Chemistry: Structure and Properties (2nd Edition)
2nd Edition
ISBN: 9780134293936
Author: Nivaldo J. Tro
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 9, Problem 40E
A kilogram of aluminum metal and a kilogram of water are each warmed to 75 °C and placed in two identical insulated containers. One hour later, the two containers are opened, and the temperature of each substance is measured. The aluminum has cooled to 35 °C, while the water has cooled only to 66 °C. Explain this difference.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 9 Solutions
Chemistry: Structure and Properties (2nd Edition)
Ch. 9 - What is thermochemistry? Why is it important?Ch. 9 - What is energy? What is work? List some examples...Ch. 9 - Prob. 3ECh. 9 - What is the law of conservation of energy? How...Ch. 9 - A friend claims to have constructed a machine that...Ch. 9 - What is a state function? List some examples of...Ch. 9 - What is internal energy? Is internal energy a...Ch. 9 - If energy flows out of a chemical system and into...Ch. 9 - If the internal energy of the products of a...Ch. 9 - What is heat? Explain the difference between heat...
Ch. 9 - How is the change in internal energy of a system...Ch. 9 - Explain how the sum of heat and work can be a...Ch. 9 - What is heat capacity? Explain the difference...Ch. 9 - Explain how the high specific heat capacity of...Ch. 9 - If two objects, A and B, of different temperature...Ch. 9 - What is pressure-volume work? How is it...Ch. 9 - What is calorimetry? Explain the difference...Ch. 9 - What is the change in enthalpy ( H) for a...Ch. 9 - Explain the difference between an exothermic and...Ch. 9 - From a molecular viewpoint where does the energy...Ch. 9 - From a molecular viewpoint, where does the energy...Ch. 9 - Is the change in enthalpy for a reaction an...Ch. 9 - Explain how the value of H for a reaction changes...Ch. 9 - What is Hess's law? Why is it useful?Ch. 9 - What is a standard state? What is the standard...Ch. 9 - How can bond energies be used to estimate H for a...Ch. 9 - Explain the difference between exothermic and...Ch. 9 - What is the standard enthalpy of formation for a...Ch. 9 - How do you calculate Hrxn from tabulated standard...Ch. 9 - What is lattice energy? How does lattice energy...Ch. 9 - Which statement is true of the internal energy of...Ch. 9 - During an energy exchange, a chemical system...Ch. 9 - Identify each energy exchange as primarily heat or...Ch. 9 - Identify each energy exchange as primarily heat or...Ch. 9 - A system releases 622 kJ of heat and does 105 kJ...Ch. 9 - A system absorbs 196 kJ of heat, and the...Ch. 9 - The gas in a piston (defined as the system) warms...Ch. 9 - The air in an inflated balloon (defined as the...Ch. 9 - A person packs two identical coolers for a picnic,...Ch. 9 - A kilogram of aluminum metal and a kilogram of...Ch. 9 - How much heat is required to warm 1.50 L of water...Ch. 9 - How much heat is required to warm 1.50 kg of sand...Ch. 9 - Suppose that 25 g of each substance is initially...Ch. 9 - An unknown mass of each substance, initially at...Ch. 9 - How much work (in J) is required to expand the...Ch. 9 - The average human lung expands by about 0.50 L...Ch. 9 - The air within a piston equipped with a cylinder...Ch. 9 - A gas is compressed from an initial volume of 5.55...Ch. 9 - When 1 mol of a fuel burns at constant pressure,...Ch. 9 - The change in internal energy for the combustion...Ch. 9 - Is each process exothermic or endothermic?...Ch. 9 - Is each process exothermic or endothermic?...Ch. 9 - Consider the thermochemical equation for the...Ch. 9 - What mass of natural gas (CH4) must bum to emit...Ch. 9 - Nitromethane (CH3NO2) burns in air to produce...Ch. 9 - Titanium reacts with iodine to form titanium (III)...Ch. 9 - The propane fuel (C3H8) used in gas barbeques bums...Ch. 9 - Charcoal is primarily carbon. Determine the mass...Ch. 9 - We submerge a silver block, initially at 58.5 °C...Ch. 9 - We submerge a 32.5-g iron rod, initially at 22.7...Ch. 9 - We submerge a 31.1-g wafer of pure gold initially...Ch. 9 - We submerge a 2.85-g lead weight, initially at...Ch. 9 - Two substances, A and B, initially at different...Ch. 9 - A 2.74-g sample of a substance suspected of being...Ch. 9 - Exactly 1.5 g of a fuel burns under conditions of...Ch. 9 - In order to obtain the largest possible amount of...Ch. 9 - When 0.514 g of biphenyl (C12H10) undergoes...Ch. 9 - Mothballs are composed primarily of the...Ch. 9 - Zinc metal reacts with hydrochloric acid according...Ch. 9 - Instant cold packs used to ice athletic injuries...Ch. 9 - For each generic reaction, determine the value of...Ch. 9 - Consider the generic reaction: A+2BC+3DH=155kJ...Ch. 9 - Calculate Hrxn for the reaction:...Ch. 9 - Calculate Hrxn for the reaction:...Ch. 9 - Calculate Hrxn for the reaction:...Ch. 9 - Calculate Hrxn for the reaction:...Ch. 9 - Hydrogenation reactions are used to add hydrogen...Ch. 9 - Ethanol is a possible fuel. Use average bond...Ch. 9 - Hydrogen, a potential future fuel, can be produced...Ch. 9 - Hydroxyl radicals react with and eliminate many...Ch. 9 - Write an equation for the formation of each...Ch. 9 - Prob. 82ECh. 9 - S3. Hydrazine (N2H4) is a fuel used by some...Ch. 9 - Prob. 84ECh. 9 - Prob. 85ECh. 9 - Prob. 86ECh. 9 - Prob. 87ECh. 9 - Prob. 88ECh. 9 - Top fuel dragsters and funny cars burn...Ch. 9 - Prob. 90ECh. 9 - Prob. 91ECh. 9 - Rubidium iodide has a lattice energy of-617...Ch. 9 - Prob. 93ECh. 9 - Prob. 94ECh. 9 - Use the Born-Haber cycle and data from Appendix...Ch. 9 - Prob. 96ECh. 9 - The kinetic energy of a rolling billiard ball is...Ch. 9 - A100-W light bulb is placed in a cylinder equipped...Ch. 9 - Evaporating sweat cools the body because...Ch. 9 - LP gas burns according to the exothermic reaction:...Ch. 9 - Use standard enthalpies of formation to calculate...Ch. 9 - Dry ice is solid carbon dioxide. Instead of...Ch. 9 - A 25.5-g aluminum block is warmed to 65.4 °C and...Ch. 9 - We mix 50.0 mL of ethanol (density = 0.789 g/mL)...Ch. 9 - Prob. 105ECh. 9 - Prob. 106ECh. 9 - One tablespoon of peanut butter has a mass of 16...Ch. 9 - Prob. 108ECh. 9 - Prob. 109ECh. 9 - When we burn 10.00 g of phosphorus in O2 (g) to...Ch. 9 - The H for the oxidation of S in the gas phase to...Ch. 9 - The Hfo of TiI3(s) is -328 kJ/mol; and the Ho for...Ch. 9 - A copper cube measuring 1.55 cm on edge and an...Ch. 9 - A pure gold ring and pure silver ring have a total...Ch. 9 - The reaction of Fe2O3(s) with Al(s) to form...Ch. 9 - Prob. 116ECh. 9 - Prob. 117ECh. 9 - Prob. 118ECh. 9 - Prob. 119ECh. 9 - Calculate the heat of atomization (see previous...Ch. 9 - Prob. 121ECh. 9 - Prob. 122ECh. 9 - Prob. 123ECh. 9 - Prob. 124ECh. 9 - Prob. 125ECh. 9 - Find H, E, q, and w for the freezing of water at...Ch. 9 - The heat of vaporization of water at 373 K is 40.7...Ch. 9 - Prob. 128ECh. 9 - Prob. 129ECh. 9 - Prob. 130ECh. 9 - Prob. 131ECh. 9 - Prob. 132ECh. 9 - Prob. 133ECh. 9 - Which expression describes the heat emitted in a...Ch. 9 - Prob. 135ECh. 9 - Prob. 136ECh. 9 - Prob. 137ECh. 9 - Prob. 138ECh. 9 - Prob. 139ECh. 9 - Which statement is true of a reaction in which V...Ch. 9 - Which statement is true of an endothermic...Ch. 9 - When a firecracker explodes, energy is obviously...Ch. 9 - Prob. 143ECh. 9 - Classify each process as endothermic or...Ch. 9 - A propane tank on a home barbeque contains 10.4 x...Ch. 9 - Prob. 146ECh. 9 - Consider the decomposition of liquid hydrogen...Ch. 9 - Prob. 148ECh. 9 - A chemical system produces 155 kJ of heat and does...Ch. 9 - Which sample is most likely to undergo the...Ch. 9 - Prob. 3SAQCh. 9 - A 12.5-g sample of granite initially at 82.0 C is...Ch. 9 - A cylinder with a moving piston expands from an...Ch. 9 - When a 3.80-g sample of liquid octane (C8H18)...Ch. 9 - Hydrogen gas reacts with oxygen to form water....Ch. 9 - Manganese reacts with hydrochloric acid to produce...Ch. 9 - Consider the reactions: A2BH1A3CH2 What is H for...Ch. 9 - Use standard enthalpies of formation to determine...Ch. 9 - Prob. 11SAQCh. 9 - Prob. 12SAQCh. 9 - Prob. 13SAQCh. 9 - Which set of compounds is arranged in order of...Ch. 9 - Prob. 15SAQ
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
- A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. 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 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forwardThe equation for the fermentation of glucose to alcohol and carbon dioxide is: C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g) The enthalpy change for the reaction is 67 kJ. Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?arrow_forwardEnthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21C. To heat the water sample to 41C, how much heat must you add to it? b Consider the hypothetical reaction,2X(aq)+Y(l)X2Y(aq)being run in an insulated container that contains 100. g of solution. If the temperature of the solution changes from 21C to 31C, how much heat does the chemical reaction produce? How does this answer compare with that in part a? (You can assume that this solution is so dilute that it has the same heat capacity as pure water.) c If you wanted the temperature of 100. g of this solution to increase from 21C to 51C, how much heat would you have to add to it? (Try to answer this question without using a formula.) d If you had added 0.02 mol of X and 0.01 mol of Y to form the solution in part b, how many moles of X and Y would you need to bring about the temperature change described in part c. e Judging on the basis of your answers so far, what is the enthalpy of the reaction 2X(aq) + Y(l) X2Y(aq)?arrow_forward
- Thermal Interactions Part 1: In an insulated container, you mix 200. g of water at 80C with 100. g of water at 20C. After mixing, the temperature of the water is 60C. a How much did the temperature of the hot water change? How much did the temperature of the cold water change? Compare the magnitudes (positive values) of these changes. b During the mixing, how did the heat transfer occur: from hot water to cold, or from cold water to hot? c What quantity of heat was transferred from one sample to the other? d How does the quantity of heat transferred to or from the hot-water sample compare with the quantity of heat transferred to or from the cold-water sample? e Knowing these relative quantities of heat, why is the temperature change of the cold water greater than the magnitude of the temperature change of the hot water. f A sample of hot water is mixed with a sample of cold water that has twice its mass. Predict the temperature change of each of the samples. g You mix two samples of water, and one increases by 20C, while the other drops by 60C. Which of the samples has less mass? How do the masses of the two water samples compare? h A 7-g sample of hot water is mixed with a 3-g sample of cold water. How do the temperature changes of the two water samples compare? Part 2: A sample of water is heated from 10C to 50C. Can you calculate the amount of heat added to the water sample that caused this temperature change? If not, what information do you need to perform this calculation? Part 3: Two samples of water are heated from 20C to 60C. One of the samples requires twice as much heat to bring about this temperature change as the other. How do the masses of the two water samples compare? Explain your reasoning.arrow_forward4.60 Why are fuel additives used?arrow_forwardExplain why oceanfront areas generally have smaller temperature fluctuations than inland areas.arrow_forward
- Classify each process as exothermic or endothermic. (a) ice melts (b) gasoline burns (c) steam condenses (d) reactants products, H = 50 kJarrow_forwardIs the Sun exothermic or endothermic? Is it any less exothermic or endothermic in the winter, as opposed to the summer?arrow_forwardThe best solar panels currently available are about 15% efficient in converting sunlight to electricity. A typical home will use about 40. kWh of electricity per day (1 kWh = 1 kilowatt hour; 1kW = 1000 J/s). Assuming 8.0 hours of useful sunlight per day, calculate the minimum solar panel surface area necessary to provide all of a typical homes electricity. (See Exercise 124 for the energy rate supplied by the sun.)arrow_forward
- xplain why aluminum cans make good storage containers for soft drinks. Styrofoam cups can be used to keep coffee hot and cola cold. How can this be?arrow_forwardWhich molecule, HF, HCl, HBr, or HI, has the strongest chemical bond?arrow_forwardWhat mass of carbon monoxide must be burned to produce 175 kJ of heat under standard state conditions?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY