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The temperature of 5.85 moles of a monatomic gas decreases from T1 to T2 during a reversible isovolumetric process. It then undergoes a reversible adiabatic compression until its temperature increases to the original value of T1, while its volume decreases to 1/6 its original volume. What is the total change in entropy? The molar specific heat of the gas at constant volume is 12.5 J/(mol · K). (Assume gamma = 5/3.)

The temperature of 5.85 moles of a monatomic gas decreases from T1 to T2 during a reversible isovolumetric process. It then undergoes a reversible adiabatic compression until its temperature increases to the original value of T1, while its volume decreases to 1/6 its original volume. What is the total change in entropy? The molar specific heat of the gas at constant volume is 12.5 J/(mol · K). (Assume gamma = 5/3.)

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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The temperature of 5.85 moles of a monatomic gas decreases from T1 to T2 during a reversible isovolumetric process. It then undergoes a reversible adiabatic compression until its temperature increases to the original value of T1, while its volume decreases to 1/6 its original volume. What is the total change in entropy? The molar specific heat of the gas at constant volume is 12.5 J/(mol · K). (Assume gamma = 5/3.)

Expert Solution
Step 1

Given that,

 Number of moles, n=5.85 moles

Molar specific heat (Cv) = 12.5 J/mol.k

γ = 5/3V=16v∘

 

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