The pressure of a sample of helium gas is directly proportional to the Kelvin temperature if the volume is forced to remain constant. (Imagine the gas sample trapped in a rigid steel cylinder, as is true for the gases in a lab setting.)   How can we explain, using kinetic molecular theory, why the pressure increases when the temperature increases? ("Using kinetic-molecular theory" means describing what the atoms of He are doing. It may help to consider the general definition of pressure.)

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Chapter4: Introduction To Gases
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The pressure of a sample of helium gas is directly proportional to the Kelvin temperature if the volume is forced to remain constant. (Imagine the gas sample trapped in a rigid steel cylinder, as is true for the gases in a lab setting.)

 

How can we explain, using kinetic molecular theory, why the pressure increases when the temperature increases? ("Using kinetic-molecular theory" means describing what the atoms of He are doing. It may help to consider the general definition of pressure.)

 

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