Con base en sus respectivas constantes de van der Waals...

Con base en sus respectivas constantes de van der Waals (Tabla 10.3), ¿cuál gas, Ar o $\mathrm{CO}_2$, cabe esperar que se comporte de forma más parecida a un gas ideal a presiones altas? Explique.

Key Concepts

Ideal Gas Behavior

The ideal gas law assumes no interactions between gas molecules and that the volume occupied by the molecules themselves is negligible compared to the container volume. At high pressures, however, these assumptions break down because the molecules are forced closer together, making intermolecular forces and molecular sizes significant factors. A gas that behaves ideally will exhibit minimal deviations from these assumptions even under higher pressures.

van der Waals Equation

The van der Waals equation introduces correction factors to the ideal gas law to account for intermolecular attractions and the finite volume of molecules. The constants 'a' and 'b' in the equation quantify these deviations: 'a' corrects for the attractive forces between molecules, while 'b' corrects for the molecular volume. Gases with smaller 'a' and 'b' values will exhibit behavior closer to that predicted by the ideal gas law, especially at high pressures.

Intermolecular Forces and Molecular Size

The magnitude of the van der Waals constants reflects the strength of intermolecular forces and the effective size of the molecules. In comparing gases, a gas with lower values of these constants experiences less deviation from ideality because the attractive forces and the impact of molecular volume are less pronounced. Thus, when choosing between gases, the one with smaller van der Waals constants is expected to behave more like an ideal gas under high-pressure conditions.

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