Pressure of a gas - quick question.

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The pressure of a gas, at constant temperature, does not depend on the container's surface area or volume, as clarified in the discussion. The ideal gas law does not factor in surface area because the behavior of gas particles is not influenced by proximity to surfaces. While larger surface areas may lead to more collisions, the collisions per unit of surface area remain constant, maintaining consistent pressure. The conversation highlights the geometric reasoning behind these principles. Understanding these concepts clarifies the relationship between gas pressure and container dimensions.
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pressure of a gas -- quick question.

Does the pressure of a gas (assuming temperature is constant) depend on the container's surface area as well as its volume? And if so why isn't this factored into the ideal gas law?
 
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No, it does not.
 


Wouldn't the surface area be directly correlated with the volume?
 


The state of the particles is not assumed to be affected by proximity to any surface in the ideal gas law.
 


drakkith - Well sure. But I was thinking of how identical volumes can have different surface areas.

Thanks for the responses. I get it now. Even though more collisions will be happening in a volume with a larger surface area, the collisions per unit of surface area will remain constant (and thus so will pressure). Geometrically it makes sense.
 

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