Although the behavior of the graph with increasing temperature at lower pressures, when the graph shows negative deviation, is justifiable ,why is it that the graph shows less positive deviation ,towards the high pressure region of the graph when the temperature increases .
i might have sent this question before twice because it was not appearing in the comments section. In case that's not the case please ignore this comment.
When the temperature is high, the high pressure is less effective at reducing the volume of the gas (i.e. the molar volume is larger). So the finite volume effects are not as important.
@@PhysicalChemistry it shows decrease in positive deviation , as temp increases in constant high pressure region .....which is not agreeable as increase in temp at high constant pressure ....must increase repuslive nature result high real volume ...high z ....but z decrease
Unfortunately, I can't. I'm not sure how we got that name for this concept. (I would love to know. Perhaps someone else can enlighten us in the comments.) "Compressibility factor" is a particularly confusing name, for several reasons. First, it is easy to get it confused with the (e.g. isothermal) compressibility, which is an entirely different thing. Second, Z doesn't seem so much like a compressiBILITY (i.e. ability to be compressed) as a compression factor (i.e. amount by which it actually is compressed). And third, it seems to be named backwards. You would expect something that is very compressible to be SMALLER than the ideal gas law would predict. But, in fact, something with a large Z has a LARGER volume than the ideal gas predicts at a given temperature and pressure. *shrug* This is the term we have, and that everyone uses, so we just have to live with it.
These equations are only *models*, not reality. Some of the models include a b term for the finite molecular volume, like the vdW model. Others do not, like the ideal gas model. You can certainly change the equations to convert V to V-Nb. And it may be more accurate. But in doing so, you've made your own model, and it is not the original model any more. Sometimes we prefer the models without finite molecular volume -- even though they are less accurate -- because they are simpler.
“I hate this doctor” got me cracking up
@@ashashankar1322 who hates what doctor??
@PhysicalChemistry I commented on the wrong video my bad
Thank you so much! This has been a big help!
You're quite welcome. I'm glad it was useful
Brilliant explanation!
Although the behavior of the graph with increasing temperature at lower pressures, when the graph shows negative deviation, is justifiable ,why is it that the graph shows less positive deviation ,towards the high pressure region of the graph when the temperature increases .
i might have sent this question before twice because it was not appearing in the comments section. In case that's not the case please ignore this comment.
When the temperature is high, the high pressure is less effective at reducing the volume of the gas (i.e. the molar volume is larger). So the finite volume effects are not as important.
.I have actually been trying to reason this out for about a month but failed to do so.Thank you so much.
@@shaurya3350 you're welcome
@@PhysicalChemistry it shows decrease in positive deviation , as temp increases in constant high pressure region .....which is not agreeable as increase in temp at high constant pressure ....must increase repuslive nature result high real volume ...high z ....but z decrease
Nice Content.... also can you please tell why "Z" is called "Compressibility Factor" ?
Unfortunately, I can't. I'm not sure how we got that name for this concept. (I would love to know. Perhaps someone else can enlighten us in the comments.)
"Compressibility factor" is a particularly confusing name, for several reasons. First, it is easy to get it confused with the (e.g. isothermal) compressibility, which is an entirely different thing. Second, Z doesn't seem so much like a compressiBILITY (i.e. ability to be compressed) as a compression factor (i.e. amount by which it actually is compressed). And third, it seems to be named backwards. You would expect something that is very compressible to be SMALLER than the ideal gas law would predict. But, in fact, something with a large Z has a LARGER volume than the ideal gas predicts at a given temperature and pressure.
*shrug* This is the term we have, and that everyone uses, so we just have to live with it.
@@PhysicalChemistry oh i see. thanks for the info!
Should not in all the equation there should be (v ideal-b ) as this whole term is equal to v real
These equations are only *models*, not reality. Some of the models include a b term for the finite molecular volume, like the vdW model. Others do not, like the ideal gas model.
You can certainly change the equations to convert V to V-Nb. And it may be more accurate. But in doing so, you've made your own model, and it is not the original model any more.
Sometimes we prefer the models without finite molecular volume -- even though they are less accurate -- because they are simpler.
nice
You can have the keys to my city.
@@Hawkman6788 PChem will open all sorts of doors ...
Wow ❤
Is he writing backwards or am I losing my mind
@@MericEyidogan Writing forwards, then reversing the image digitally