Ideal gases exhibit specific mathematical relationships among the number of particles present, temperature, pressure and volume.
In a mixture of ideal gases, the pressure exerted by each component (partial pressure) is independent of the other components. Therefore, the total pressure is the sum of the partial pressures..Graphical representtion of the relationships between P, V, and T are useful to describe gas behaviorKinetic molecular theory combined with a qualitative use of Maxwell Boltzmann distribution provides a robust model for qualitative explanations of these mathematical relationships.Some real gases exhibit ideal or near ideal behavior under typical lab conditions. Lab data can be used to generate or investigate the relationships and to estimate absolute zero on the Celsius scale.All real gases are observed to deviate from ideal behavior particularly under conditions that are close to those resulting in condensation. Except at extreme high pressures that are not typically seen in laboratory, devations from ideal behavior are the result of intermolecular attractions among gas molecules. These forces are strongly distance dependent so they are most significant during collisions.
Observed deviations from ideal gas behavior can be explained through an understanding of the structure of atoms and molecules and their intermolecular interactions.chemteam.info has a good tutorial section with gas laws problems