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A sample consisting of 1.5 mol of perfect gas molecules with Cv = 20.8 J K-¹ is initially at 3.50 atm and 300 K. It undergoes reversible adiabatic expansion until its pressure reaches 2.25 atm. Calculate a) the final volume, b) temperature, and c) the work done.

A sample consisting of 1.5 mol of perfect gas molecules with Cv = 20.8 J K-¹ is initially at 3.50 atm and 300 K. It undergoes reversible adiabatic expansion until its pressure reaches 2.25 atm. Calculate a) the final volume, b) temperature, and c) the work done.

Chemistry
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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A sample consisting of 1.5 mol of perfect gas molecules with Cv = 20.8 J K-¹ is initially at 3.50 atm and 300 K. It undergoes reversible adiabatic expansion until its pressure reaches 2.25 atm. Calculate a) the final volume, b) temperature, and c) the work done.
Transcribed Image Text:A sample consisting of 1.5 mol of perfect gas molecules with Cv = 20.8 J K-¹ is initially at 3.50 atm and 300 K. It undergoes reversible adiabatic expansion until its pressure reaches 2.25 atm. Calculate a) the final volume, b) temperature, and c) the work done.
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Step 1: Given Information

Given information:

number of moles of an ideal gas, straight n equals 1.5 space mol

specific heat constant at constant volume, straight C subscript straight v space equals space 20.8 space JK to the power of negative 1 end exponent

initial pressure, straight P subscript 1 space equals space 3.50 space atm

initial temperature, straight T subscript 1 space equals space 300 space straight K

final pressure, straight P subscript 2 space equals space 2.25 space atm

The gas undergoes reversible adiabatic expansion.


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