbon and water at high temperature to form a mixture of gaseous CO and H2 (known as water gas and once used as a fuel). (c) The reaction of liquid silicon tetrachloride and magnesium forming silicon and magnesium chloride. This is one step in the preparation of ultrapure silicon used in the semiconductor industry
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