what are the main reason for which real gases deviate from Ideal behaviour
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Explanation:
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Gases deviate from the ideal gas behaviour because their molecules have forces of attraction between them.Assumptions of kinetic theory of gases : 1). The volume occupied by gas molecules is negligibly small as compared to the volume occupied by the gas.The first assumption is valid only at low pressures and high temperature, when the volume occupied by the gas molecules is negligible as compared to the total volume of the gas. But at low temperature or at high pressure, the molecules being in compressible the volumes of molecules are no more negligible as compared to the total volume of the gas. 2).The forces of attraction between gas molecules are negligible.The second assumption is not valid when the pressure is high and temperature is low. But at high pressure or low temperature when the total volume of gas is small, the forces of attraction become appreciable and cannot be ignored.
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Explanation:
Gases deviate from the ideal gas behaviour because their molecules have forces of attraction between them. Assumptions of kinetic theory of gases : 1). The volume occupied by gas molecules is negligibly small as compared to the volume occupied by the gas.
An ideal gas is a gas that follows the assumptions of the Kinetic Molecular Theory of Gases (KMT). Real gases deviate from ideal behavior because 1) they have intermolecular forces between molecules, 2) collisions aren't always elastic (also due to intermolecular forces), and 3) gas molecules have volume.
For gases such as hydrogen, oxygen, nitrogen, helium, or neon, deviations from the ideal gas law are less than 0.1 percent at room temperature and atmospheric pressure. Other gases, such as carbon dioxide or ammonia, have stronger intermolecular forces and consequently greater deviation from ideality.