Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 2, Problem 2.82E
The thermite reaction combines aluminum powder and iron oxide and ignites the mixture to make aluminum oxide and iron. So much energy is given off that the iron productfrequently is molten. Write a balanced
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 2 Solutions
Physical Chemistry
Ch. 2 - Calculatethe work performed by a person whoexertsa...Ch. 2 - Explain inyour own words why work done by the...Ch. 2 - Calculate the work in joules when a piston moves...Ch. 2 - Calculatethe work on the system whena piston is...Ch. 2 - Calculatethe work in joules needed to expanda...Ch. 2 - Consider exercise 2.5. Would the workbe more or...Ch. 2 - Apistonhaving0.033 mol ofgas at 35.0Cexpands...Ch. 2 - A bottle of soda has a head space containing 25.0...Ch. 2 - Prob. 2.9ECh. 2 - Calculate the specific heat of a material if 288J...
Ch. 2 - There is 3930 J of energy added to a 79.8-g sample...Ch. 2 - If the heat capacity varies withtemperature,...Ch. 2 - Liquid hydrogen fluoride, liquid water,and liquid...Ch. 2 - A 5-mmdiameter hailstone has a terminal velocity...Ch. 2 - A7.50-gpiece of iron at 100.0C is dropped into...Ch. 2 - With reference to Joules apparatus inFigure2.6,...Ch. 2 - Prob. 2.17ECh. 2 - True or false: Althoughwork done bya free...Ch. 2 - What arethe differencesbetween an open, a closed,...Ch. 2 - The statement Energycan beneithercreatednor...Ch. 2 - Prob. 2.21ECh. 2 - What is the change in internal energy when a gas...Ch. 2 - Calculate the work for the isothermal, reversible...Ch. 2 - Calculate the work donewhen 1.000 mole of an ideal...Ch. 2 - Apistonhaving0.033 mol of gas at 35.0C expands...Ch. 2 - Prob. 2.26ECh. 2 - Indicate which state function is equal to heat, q,...Ch. 2 - The distance between downtown San Francisco and...Ch. 2 - Is temperature astate function?Defend your answer.Ch. 2 - A piston reversibly and adiabatically contracts...Ch. 2 - Calculate U when 1.00 mol of H2 goes from 1.00...Ch. 2 - Many compressed gases come in large,heavy metal...Ch. 2 - Under what conditions will U be exactly zero for a...Ch. 2 - Aballoon filled with 0.505 mole of gascontracts...Ch. 2 - A piston having 7.23 g of steam at 110 C increases...Ch. 2 - It takes 2260 J to vaporize a gram of liquid water...Ch. 2 - True or false: Any process for which H is negative...Ch. 2 - Prob. 2.38ECh. 2 - A refrigerator contains approximately 17cubic...Ch. 2 - In a constant-volume calorimeter, 35.0g of H2cools...Ch. 2 - A 2.50-mol sample of gas is compressed...Ch. 2 - A 244-g amount of coffee in an open plastic cup...Ch. 2 - Prob. 2.43ECh. 2 - Starting with equation 2.27 andthe original...Ch. 2 - Derive the fact that HpT is also zero for an ideal...Ch. 2 - Define isobaric,isochoric, isenthalpic,and...Ch. 2 - Starting from the cyclicrule involvingthe Joule-...Ch. 2 - The ideal gas law is theequation of state for an...Ch. 2 - Prob. 2.49ECh. 2 - Estimatethe final temperature of a mole of gas at...Ch. 2 - With regard to exercise 2.50, how accurate do you...Ch. 2 - Use the data in Table 2.2 to determine Hp T for Ar...Ch. 2 - Use the data in Table 2.2 to determine PH T for N2...Ch. 2 - Someone proposes thatthe Joule-Thomson coefficient...Ch. 2 - Why is equation2.37 written interms of CV and Cp...Ch. 2 - What are the numerical values of the heat...Ch. 2 - In a constant-pressure calorimeter that is, one...Ch. 2 - What is the finaltemperature of0.122 mole...Ch. 2 - Prob. 2.59ECh. 2 - Show that =5/3 for a monatomic ideal gas.Ch. 2 - Prob. 2.61ECh. 2 - Prob. 2.62ECh. 2 - A 1.00 mol sample of H2 is carefully warmed from...Ch. 2 - Asampleof a monatomic ideal gas doubles itsvolume...Ch. 2 - A sample of an ideal diatomic gas is compressed...Ch. 2 - In orbit about Earth, a weather balloonjettisons a...Ch. 2 - Prob. 2.67ECh. 2 - Prob. 2.68ECh. 2 - If pumping up an automobile tire is assumed to be...Ch. 2 - Prob. 2.70ECh. 2 - Take the volume change into account and calculate...Ch. 2 - How much work is performed by 1 mole of water...Ch. 2 - Why are steam burns so much worse than water burns...Ch. 2 - How many grams of water at 0C will be melted by...Ch. 2 - Draw a diagram like Figure 2.11 that illustrates...Ch. 2 - Determine the rxnH(25C) of the following reaction:...Ch. 2 - Determine rxnH 25 C for the following reaction: NO...Ch. 2 - The enthalpy of combustion of...Ch. 2 - The enthalpy of combustion of diamond is -395.4...Ch. 2 - Using Hesss law, writeout allof the formation...Ch. 2 - Sublimation is the phase change from solid to gas...Ch. 2 - The thermite reaction combines aluminum powder and...Ch. 2 - Benzoic acid, C6H5COOH, is a common standard used...Ch. 2 - Assume that 1.20 g of benzoicacid, C6H5COOH, is...Ch. 2 - Natural gas is mostly CH4. When it burns, the...Ch. 2 - Assuming constant heatcapacities for products and...Ch. 2 - Use the heat capacities of the products and...Ch. 2 - The following are values of heat capacity for...Ch. 2 - Prob. 2.89ECh. 2 - Prob. 2.90ECh. 2 - The Dieterici equation of state for one mole of...Ch. 2 - Prob. 2.92ECh. 2 - Find the enthalpies of the combustion reactions...
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
- The decomposition of ozone, O3, to oxygen, O2, is an exothermic reaction. What is the sign of q? If you were to touch a flask in which ozone is decomposing to oxygen, would you expect the flask to feel warm or cool?arrow_forwardThe combustion of methane can be represented as follows: a. Use the information given above to determine the value of H for the combustion of methane to form CO2(g) and 2H2O(l). b. What is Hf for an element in its standard state? Why is this? Use the figure above to support your answer. c. How does H for the reaction CO2(g) + 2H2O (1) CH4(g) + O2(g) compare to that of the combustion of methane? Why is this?arrow_forwardCoal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.arrow_forward
- Using the data in Appendix G, calculate the standard enthalpy change for each of the following reactions: (a) Si(s)+2F2(g)SiF4(g) (b) 2C(s)+2H2(g)+O2(g)CH3CO2H(l) (c) CH4(g)+N2(g)HCN(g)+NH3(g) ; (d) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)arrow_forwardConsider the Haber process: N2(g)+3H2(g)2NH3(g);H=91.8kJ The density of ammonia at 25C and 1.00 atm is 0.696 g/L. The density of nitrogen, N2, is 1.145 g/L, and the molar heat capacity is 29.12 J/(mol C). (a) How much heat is evolved in the production of 1.00 L of ammonia at 25C and 1.00 atm? (b) What percentage of this heat is required to heat the nitrogen required for this reaction (0.500 L) from 25C to 400C, the temperature at which the Haber process is run?arrow_forwardHow much will the temperature of a cup (180 g) of coffee at 95 C be reduced when a 45 g silver spoon (specific heat 0.24 J/g C) at 25 C is placed in the coffee and the two are allowed to reach the same temperature? Assume that the coffee has the same density and specific heat as water.arrow_forward
- An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?arrow_forwardOne step in the manufacturing of sulfuric acid is the conversion of SO2(g) to SO3(g). The thermochemical equation for this process is SO2(g)+12O2(g)SO3(g)H=98.9kJ The second step combines the SO3 with H2O to make H2SO4. (a) Calculate the enthalpy change that accompanies the reaction to make 1.00 kg SO3(g). (b) Is heat absorbed or released in this process?arrow_forwardA 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?arrow_forward
- 9.41 Under what conditions does the enthalpy change equal the heat of a process?arrow_forwardUsing data from Appendix 4, calculate H, S and G for the following reactions that produce acetic acid: Which reaction would you choose as a commercial method for producing acetic acid (CH3CO2H) at standard conditions? What temperature conditions would you choose for the reaction? Assume H and S do not depend on temperature.arrow_forwardWrite the balanced chemical equation for the combustion of methane, CH4(g), to give carbon dioxide and water vapor. Explain why it is difficult to predict whether S is positive or negative for this chemical reaction.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
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: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher: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: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
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
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
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