Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 4, Problem 4.6PAE
4.6 Use the web to research prices of gasoline at the pump for consumers in your area during the past year. Also find information about the price of crude oil for the same period. Discuss any correlations you observe between the two prices.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Consider the reaction between hydrogen gas and bromine gas to form gaseous hydrogen bromide (HBr).
If 7 moles of hydrogen gas are mixed with 5 moles of bromine gas, how many moles of each species will be present when the reaction goes to completion.
Hydrogen gas?
bromine gas?
hydrogen bromide gas?
Aspirin, C₉H₆O₄, is prepared by reacting salicylic acid, C₇H₆O₃, with acetic anhydride, C₄H₆O₃, in the reaction:2C₇H₆O₃ + C₄H₆O₃ → 2C₉H₆O₄ + H₂OA student is told to prepare 22.0 g of aspirin. He is also told that he should use a 50.0% excess of acetic anhydride and expect to get a 64.0% yield in the reaction.How many grams of salicylic acid, C₇H₆O₃, should he use?
And how many grams of acetic anhydride, C₄H₆O₃, should he use?
A possible practical way to eliminate oxides of nitrogen (such as NO2) from automobile exhaust gases uses cyanuric acid, C3N3(OH)3. When heated to the relatively low temperature of 625°F, cyanuric acid converts to gaseous isocyanic acid (HNCO). Isocyanic acid reacts with NO2 in the exhaust to form nitrogen, carbon dioxide, and water, all of which are normal constituents of the air.
(a) Write balanced equations for these two reactions.
(b) If the process described earlier became practical, how much cyanuric acid (in kilograms) would be required to absorb the 1.7 × 1010 kg NO2 generated annually in auto exhaust in the United States?
Chapter 4 Solutions
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 - 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. 4.34PAECh. 4 - Prob. 4.35PAECh. 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. 4.50PAECh. 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. 4.53PAECh. 4 - Prob. 4.54PAECh. 4 - Hydrazine, N2H4, is a weak base and can react with...Ch. 4 - Prob. 4.56PAECh. 4 - Prob. 4.57PAECh. 4 - Prob. 4.58PAECh. 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. 4.62PAECh. 4 - Prob. 4.63PAECh. 4 - 4.64 Using the web, find information about the...Ch. 4 - 4.65 Using the web, find out how lead “poisons”...Ch. 4 - 4.66 If 3.4 mol Al is mixed with 1.5 times as many...Ch. 4 - 4.67 If 8.4 moles of disilane, Si2H6, are combined...Ch. 4 - 4.68 The pictures below show a molecular-scale...Ch. 4 - 4.69 The pictures below show a molecular-scale...Ch. 4 - 4.70 The particulate scale drawing shown depicts...Ch. 4 - 4.71 The particulate scale drawing shown depict...Ch. 4 - 4.72 The picture shown depicts the species present...Ch. 4 - Prob. 4.73PAECh. 4 - Prob. 4.74PAECh. 4 - Prob. 4.75PAECh. 4 - Prob. 4.76PAECh. 4 - You have 0.954 g of an unknown acid, H2A, which...Ch. 4 - Prob. 4.78PAECh. 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. 4.81PAECh. 4 - One way of determining blood alcohol levels is by...Ch. 4 - Prob. 4.83PAECh. 4 - 4.84 Aluminum chloride (AlCl3) is used as a...Ch. 4 - 4.85 In the cold vulcanization of rubber, disulfur...Ch. 4 - Prob. 4.86PAECh. 4 - Prob. 4.87PAECh. 4 - 4.88 A quality control technician needs to...Ch. 4 - Prob. 4.89PAECh. 4 - 4.90 Iron metal can be refined (rom the mineral...Ch. 4 - Prob. 4.91PAECh. 4 - Prob. 4.92PAECh. 4 - 4.93 A mixture of methane (CH4) and propane (C3H8)...Ch. 4 - Prob. 4.94PAECh. 4 - Prob. 4.95PAECh. 4 - Prob. 4.96PAECh. 4 - Prob. 4.97PAECh. 4 - Prob. 4.98PAECh. 4 - Prob. 4.99PAECh. 4 - Prob. 4.100PAECh. 4 - Prob. 4.101PAECh. 4 - Prob. 4.102PAECh. 4 - Prob. 4.103PAECh. 4 - 4.104 When 2.750 g of the oxide Pb3O4 is heated to...Ch. 4 - Prob. 4.105PAECh. 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. 4.109PAECh. 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...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 4.17 Phosgene is a highly toxic gas that has been used as a chemical weapon at times in the past. It is now used in the manufacture of polycarbonates, which are used to make phone cases and plastic eyeglass lenses. Phosgene is produced by the reaction, CO+Cl2COCl2 . Given an excess of carbon monoxide, what mass of chlorine gas must be reacted to form 4.5 g of phosgene?arrow_forwardConsider the balanced chemical equation :math>A+5B3C+4D en equal masses of A and B are reacted, which is limiting, A or B? Justify your choice. If the molar mass of A is greater than the molar mass of B, then A must be limiting. If the molar mass of A is less than the molar mass of B, then A must be limiting. If the molar mass of A is greater than the molar mass of B, then B must be limiting. If the molar mass of A is less than the molar mass of B, then B must be limiting.arrow_forwardThe compound sodium thiosulfate pentahydrate, , is important commercially to the photography business as "hypo", because it has the ability to dissolve unreacted silver salts from photographic film during development. Sodium thiosulfate pentahydrate can be produced by boiling elemental sulfur in an aqueous solution of sodium sulfite. S8 + Na2SO3 + H2O---> NaS2OH2O (unbalanced) What is the theoretical yield of sodium thiosulfate pentahydrate when 2.95 g of sulfur is boiled with 13.6 g of sodium sulfite? Theoretical yield =___ g Sodium thiosulfate pentahydrate is very soluble in water. What is the percent yield of the synthesis if a student doing this experiment is able to isolate (collect) only 5.15 g of the product? Percent yield =____ %arrow_forward
- In the 1980s, there was an international agreement to destroy all stockpiles of mustard gas, ClCH2CH2SCH2CH2Cl. When this substance contacts the moisture in eyes, nasal passages, and skin, the −OH groups of water replace the Cl atoms and create high local concentrations of hydrochloric acid, which cause severe blistering and tissue destruction. Write a balanced equation for this reaction and calculate Δ H o rxn . Do not include states in your equation.arrow_forwardConsider the mixture of ethanol, C2H5OH, and O2 shown inthe accompanying diagram. (a) Write a balanced equationfor the combustion reaction that occurs between ethanoland oxygen. (b) Which reactant is the limiting reactant?(c) How many molecules of CO2, H2O, C2H5OH, and O2 willbe present if the reaction goes to completion?arrow_forwardgiven the unbalance equation CO2+H2 ----> CH4+H2o a) How many moles of water can be produced from 10 moles of CO2 ? b) How many moles of CH4 will be produced along with 14 moles of water?arrow_forward
- The compound geraniol (molar mass 154.25 g/mol) is on the U.S. Food and Drug Administration’s GRAS (Generally Recognized As Safe) list and can be used in foods and personal care products. By itself, geraniol smells like roses, but it is frequently blended with other fragrances on the GRAS list and then added to products to produce a pleasant peachlike or lemonlike aroma. In an analysis, the complete combustion of 175 mg of geraniol produced 499 mg of CO2 and 184 mg of H2O. Give the empirical formula for geraniol, listing carbon and hydrogen at the beginning of the formula followed by oxygen, in that order.arrow_forwardBalance the following reaction. Please place "1" if the coefficient is B2H6 + 3O2 → 2HBO2 + 2H2Oarrow_forwardA student was synthesizing aspirin in the laboratory. Using the amount of limiting reactant, she calculated the mass of aspirin that should form as 10.15 g. When she weighed her aspirin product on the balance, its mass was 6.17 g. Calculate the percent yield for this synthesis.arrow_forward
- ---CH3NH2(g)+---02(g)= CO2(g)+----H2O(g)+----N2(g) Consider the oxidation of methylamine shown in the image above. a.When properly balanced the coefficient infront of O2= ? b. If you want to combust 45.0 g of CH3NH2, how many grams of O2 do you need? c. How many grams of N2 gas can be formed from this oxidation?arrow_forwardWhen you balance the equation FeCl₃ + NH₄OH ---> Fe(OH)₃ + NH₄Cl, what is the coefficient of ammonium chloride? 2 3 1 4arrow_forwardFor the following reaction, 6.61 grams of benzene (C6H6) are mixed with excess oxygen gas. The reaction yields 18.6 grams of carbon dioxide.benzene (C6H6) (l) + oxygen (g) carbon dioxide (g) + water (g) What is the ideal yield of carbon dioxide? grams What is the percent yield for this reaction? %arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
World of ChemistryChemistryISBN:9780618562763Author:Steven S. ZumdahlPublisher:Houghton Mifflin College Div
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
World of Chemistry
Chemistry
ISBN:9780618562763
Author:Steven S. Zumdahl
Publisher:Houghton Mifflin College Div
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Types of Matter: Elements, Compounds and Mixtures; Author: Professor Dave Explains;https://www.youtube.com/watch?v=dggHWvFJ8Xs;License: Standard YouTube License, CC-BY