A real gas behaves like an ideal gas if its
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As per the kinetic theory of gases, the real gas deviates from the ideal gas but they behave the same in some particular temperature and pressure conditions.
- pressure and temperature are both high
- pressure and temperature are both low
- pressure is high and temperature is low
- pressure is low and temperature is high
The Correct Option is D
Solution and Explanation
A real gas behaves like an ideal gas at low pressure and high temperature.
As per the kinetic theory of gases, there are two main assumptions made explaining the deviation of real gases from ideal gas behavior:
1. Compared to the volume of the vessel, the volume of the gas particle is negligible. But, in the case of a real gas, the volume of every individual gas particle is very significant.
2. There is no interaction between the gaseous particles. However, in a real gas, there are forces of attraction between the molecules.
From the ideal gas equation we know, PV=nRT. Thus, if the pressure of the gas is very high, or the temperature is very low, there is a substantial deviation from the ideal gas equation. Thus, a real gas obtains ideal gas behavior at very low pressure and high temperature.
Also Read: Behavior of Gas Molecules
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Concepts Used:
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Postulates of Kinetic Theory of Gases:
- Gases consist of particles in constant, random motion. They continue in a straight line until they collide with each other or the walls of their container.
- Particles are point masses with no volume. The particles are so small compared to the space between them, that we do not consider their size in ideal gases.
- Gas pressure is due to the molecules colliding with the walls of the container. All of these collisions are perfectly elastic, meaning that there is no change in energy of either the particles or the wall upon collision. No energy is lost or gained from collisions. The time it takes to collide is negligible compared with the time between collisions.
- The kinetic energy of a gas is a measure of its Kelvin temperature. Individual gas molecules have different speeds, but the temperature and
kinetic energy of the gas refer to the average of these speeds. - The average kinetic energy of a gas particle is directly proportional to the temperature. An increase in temperature increases the speed in which the gas molecules move.
- All gases at a given temperature have the same average kinetic energy.
- Lighter gas molecules move faster than heavier molecules.
