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For monotomic molecules, the avg kinetic energy is 3/2 k_b T

for diatomic, it is 5/2 k_b T

PV = n_particles * k_b T

Why is there no factor of 3/2 or 5/2 in the ideal gas law? How is it factored out?

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- Thread starter vjk2
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- #1

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For monotomic molecules, the avg kinetic energy is 3/2 k_b T

for diatomic, it is 5/2 k_b T

PV = n_particles * k_b T

Why is there no factor of 3/2 or 5/2 in the ideal gas law? How is it factored out?

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- #2

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pressure * total volume is not equal to total energy.

energy density * total volume is equal to total energy.

Kinetic energy is the energy that an object possesses due to its motion. In the context of the ideal gas law, it refers to the energy that gas molecules possess due to their random movement.

Kinetic energy is directly related to the temperature of a gas. As the temperature increases, the average kinetic energy of the gas molecules also increases, resulting in faster movement and increased pressure.

Yes, the ideal gas law can be used to calculate the kinetic energy of a gas by rearranging the equation to solve for kinetic energy. The formula for kinetic energy is KE = 3/2 * nRT, where n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

The ideal gas law, PV=nRT, shows that as temperature increases, the pressure and volume of a gas also increase. This is because an increase in temperature leads to an increase in the average kinetic energy of the gas molecules, which results in more frequent and harder collisions with the walls of the container, leading to an increase in pressure.

No, other factors such as volume, pressure, and number of particles also play a role in determining the behavior of an ideal gas. The ideal gas law takes into account all of these factors to describe the relationship between them and the behavior of a gas.

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