Variables in ideal gas law?

[September24]

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I just want to confirm something, in PV=NRT

P= pressure EXERTED BY GAS MOLECULES on surface of container...right?

V= Is this volume occupied by gas molecules or volume of container in which gas is?

Thats my main questions.

Reason I ask this is due to ideal vs real gases. If there is strong attraction, pressure decreases right (compared to ideal) since some gas will be attracted to one another resulted in less collision with wall. Likewise, if gas volume is large, volume is higher than expected for a real gas (in low volume container with high temperature).

 

[Heday]

I just want to confirm something, in PV=NRT

P= pressure EXERTED BY GAS MOLECULES on surface of container...right?

V= Is this volume occupied by gas molecules or volume of container in which gas is?

Thats my main questions.

Reason I ask this is due to ideal vs real gases. If there is strong attraction, pressure decreases right (compared to ideal) since some gas will be attracted to one another resulted in less collision with wall. Likewise, if gas volume is large, volume is higher than expected for a real gas (in low volume container with high temperature).

Yes regarding pressure. V is the volume of the container. The volume of the gas is always equal to its container.

 

[monkeyvokes]

Reason I ask this is due to ideal vs real gases. If there is strong attraction, pressure decreases right (compared to ideal) since some gas will be attracted to one another resulted in less collision with wall.

yea

Likewise, if gas volume is large, volume is higher than expected for a real gas (in low volume container with high temperature).

what

 

[keikoblue2]

Likewise, if gas volume is large, volume is higher than expected for a real gas (in low volume container with high temperature).

Volume for a real gas is smaller than the ideal volume. Volume refers to the volume of the container (the free space in it). Ideal volume ignores the volume of the gas molecules in the container. However, in a real gas, the gas molecules actually have volume and take up free space in the container, leading the volume of a real gas to be smaller than the volume of an ideal gas.

V(ideal) = V(container) - nb
b is the empirical value for each gas, and n is the number of moles.
The greater the number of gas particles 👎, the more volume the molecules occupy.
The bigger the size of the gas molecules (b), the more volume the molecules occupy.
Therefore, the volume of a real gas is always less than ideal.

 

[September24]

Okay I see now. V is volume of container. If there is gas in it, which actually DO have volume, then the volume of the gas occupies some of the space thus reducing volume.