Question

At a pressure of 1 atm, liquid helium boils at 4.20 K. The latent heat of vaporization is 20.5 kJ/kg. Determine the entropy change (per kilogram) of the helium resulting from vaporization.

Name: Problem 36, Chapter 22: Physics for Scientists and Engineers with Modern Physics
Uploaded: 2020-09-17T12:50:57-08:00
Duration: 56 s
Channel: Sheh Lit Chang
Description: At a pressure of 1 atm, liquid helium boils at 4.20 K. The latent heat of vaporization is 20.5 kJ/kg. Determine the entropy change (per kilogram) of the helium resulting from vaporization.

   At a pressure of 1 atm, liquid helium boils at 4.20 K. The latent heat of vaporization is 20.5 kJ/kg. Determine the entropy change (per kilogram) of the helium resulting from vaporization.

Physics for Scientists and Engineers with Modern Physics

Paul Tipler, Gene… 6th Edition

Chapter 22, Problem 36

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Solved by Expert Sheh Lit Chang

09/17/2020

Step 1

Step 1: The entropy change for a process can be calculated using the formula: \[ \Delta S = \frac{Q}{T} \] where \( \Delta S \) is the entropy change, \( Q \) is the heat transferred during the process, and \( T \) is the absolute temperature. Show more…

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At a pressure of 1 atm, liquid helium boils at 4.20 K. The latent heat of vaporization is 20.5 kJ/kg. Determine the entropy change (per kilogram) of the helium resulting from vaporization.

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Key Concepts

Entropy Change in Phase Transitions

This concept refers to the change in the disorder or randomness of a system when it undergoes a phase change, such as from a liquid to a gas. In a reversible phase transition, the entropy change can be calculated by dividing the latent heat by the temperature at which the phase change occurs, following the relation ?S = ?H/T. This relationship is fundamental in thermodynamics and helps in understanding how energy and disorder are interrelated during phase changes.

Latent Heat of Vaporization

Latent heat of vaporization is the energy required per unit mass to convert a substance from its liquid phase to its gaseous phase at constant temperature and pressure. This energy input does not raise the temperature but is used to overcome intermolecular forces during the phase change, making it a critical parameter in calculating changes in entropy and other thermodynamic properties during vaporization.

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