A vessel contains Ar(g) at a high pressure. Which of the following statements best helps to explain why the measured pressure is significantly greater than the pressure calculated using the ideal gas law?
1. The molar mass of Ar is relatively large.2. A significant number of Ar2 molecules form.3. The attractive forces among Ar atoms cause them to collide with the walls of the container with less force.4. The combined volume of the Ar atoms is too large to be negligible compared with the total volume of the container.

Deviations from ideality are due to intermolecular forces and to the nonzero volume of the molecules themselves. At infinite volume, the volume of the molecules themselves is negligible compared with the infinite volume the gas occupies.

However, the volume occupied by the gas molecules must be taken into account. Each molecule does occupy a finite, although small, intrinsic volume.

The non-zero volume of the molecules implies that instead of moving in a given volume V they are limited to doing so in a smaller volume. Thus, the molecules will be closer to each other and repulsive forces will dominate, resulting in greater pressure than the one calculated with the ideal gas law, that means, without considering the volume occupied by the molecules.

shrutiagrawal1798 shrutiagrawal1798 · Answer 2 · 2022-01-05T07:54:00+01:00

The pressure of Ar vessel has been high than the theoretical value, because the volume of Ar has has been large and contribute in the total volume and thereby the pressure. Thus, option D is correct.

An ideal gas has been the theoretical gas that has been composed of non interacting particles. The pressure of the ideal gas has been assumed to be responsible for the collision with the walls.

In an ideal gas, the pressure exerted by the inter particle interaction has been assumed to be negligible.

The Ar present in the vessel at high temperature has been composed of the high volume as well. Since the volume of the gas has been more, the inter-molecular interactions have been increased as well.

This results in the increased pressure of the gas, as the pressure of inter-molecular particles has not been considered negligible as in an ideal gas law.

Thus, the pressure of Ar has been high than the theoretical pressure from ideal gas law, as the volume of Ar has been large and is responsible for the increased pressure. Thus, option D is correct.

For more information about the ideal gas law, refer to the link:

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