Isotherms of real gases and their comparison with Van der Waals isotherms
Understand the Problem
The question is asking for a comparison between isotherms of real gases and the isotherms derived from the Van der Waals equation. It requires an understanding of the behavior of real gases under various conditions and how these behaviors are modeled compared to an idealized framework.
Answer
Van der Waals isotherms provide a good approximation for real gases by including molecular volume and interactions, accurately predicting phase transitions.
Van der Waals isotherms are approximations for real gases improving upon ideal gas behavior by including molecule volume and intermolecular forces. Real gas isotherms show deviations, especially near critical points, while Van der Waals isotherms predict phase transitions and critical phenomena reasonably well.
Answer for screen readers
Van der Waals isotherms are approximations for real gases improving upon ideal gas behavior by including molecule volume and intermolecular forces. Real gas isotherms show deviations, especially near critical points, while Van der Waals isotherms predict phase transitions and critical phenomena reasonably well.
More Information
Van der Waals isotherms account for the volume occupied by gas molecules and attractions between them, unlike the ideal gas law. These modifications allow for more accurate predictions of real gas behaviors, especially near the critical state where ideal gas laws fail.
Tips
A common mistake is treating van der Waals isotherms as exact for all real gas conditions without considering that they still have limitations, particularly at very high pressures or temperatures far below critical points.
Sources
- Van der Waals Isotherms for Real and Ideal Gases - demonstrations.wolfram.com
- 2.5: Condensation of Gases and the Critical State - chem.libretexts.org
- Van der Waals Equation - Derivation, Relation Between Ideal Gas ... - byjus.com
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