If the ideal gas law is re-expressed in terms of temperature,
When considering the kinetic theory as applied to an ideal gas (see Jeans [19]), any of the associated results are inherently linked to the conditions which gave rise to the ideal gas law. For instance, 1) a large number of rapidly moving particles must be considered, 2) these must be negligibly small relative to the total volume, 3) all collisions must be elastic, 4) no net forces must exist between the particles, 5) the walls of the enclosure must be rigid, 6) the only force or change in momentum with time, dp/dt, which is experienced to define pressure, P, must occur at the walls, and 7) the sum of forces everywhere else must be zero.
Yet, the results relative to the ideal gas law were critically dependent on the presence of this enclosure.
Additionally, a gravitationally collapsing gaseous cloud, which obeys the ideal gas law, violates the 2nd law of thermodynamics.
Prior to experimentation, I spend 15-25 minutes probing and questioning students with the intent of drawing out prior understanding of the Ideal
Gas Law, with the goal of having the students determine how to measure the molar mass of an unknown gas on their own, with the guidance of directed teacher questioning.
Assuming that the ideal gas laws apply (an assumption which is not in fact justified), then the volume [V.sub.2] of 1 mol of gas under HIPing conditions can be obtained from:
Despite the fact that this calculation requires an assumption that the ideal gas laws do in fact apply, when the result shows that strictly they cannot, it does illustrate that the atomic spacing in the HIPing gas is much closer to that of a solid or liquid than to that of a gas at stp (Atkinson & Rickinson, 1991; Vogel & Ratke, 1991).
Assuming that the ideal gas laws apply, we can calculate:
The ideal gas law can be viewed as arising from the kinetic pressure of gas molecules colliding with the walls of a container in accordance with Newton's laws.