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Explain why you might expect the behavior of carbon dioxide to be less ideal than that of hydrogen?

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Which one has stronger inter molecular forces ?

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Other answers:

Eh ? why ?
oh yes carbon dioxide.. i was about to write it..
Why carbon dioxide then ?
can u tell me...
Yes I can, but you don't know why CO2 has stronger intermolecular forces? just guessed it hmm ?
because.... it has lone pair of electrons ?
o.O NOPES! CO2 has larger size! Hence a greater Van der Wall's force of attraction. Thus CO2 has greater intermolecular forces.
Now, reason you need to know that is : One of the many assumptions of an ideal gas is that Intermolecular forces of an ideal gas are negligible (or 0) More the intermolecular forces, lesser the ideality of the gas, or more the deviation from ideal behavior. So , you got your answer ?
OH YES! I got it!
:) Can i ask you 3 to 4 more questions i need to know for my assignment ?
But I gotta go soon. You should study harder for the homework, comeon, consult some good books. Best of luck. :)
Its alright if u r going.. i'll submit my assignment on 20th of january
Tell me the ans: Under what conditions of temperature and pressure would you expect the behavior of CO2 to be most like an ideal gas?
For a gas to behave ideally, Intermolecular forces must be minimum. What can you make out of this ?
to decrease the pressure and inc the temp ? to make it ideal
Are you just guessing it ?
no i m telling u the answer..
What logic you apply ?
At low pressure and high temp, intermolecular forces do not attract which makes the gas ideal
Just beating around the bush aren;t you ? :D
i m right... i think
Anyways, that answer is correct At high temperature, rms velocity (or average velocity) of gases inc, which enables them to move with higher speed much more freely, which is accompanied by low pressure.
But if we relate it to kinetic molecular theory then my answer will be correct.. No?
That is what i just said, I related to KTOG only yes that is correct.

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