Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 2, Problem 2.2CP
Two ideal gas systems undergo reversible expansion under different conditions starting from the same P and V. At the end of the expansion, the two systems have the same volume. The pressure in the system that has undergone adiabatic expansion is lower than in the system that has undergone isothermal expansion. Explain this result without using equations.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 2 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
Ch. 2 - Electrical current is passed through a resistor...Ch. 2 - Two ideal gas systems undergo reversible expansion...Ch. 2 - You have a liquid and its gaseous form in...Ch. 2 - Prob. 2.4CPCh. 2 - For a constant pressure process, H=qp. Does it...Ch. 2 - A cup of water at 278 K (the system) is placed in...Ch. 2 - In the experiments shown in Figure 2.4a and 2.4b,...Ch. 2 - What is wrong with the following statement? Burns...Ch. 2 - Why is it incorrect to speak of the heat or work...Ch. 2 - You have a liquid and its gaseous form in...
Ch. 2 - Prob. 2.11CPCh. 2 - Explain how a mass of water in the surroundings...Ch. 2 - A chemical reaction occurs in a constant volume...Ch. 2 - Explain the relationship between the terms exact...Ch. 2 - In the experiment shown in Figure 2.4b, the weight...Ch. 2 - Discuss the following statement: If the...Ch. 2 - Discuss the following statement: Heating an object...Ch. 2 - An ideal gas is expanded reversibly and...Ch. 2 - An ideal gas is expanded reversibly and...Ch. 2 - An ideal gas is expanded adiabatically into a...Ch. 2 - Prob. 2.21CPCh. 2 - Prob. 2.22CPCh. 2 - A student gets up from her chair and pushes a...Ch. 2 - Explain why ethene has a higher value for CV,m at...Ch. 2 - Prob. 2.25CPCh. 2 - Prob. 2.26CPCh. 2 - A 3.75 mole sample of an ideal gas with Cv,m=3R/2...Ch. 2 - The temperature of 1.75 moles of an ideal gas...Ch. 2 - A 2.50 mole sample of an ideal gas, for which...Ch. 2 - A hiker caught in a thunderstorm loses heat when...Ch. 2 - Count Rumford observed that using cannon boring...Ch. 2 - A 1.50 mole sample of an ideal gas at 28.5C...Ch. 2 - Calculate q, w, U, and H if 2.25 mol of an ideal...Ch. 2 - Calculate w for the adiabatic expansion of 2.50...Ch. 2 - Prob. 2.9NPCh. 2 - A muscle fiber contracts by 3.5 cm and in doing so...Ch. 2 - A cylindrical vessel with rigid adiabatic walls is...Ch. 2 - In the reversible adiabatic expansion of 1.75 mol...Ch. 2 - A system consisting of 82.5 g of liquid water at...Ch. 2 - A 1.25 mole sample of an ideal gas is expanded...Ch. 2 - A bottle at 325 K contains an ideal gas at a...Ch. 2 - A 2.25 mole sample of an ideal gas with Cv,m=3R/2...Ch. 2 - Prob. 2.17NPCh. 2 - An ideal gas undergoes an expansion from the...Ch. 2 - An ideal gas described by Ti=275K,Pi=1.10bar, and...Ch. 2 - In an adiabatic compression of one mole of an...Ch. 2 - The heat capacity of solid lead oxide is given by...Ch. 2 - Prob. 2.22NPCh. 2 - Prob. 2.23NPCh. 2 - Prob. 2.24NPCh. 2 - Prob. 2.25NPCh. 2 - A 2.50 mol sample of an ideal gas for which...Ch. 2 - A 2.35 mole sample of an ideal gas, for which...Ch. 2 - Prob. 2.28NPCh. 2 - A nearly flat bicycle tire becomes noticeably...Ch. 2 - Prob. 2.30NPCh. 2 - Prob. 2.31NPCh. 2 - Consider the isothermal expansion of 2.35 mol of...Ch. 2 - An automobile tire contains air at 225103Pa at...Ch. 2 - One mole of an ideal gas is subjected to the...Ch. 2 - Prob. 2.35NPCh. 2 - A pellet of Zn of mass 31.2 g is dropped into a...Ch. 2 - Calculate H and U for the transformation of 2.50...Ch. 2 - A 1.75 mole sample of an ideal gas for which...Ch. 2 - Prob. 2.39NPCh. 2 - Prob. 2.40NPCh. 2 - The Youngs modulus (see Problem P2.40) of muscle...Ch. 2 - DNA can be modeled as an elastic rod that can be...Ch. 2 - Prob. 2.43NPCh. 2 - Prob. 2.44NP
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 sample of an ideal diatomic gas is compressed adiabatically and reversibly to double its initial pressure. By what percentage does its absolute temperature change in a the low-temperature limit and b the high-temperature limit?arrow_forward9.11 Analyze the units of the quantity (pressurevolume) and show that they are energy units, consistent with the idea of PV-work.arrow_forwardThe statement Energycan beneithercreatednor destroyedis sometimes used as an equivalent statement of the first law of thermodynamics. There areinaccuracies to the statement, however. Restate it tomake it less inaccurate.arrow_forward
- Starting with equation 2.27 andthe original definitionof enthalpy, derive the fact that Cp-=Cv-+Rarrow_forwardExplain why absolute enthalpies and energies cannot be measured, and only changes can be determined.arrow_forwardConsider 2.00 moles of an ideal gas that are taken from state A (PA = 2.00 atm, vA = 10.0 L) to state B (PB = 1.00 attn, VB = 30.0 L) by two different pathways: These pathways are summarized on the following graph of P versus V: Calculate the work (in units of J) associated with the two pathways. Is work a state function? Explain.arrow_forward
- A refrigerator is the reverse of an engine: Work is performed to remove heat from a system, making it colder. The efficiency of a refrigerator often termed the coefficient of performance is defined as q3/wcycle=Tlow/(ThighTlow). Use this definition to determine the efficiency needed to halve the absolute temperature. What does your answer imply about attempts to reach absolute zero?arrow_forward6.10. Use Hess’s law to prove that .arrow_forwardDefine the following terms: potential energy, kinetic energy, path-dependent function, state function, system, surroundings.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY