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3.50 moles of an ideal gas is expanded from 450 K and an initial pressure of 5.00 bar to a final pressure of 1.00 bar. Cp.m = 5/2R. Calculate w for the following two cases: %3D (a) The expansion is isothermal and reversible. (b) The expansion is adiabatic and reversible. (c) Without resorting to equations, explain why the result to part b) is greater than (or less than) the result to part a).

3.50 moles of an ideal gas is expanded from 450 K and an initial pressure of 5.00 bar to a final pressure of 1.00 bar. Cp.m = 5/2R. Calculate w for the following two cases: %3D (a) The expansion is isothermal and reversible. (b) The expansion is adiabatic and reversible. (c) 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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Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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2. 3.50 moles of an ideal gas is expanded from 450 K and an initial pressure of 5.00 bar to a final pressure of 1.00 bar. Cp,m = 5/2R. Calculate w for the following two cases: (a) The expansion is isothermal and reversible. (b) The expansion is adiabatic and reversible. (c) Without resorting to equations, explain why the result to part b) is greater than (or less than) the result to part a).
Transcribed Image Text:2. 3.50 moles of an ideal gas is expanded from 450 K and an initial pressure of 5.00 bar to a final pressure of 1.00 bar. Cp,m = 5/2R. Calculate w for the following two cases: (a) The expansion is isothermal and reversible. (b) The expansion is adiabatic and reversible. (c) 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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