suppose you had 1.0 mol samples of the following gases at STP. if the volume of each of the samples of gas was reduced to one tenth of its original size and the temperatures remained the same, which gas would have the lowest pressure?
A)C6H8
B)C3H4
C)N2
D)O2
E)Cl2

Question

suppose you had 1.0 mol samples of the following gases at STP. if the volume of each of the samples of gas was reduced to one tenth of its original size and the temperatures remained the same, which gas would have the lowest pressure?
A)C6H8
B)C3H4
C)N2
D)O2
E)Cl2

anonymous · Answer

The one with the lowest molar mass...?

anonymous · Answer

I am thinking nitrogen?????

anonymous · Answer

okay but can you please explain why it would be the one with the lowest molar mass?

anonymous · Answer

I am not quite sure now that I think about it. Since the gases are at STP and they are all 1.0 mol, that means each gases have a volume of 22.4L. If each is reduced to one tenth, all should now have a volume of 2.24L.

anonymous · Answer

With the same number of moles, same volume, same temperature, the pressure should also be the same...?

anonymous · Answer

I am sorry, I don't have a solid answer to that.

anonymous · Answer

I was thinking the same thing as you.

australopithecus · Answer

It wont be the same because we need to think of this in terms of real gasses

anonymous · Answer

Real gases are such a pain T^T

australopithecus · Answer

You guys need to realize that the ideal gas law is just a model for gases that do not interact intermolecularly

australopithecus · Answer

In reality these gases do interact intermolecularly and this effects their properties as a gas

australopithecus · Answer

https://en.wikipedia.org/wiki/Real_gas

australopithecus · Answer

Pick one of the models to apply or maybe your text book or prof gave you a specific model to utilize

australopithecus · Answer

Or you could try using logic