jkasdhk
Explain why you might expect the behavior of carbon dioxide to be less ideal than that of hydrogen?
Delete
Share
This Question is Closed
jkasdhk
Best Response
You've already chosen the best response.
0
@shubhamsrg
shubhamsrg
Best Response
You've already chosen the best response.
1
Which one has stronger inter molecular forces ?
jkasdhk
Best Response
You've already chosen the best response.
0
Hydrogen
jkasdhk
Best Response
You've already chosen the best response.
0
?
shubhamsrg
Best Response
You've already chosen the best response.
1
Eh ? why ?
jkasdhk
Best Response
You've already chosen the best response.
0
oh yes carbon dioxide.. i was about to write it..
shubhamsrg
Best Response
You've already chosen the best response.
1
Why carbon dioxide then ?
jkasdhk
Best Response
You've already chosen the best response.
0
can u tell me...
shubhamsrg
Best Response
You've already chosen the best response.
1
Yes I can, but you don't know why CO2 has stronger intermolecular forces? just guessed it hmm ?
jkasdhk
Best Response
You've already chosen the best response.
0
because.... it has lone pair of electrons ?
shubhamsrg
Best Response
You've already chosen the best response.
1
o.O
NOPES!
CO2 has larger size! Hence a greater Van der Wall's force of attraction. Thus CO2 has greater intermolecular forces.
jkasdhk
Best Response
You've already chosen the best response.
0
OK OK
shubhamsrg
Best Response
You've already chosen the best response.
1
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 ?
jkasdhk
Best Response
You've already chosen the best response.
0
OH YES! I got it!
jkasdhk
Best Response
You've already chosen the best response.
0
:) Can i ask you 3 to 4 more questions i need to know for my assignment ?
shubhamsrg
Best Response
You've already chosen the best response.
1
But I gotta go soon.
You should study harder for the homework, comeon, consult some good books. Best of luck. :)
jkasdhk
Best Response
You've already chosen the best response.
0
Its alright if u r going.. i'll submit my assignment on 20th of january
jkasdhk
Best Response
You've already chosen the best response.
0
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?
shubhamsrg
Best Response
You've already chosen the best response.
1
For a gas to behave ideally, Intermolecular forces must be minimum.
What can you make out of this ?
jkasdhk
Best Response
You've already chosen the best response.
0
to decrease the pressure and inc the temp ? to make it ideal
shubhamsrg
Best Response
You've already chosen the best response.
1
Are you just guessing it ?
jkasdhk
Best Response
You've already chosen the best response.
0
no i m telling u the answer..
shubhamsrg
Best Response
You've already chosen the best response.
1
What logic you apply ?
jkasdhk
Best Response
You've already chosen the best response.
0
At low pressure and high temp, intermolecular forces do not attract which makes the gas ideal
jkasdhk
Best Response
You've already chosen the best response.
0
?
shubhamsrg
Best Response
You've already chosen the best response.
1
Just beating around the bush aren;t you ? :D
jkasdhk
Best Response
You've already chosen the best response.
0
i m right... i think
shubhamsrg
Best Response
You've already chosen the best response.
1
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.
jkasdhk
Best Response
You've already chosen the best response.
0
But if we relate it to kinetic molecular theory then my answer will be correct.. No?
shubhamsrg
Best Response
You've already chosen the best response.
1
That is what i just said, I related to KTOG only
yes that is correct.
shubhamsrg
Best Response
You've already chosen the best response.
1
BYE -BYE! :P