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MaxineIn a private relationship for non-ideal gases, the behavior of gases is described by the Van der Waals equation, which accounts for the volume occupied by gas molecules and intermolecular forces. This equation provides a more accurate prediction of gas behavior at high pressures and low temperatures compared to the ideal gas law.
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What is meant by the term 'ideal gas'?
An ideal gas is a theoretical gas composed of a set of randomly-moving, non-interacting point particles. The ideal gas concept is useful because it obeys the ideal gas law. At normal conditions such as standard temperature and pressure, most real gases behave qualitatively like an ideal gas. Many gases such as air, nitrogen, oxygen, hydrogen, noble gases, and some heavier gases like carbon dioxide can be treated like ideal gases within reasonable tolerances.
How does an ideal gas diff from a real gas?
An ideal gas follows the ideal gas law exactly, while a real gas may deviate from the ideal gas law at high pressures and low temperatures due to intermolecular forces and molecular volume. Real gases have non-zero molecular volume and experience intermolecular interactions, while ideal gases are assumed to have no volume and no intermolecular forces.
What are two types of non-ideal solutions?
Two types of non-ideal solutions are ideal mixtures and non-ideal mixtures. Ideal mixtures follow Raoult's Law, where the vapor pressure of each component is directly proportional to its mole fraction in the solution. Non-ideal mixtures do not obey Raoult's Law due to interactions between the components, such as deviations from ideal behavior or the formation of new chemical species.
How can a real gas be made to approach being an ideal gas?
A real gas can approach being an ideal gas by decreasing its pressure and increasing its temperature. At low pressures or high temperatures, the interactions between gas molecules become less significant, causing the gas to behave more like an ideal gas. Additionally, using larger volumes can also help minimize intermolecular interactions and make a real gas behave more like an ideal gas.
What characteristics do real gases have that contradict the assumptions of kinetic-molecular theory?
Real gases have non-zero volume and experience intermolecular forces, which contradict the assumptions of kinetic-molecular theory that gases consist of point particles with no volume and that there are no intermolecular forces present. Real gases also deviate from ideal behavior at high pressures and low temperatures, which is not accounted for in the kinetic-molecular theory.
