ideal gas

[nartnad]

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How do actual volume and predicted volume of a gas compare at:
1)moderately high pressure?
2)Extremely high pressure?
3)very low temp?

Answer:
1) less than predicted
2) more than predicted
3) less than predicted

Can someone explain each scenario? Thanks

 

[mermaid66]

So thats what i think,
ideal gas obey the PV=nRT formula, and in ordet to have a gar behave ideally, you have to have high Tempreture and Low pressure, so you can get the V. any situation othet than that lead an unusuall behaviour of ideal gas.
So when you have high T and Low P, you can predict the gas behaviour, other than that it would be in Low T less than predicted and in high P more than predicted.
Thats what I think, hope it helps.👍

 

[americanpierg]

So thats what i think,
ideal gas obey the PV=nRT formula, and in ordet to have a gar behave ideally, you have to have high Tempreture and Low pressure, so you can get the V. any situation othet than that lead an unusuall behaviour of ideal gas.
So when you have high T and Low P, you can predict the gas behaviour, other than that it would be in Low T less than predicted and in high P more than predicted.
Thats what I think, hope it helps.👍

doesnt explain A and B, and high p is actually less volume than predicted, unless its really high p

at high pressure, intermolecular forces are great enough to come into play, and the volume is smaller than expected

at extremely high temperatures, the size of the molecules become significant in comparision to the space between molecules, so volume is larger

at low temperatures, intermolecular forces become become great enough to come into play also, so volume is smaller than expected

 

[nze82]

How do actual volume and predicted volume of a gas compare at:
1)moderately high pressure?
At moderately high pressure, gas particles get closer to one another. Thus, the Van der Waals force between them becomes stronger. As a result, the volume would be smaller than what's predicted under standard conditions.
2)Extremely high pressure?
At extremely high pressure, gas particles get way too close. Thus, the volume of each particle becomes significant compared to the distance between particles (Recall that for ideal gasses you can essentially ignore the volume of each particle compared to the distance between them). When the volume of each particle become significant, you can no longer ignore it. As a result, the total volume will be greater than what's predicted under standard conditions.
3)very low temp?
At low temperature, the kinetic energy of gas particles drops significantly (gas particle won't move as fast). Subsequently, they can interact with one another more effectively, which will in turn result in stronger Van der Waals forces (similar to case#1). As a result, the particles are drawn close to one another, which will in turn cause the true volume of the gas to be smaller than what's predicted under standard conditions.
Answer:
1) less than predicted
2) more than predicted
3) less than predicted

Can someone explain each scenario? Thanks

I hope this helps!

 

[nartnad]

totally makes sense now. thanks