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Exactly one mole of a monatomic ideal gas (C,=R) undergoes isothermal expansion from 24.4 L to 34.4 Lagainst a constant external pressure of 1.00 bar at 298 K. Calculate the change in entropy of the system and the change in entropy of the surroundings. Assume that the temperature of the surroundings is 298 K.

Exactly one mole of a monatomic ideal gas (C,=R) undergoes isothermal expansion from 24.4 L to 34.4 Lagainst a constant external pressure of 1.00 bar at 298 K. Calculate the change in entropy of the system and the change in entropy of the surroundings. Assume that the temperature of the surroundings is 298 K.

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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Exactly one mole of a monatomic ideal gas (C,=R) undergoes isothermal expansion from 24.4 L to 34.4 L'against a constant external pressure of 1.00 bar at 298 K. Calculate the change in entropy of the system and the change in entropy of the surroundings. Assume that the temperature of the surroundings is 298 K.
Transcribed Image Text:Exactly one mole of a monatomic ideal gas (C,=R) undergoes isothermal expansion from 24.4 L to 34.4 L'against a constant external pressure of 1.00 bar at 298 K. Calculate the change in entropy of the system and the change in entropy of the surroundings. Assume that the temperature of the surroundings is 298 K.
Expert Solution
Step 1

For the isothermal process, the change in entropy can be calculated by using following equation: 

delta S = nRln(V2/V1)      .............(1) 

where delta S denotes change in entropy

      n is number of moles

      R is gas constant = 8.314 J/K.mol

      V2 is the final volume and 

      V1 is the initial volume 

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