Welcome Guest Search | Active Topics |

 Real Gases Previous Topic Next Topic
 Nicole_5521 #1 Posted : Wednesday, July 14, 2021 3:11:29 AM Rank: Advanced MemberGroups: Registered Joined: 4/30/2020Posts: 71Thanks: 0 timesWas thanked: 0 time(s) in 0 post(s) Hi,I'm wondering why at high pressures gases deviate from ideal behaviour, but when looking at real vs. ideal gases, the pressure of a real gas is actually lower than ideal gas? Why do these 2 points seem like they contradict each other?Thanks! Back to top | Edit by user User Profile
 INSTR_Calla_139 #2 Posted : Thursday, July 15, 2021 4:48:58 PM Rank: MemberGroups: Registered Joined: 6/8/2021Posts: 13Thanks: 0 timesWas thanked: 0 time(s) in 0 post(s) Hi Nicole,At high pressures gasses deviate from ideal behavior because the molecules are closer together which causes intermolecular forces that are not accounted for in ideal gas behavior. These forces would make the assumptions about real gasses incorrect - which is why they deviate from ideal behavior. A real gas should be under more pressure than an ideal gas because a real gas has a finite volume where as an ideal gas doesn't. Back to top User Profile
 Nicole_5521 #3 Posted : Saturday, July 17, 2021 2:22:27 AM Rank: Advanced MemberGroups: Registered Joined: 4/30/2020Posts: 71Thanks: 0 timesWas thanked: 0 time(s) in 0 post(s) Hello,In the real gases section in the CC pg. 352, it mentioned that "For real gases, attractive forces between gas molecules lead to lower pressures than predicted by the ideal gas law." How come the pressure of a real gas is lower?But, at the same time, gases are real at high pressures?Why do these 2 points seem contradictory?Thank you! Back to top User Profile
 INSTR_Molly_129 #4 Posted : Saturday, July 17, 2021 9:20:11 PM Rank: Advanced MemberGroups: Registered Joined: 5/23/2021Posts: 74Thanks: 0 timesWas thanked: 0 time(s) in 0 post(s) Hi Nicole,These are two different concepts.Real gases are different from ideal gases, in that in ideal gases, we assume that there is no attractive forces between atoms, when really, there are. This is why the pressure of real gases are slightly smaller than ideal.Now, at high pressures, gases are "pushed" by the pressure to become more liquid, which is why at high pressures, gases become LESS ideal, and become "real". They can no longer say that in such a small amount of volume, that it the volume each gas particle takes up is negligible.Hope this helps!Molly Back to top User Profile
 Users browsing this topic Guest
You cannot post new topics in this forum.
You cannot reply to topics in this forum.
You cannot delete your posts in this forum.
You cannot edit your posts in this forum.
You cannot create polls in this forum.
You cannot vote in polls in this forum.

Clean Slate theme by Jaben Cargman (Tiny Gecko)
Powered by YAF | YAF © 2003-2009, Yet Another Forum.NET
This page was generated in 0.095 seconds.