Kinetic Molecular Theory of Gases

In summary, the conversation discusses the concept of gas particles of different masses having the same average kinetic energy at a specific temperature. The question is raised whether this is due to momentum, and it is explained that each particle is given a certain amount of energy which determines their velocity. The concept of temperature is also linked to kinetic energy and heat transfer is mentioned. The speaker also mentions the possible involvement of statistical mechanics in this concept.
  • #1
Bashyboy
1,421
5
Hello,

So, I am reading this theory, and I come across this sentence explaining to me that gas particles of different mass have the same average kinetic energy at a particular temperature. Is this somehow due to momentum? Each particle is given a certain energy which will cause them to move at a certain velocity, and, since they have different masses, the energy they receive will cause them to move at a certain velocity that is relative to their mass? If this isn't a correct way of thinking, please explain to me why particles of different masses can have the same average kinetic energy.

Thank you.
 
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  • #2
Because it is the kinetic energy that determines the temperature. I think that particles with higher kinetic energy, on average, is more likely to transfer their energy to particles with lower kinetic energy. Therefore, temperature is the representation of this, since heat flows from higher temperature to lower temperature. (I think it has something to do with statistical mechanics which I haven't learned any)

Since K.E is the same, different mass would have different velocity.
 

1. What is the Kinetic Molecular Theory of Gases?

The Kinetic Molecular Theory of Gases is a scientific model that explains the behavior of gases based on the movement of their individual particles. It states that gas particles are in constant, random motion and do not interact with each other except during collisions.

2. What are the main assumptions of the Kinetic Molecular Theory of Gases?

The main assumptions of the Kinetic Molecular Theory of Gases are that gas particles are in constant motion, have negligible volume compared to the container they are in, and do not exert any attractive or repulsive forces on each other. It also assumes that gas particles have elastic collisions and that the average kinetic energy of the particles is directly proportional to the temperature of the gas.

3. How does the Kinetic Molecular Theory of Gases explain the properties of gases?

The Kinetic Molecular Theory of Gases explains the properties of gases by describing how the movement of gas particles affects those properties. For example, the high compressibility of gases is due to the large spaces between particles, and the expansion of gases when heated is a result of the increased motion of particles.

4. What is the significance of the Kinetic Molecular Theory of Gases?

The Kinetic Molecular Theory of Gases is significant because it provides a theoretical framework for understanding and predicting the behavior of gases. It has been validated by numerous experiments and is used in many fields of science, such as chemistry, physics, and atmospheric science.

5. Are there any limitations to the Kinetic Molecular Theory of Gases?

Yes, there are some limitations to the Kinetic Molecular Theory of Gases. It does not take into account the volume of gas particles, so it is only accurate for gases at low pressures and high temperatures. It also does not account for intermolecular forces, which can affect the behavior of gases at high pressures and low temperatures.

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