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## Real gases do not behave according to the kinetic-molecular theory. Because particles of gases occupy space and exert attractive forces on each other, all real gases deviate to some degree from ideal gas behavior. A real gas is a gas that does not behave completely according to the assumptions o...
## Real gases do not behave according to the kinetic-molecular theory. Because particles of gases occupy space and exert attractive forces on each other, all real gases deviate to some degree from ideal gas behavior. A real gas is a gas that does not behave completely according to the assumptions of the kinetic-molecular theory. At very high pressures and low temperatures, the gas particles will be closer together, and their kinetic energy will be insufficient to completely overcome the attractive forces. At such conditions, the gas deviates from ideal behavior. At very low temperatures or very high pressures, gases condense to the liquid phase. The kinetic-molecular theory is more likely to hold true for gases whose particles have little attraction for each other. The noble gases, such as helium, He, and neon, Ne, show essentially ideal gas behavior over a wide range of temperatures and pressures. The particles of these gases are monatomic and thus nonpolar. The particles of gases such as nitrogen, N₂ and hydrogen, H₂ are nonpolar diatomic molecules. The behavior of these gases most closely approximates that of the ideal gas under certain conditions. The more polar the molecules of a gas are, the greater the attractive forces between them and the more the gas will deviate from ideal gas behavior. For example, highly polar gases, such as ammonia (NH₃) and water vapor, deviate from ideal behavior to a larger degree than nonpolar gases.
