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Give the Postulates of Kinetic Theory Of Gases.?
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The kinetic theory of gases (also known as kinetic-molecular theory) explains the behavior of a hypothetical ideal gas. According to this theory, gases are made up of tiny particles in random, straight line motion. They move rapidly and continuously and make collisions with each other and the walls. This was the first theory to describe gas pressure in terms of collisions with the walls of the container, rather than from static forces that push the molecules apart. Kinetic theory also explains how the different sizes of the particles in a gas can give them different, individual speeds.
POSTULATES
Kinetic theory makes many assumptions in order to explain the reasons gases act the way they do. According to kinetic theory:
Gases consist of particles in constant, random motion. They continue in a straight line until they collide with something—usually 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.
No molecular forces are at work. This means that there is no attraction or repulsion between the particles.
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.
Thermal Energy
Keep in mind that the temperature of a gas is actually a measure of its average kinetic energy, and kinetic energy of a particle is related to its velocity according to the following equation:
\[ KE= \frac{1}{2} mv^2\]
where KE represents kinetic energy of a particle, m equals mass, and v2 is the square of its velocity. As velocity increases so does kinetic energy. Of course the inverse is also true, that as kinetic energy increases so does velocity. You can see from this relationship how a molecule with a higher temperature will be moving faster. The temperature of the system is the average kinetic energy of its particles. Thermal energy is the total kinetic energy of all the particles in a system. Temperature, thermal energy, and the speed of a molecule are all directly related.
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POSTULATES
Kinetic theory makes many assumptions in order to explain the reasons gases act the way they do. According to kinetic theory:
Gases consist of particles in constant, random motion. They continue in a straight line until they collide with something—usually 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.
No molecular forces are at work. This means that there is no attraction or repulsion between the particles.
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.
Thermal Energy
Keep in mind that the temperature of a gas is actually a measure of its average kinetic energy, and kinetic energy of a particle is related to its velocity according to the following equation:
\[ KE= \frac{1}{2} mv^2\]
where KE represents kinetic energy of a particle, m equals mass, and v2 is the square of its velocity. As velocity increases so does kinetic energy. Of course the inverse is also true, that as kinetic energy increases so does velocity. You can see from this relationship how a molecule with a higher temperature will be moving faster. The temperature of the system is the average kinetic energy of its particles. Thermal energy is the total kinetic energy of all the particles in a system. Temperature, thermal energy, and the speed of a molecule are all directly related.
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The five main postulates of the KMT are as follows:
(1) the particles in a gas are in constant, random motion,
(2) the combined volume of the particles is negligible,
(3) the particles exert no forces on one another,
(4) any collisions between the particles are completely elastic.
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