Kinetic Theory of Gases Little help please

In summary, the conversation discusses the application of the kinetic theory of gases in solving a problem involving a massless cylinder divided into two sections containing nitrogen and oxygen. The pressure of the nitrogen is twice that of the oxygen, and the question is how far the cylinder will move when the membrane separating the sections is removed. The conversation also touches on the concept of relative molecular densities and the difference in molecular masses between N2 and O2.
  • #1
Seiya
43
1
Kinetic Theory of Gases... Little help please :)

Hey, i didnt seem to have trouble with any other questions except this one... all i could figure out is that i somehow must use the kinetic theory of gases?
A massless cylinder 34 cm long rests on a horizontal frictionless table. The cylinder is divided into two equal sections by a membrane. One section contains nitrogen and the other contains oxygen. The pressure of the nitrogen is twice that of the oxygen. How far will the cylinder move if the membrane is removed?
I tried setting 2pv= 2N(1/2mvx^2)av and divide it by pv= 2N(1/2mvx^2)
well i don't really know any advice appreciated :|
 
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  • #2
Where is the center of mass before the membrane is removed and then after?

At the same temperature and same volume, what are the relative molecular densities of N2 and O2. Think PV=nRT.

Note also the difference in molecular masses.
 
  • #3
Got it, thanks
 
Last edited:

1. What is the Kinetic Theory of Gases?

The Kinetic Theory of Gases is a scientific model that explains the behavior and properties of gases. It states that gases are composed of a large number of particles that are in constant random motion, and that the pressure, volume, and temperature of a gas are directly related to the average kinetic energy of its particles.

2. How does temperature affect the Kinetic Theory of Gases?

According to the Kinetic Theory of Gases, as the temperature of a gas increases, the average kinetic energy of its particles also increases. This leads to an increase in the speed of the particles and a corresponding increase in the pressure and volume of the gas. As the temperature decreases, the average kinetic energy and speed of the particles also decrease, resulting in a decrease in pressure and volume.

3. What is the relationship between pressure and volume in the Kinetic Theory of Gases?

The Kinetic Theory of Gases states that there is an inverse relationship between pressure and volume. This means that as the volume of a gas decreases, the pressure increases and vice versa. This can be explained by the fact that as the volume decreases, the particles of the gas have less space to move around, leading to more frequent collisions with the walls of the container and an increase in pressure.

4. What is the significance of the Boltzmann constant in the Kinetic Theory of Gases?

The Boltzmann constant is a fundamental constant in the Kinetic Theory of Gases that relates the average kinetic energy of gas particles to the temperature of the gas. It is denoted by the symbol "k" and has a value of 1.38 x 10^-23 Joules per Kelvin. It allows scientists to accurately calculate the average kinetic energy of gas particles at a given temperature, which is essential in understanding the behavior of gases.

5. How does the Kinetic Theory of Gases explain the properties of an ideal gas?

The Kinetic Theory of Gases provides a theoretical basis for understanding the properties of an ideal gas. According to this theory, an ideal gas is composed of a large number of particles that have negligible volume and do not interact with each other. This explains why an ideal gas follows the gas laws, such as Boyle's law and Charles's law, which are based on the assumptions of the Kinetic Theory of Gases.

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