Kinetic theory and gas molecules

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The kinetic theory explains that gas molecules move rapidly and collide with each other and container walls, exerting significant force due to their small area. Despite this, gas molecules do not escape or drill holes in the container because their mass is relatively low, and the area they occupy is minimal compared to their force. Pressure, defined as force per area, is a macroscopic concept that does not effectively describe atomic-level interactions. The discrepancy arises from the scaling differences between area and mass, with area increasing with the square of length and mass with the cube. Understanding these principles clarifies why gas behavior does not align with initial expectations of high pressure leading to escape.
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The kinetic theory states that the gas molecules are randomly colliding with each other and with the wall of the container with high speed.The area of each molecule is very less and as they are moving with high speed,they exert great force. since the pressure is force/area , the pressure should be very high and each gas molecules should be able to drill holes and escape.
But this doesn't happen.Why?
 
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adjacent said:
The area of each molecule is very less ...
Their mass is much more less. Area scales with length2, mass with length3.

since the pressure is force/area
Pressure is a macroscopic concept, which is not useful for atomic level interactions.
 

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