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Apr 16, 2021 at 15:58 history edited user281837 CC BY-SA 4.0
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Apr 16, 2021 at 15:57 history closed Mithoron
Mathew Mahindaratne
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Duplicate of Why must both the critical temperature and pressure be exceeded to achieve the supercritical phase?
Apr 16, 2021 at 15:05 answer added Karsten timeline score: 2
Apr 16, 2021 at 13:17 answer added Neil_UK timeline score: 2
Apr 16, 2021 at 13:06 history edited Buck Thorn
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Apr 16, 2021 at 12:56 history edited Buck Thorn CC BY-SA 4.0
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Apr 15, 2021 at 21:43 review Close votes
Apr 16, 2021 at 9:25
Apr 15, 2021 at 17:54 history became hot network question
Apr 15, 2021 at 13:23 comment added Alchimista In short, it is not that you cannot push them against each other. It is that they don't stay.
Apr 15, 2021 at 12:40 answer added Oscar Lanzi timeline score: 14
Apr 15, 2021 at 11:12 comment added Karl Critical temperature means the evaporation enthalpy has become zero. The term "liquify" makes no sense then.
Apr 15, 2021 at 10:38 answer added Poutnik timeline score: 16
Apr 15, 2021 at 10:08 comment added Ivan Neretin What is so special about the age of 18 (in many jurisdictions) that makes a person suddenly acquire all those rights? Nothing, except a human convention. Same thing here. Sure, by applying enough pressure you may bring the molecules of a supercritical fluid as close as they are in liquid. It is just that we don't call that "liquid".
Apr 15, 2021 at 10:01 comment added Desai The temperature is too high to allow any inter molecular attractions that'd help them liquefy. Imagine you're running a relay race and have to hand over the baton to the next member, if you're running too fast then the baton cannot be passed. I know it's a funny way to understand it but that's how I think of it.
Apr 15, 2021 at 9:51 history asked user281837 CC BY-SA 4.0