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Question
Under which one of the following conditions do real gases approach the ideal gas behaviour?
Under which one of the following conditions do real gases approach the ideal gas behaviour?
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Solution
The correct option is C High temperature and low pressure
The equation for an ideal gas is PV=nRT.
Ideal gas behaviour can be explained with the following assumptions:
1. Negligible attractive forces operate between the gas molecules.
2. The volume occupied by the gas molecules is negligible compared to that occupied by the gas.
3. The gas molecules 'bounce' off the walls of the container in which they are contained with no loss of energy.
4. The gas molecules are in continuous, rapid, random and linear motion.
With reference to point 1, in order for a gas to approach (though realistically this is impossible) idealize by having negligible attractive forces to operate between its molecules, the molecules have to somehow be arranged far apart to prevent the attraction from being significant. This means that low pressure is needed to keep the gas molecules somewhat "scattered".
Secondly, the high temperature is needed for the same reason for overcoming the attraction between gas molecules.
Hence, the correct option is C
The equation for an ideal gas is PV=nRT.
Ideal gas behaviour can be explained with the following assumptions:
1. Negligible attractive forces operate between the gas molecules.
2. The volume occupied by the gas molecules is negligible compared to that occupied by the gas.
3. The gas molecules 'bounce' off the walls of the container in which they are contained with no loss of energy.
4. The gas molecules are in continuous, rapid, random and linear motion.
With reference to point 1, in order for a gas to approach (though realistically this is impossible) idealize by having negligible attractive forces to operate between its molecules, the molecules have to somehow be arranged far apart to prevent the attraction from being significant. This means that low pressure is needed to keep the gas molecules somewhat "scattered".
Secondly, the high temperature is needed for the same reason for overcoming the attraction between gas molecules.
1. Negligible attractive forces operate between the gas molecules.
2. The volume occupied by the gas molecules is negligible compared to that occupied by the gas.
3. The gas molecules 'bounce' off the walls of the container in which they are contained with no loss of energy.
4. The gas molecules are in continuous, rapid, random and linear motion.
With reference to point 1, in order for a gas to approach (though realistically this is impossible) idealize by having negligible attractive forces to operate between its molecules, the molecules have to somehow be arranged far apart to prevent the attraction from being significant. This means that low pressure is needed to keep the gas molecules somewhat "scattered".
Secondly, the high temperature is needed for the same reason for overcoming the attraction between gas molecules.
Hence, the correct option is C
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