Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
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Textbook Question
Chapter 2, Problem 2.14NP
A 1.25 mole sample of an ideal gas is expanded from 320. K and an initial pressure of 3.10 bar to a final pressure of 1.00 bar, and
- The expansion is isothermal and reversible.
- The expansion is adiabatic and reversible.
Without resorting to equations, explain why the result to part (b) is greater than or less than the result to part (a).
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A 0.357 mol sample of N, (g), initially at 298 K and 1.00 atm, is held at constant pressure while enough heat is applied to
raise the temperature of the gas by 12.3 K. Calculate the amount of heat q required to bring about this temperature change,
and find the corresponding total change in the internal energy AU of the gas.
Assume that the constant-pressure molar specific heat for N,(g), which consists of linear molecules, is equal to 7 R/2, where
R = 8.3145 J/(mol·K) is the ideal gas constant.
q =
AU =
} TOOLS
x10
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Chapter 2 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
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