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For real gases Cp = Cv at
- a)critical temperature
- b)triple point
- c)all temperature
- d)absolute zero temperatur
Correct answer is option 'D'. Can you explain this answer?
Most Upvoted Answer
For real gases Cp = Cv ata)critical temperatureb)triple pointc)all tem...
Explanation:
Real Gases and Specific Heats:
Real gases deviate from ideal behavior under certain conditions, such as high pressure or low temperature. In these cases, the specific heat at constant pressure (Cp) and specific heat at constant volume (Cv) are no longer equal.
Cp and Cv at Absolute Zero Temperature:
At absolute zero temperature, the molecules of a gas have minimum kinetic energy and are at rest. This means that there is no translational, rotational, or vibrational motion in the gas molecules. At this point, the internal energy of the gas is solely due to the potential energy of the molecules.
Cp and Cv at Absolute Zero:
- At absolute zero temperature, the specific heat at constant pressure (Cp) and specific heat at constant volume (Cv) of a gas approach the same value.
- This is because there is no energy associated with motion at absolute zero, and all the energy is in the form of potential energy.
- The difference between Cp and Cv arises from the energy associated with motion, which is negligible at absolute zero temperature.
Conclusion:
Therefore, at absolute zero temperature, the specific heat at constant pressure (Cp) equals the specific heat at constant volume (Cv) for real gases. This is because there is no thermal motion present at absolute zero, leading to the equality of Cp and Cv.
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