Timeline for Why do liquids boil when their vapor pressure equals the ambient pressure?
Current License: CC BY-SA 3.0
6 events
| when toggle format | what | by | license | comment | |
|---|---|---|---|---|---|
| Sep 2, 2014 at 4:03 | comment | added | André Chalella | THIS! @clark599, your comment about equilibrium is EXACTLY what I was looking for! | |
| Aug 6, 2014 at 2:58 | vote | accept | Tim Clark | ||
| Aug 6, 2014 at 2:57 | comment | added | Tim Clark | Thanks for the answer. "There is no possibility for the water bubbles to form at any other pressure than the vapor pressure" definitely addresses my question, but I was wondering why this is so, if it is true. After some thought, I think the answer is simple: if the pressure in such a bubble were higher than the v.p., some bubble vapor molecules would condense until the pressure was the v.p. If it were less than the v.p., inner surface liquid molecules would evaporate into it until the pressure was the v.p. I needed to apply equilibrium logic to the inner surface of the bubble. | |
| Aug 5, 2014 at 15:18 | comment | added | Whelp | Perhaps I should rephrase that. What I meant to say is that the bubbles that can be observed before the water is hot enough for boiling are composed of dissolved air gases. | |
| Aug 5, 2014 at 13:32 | comment | added | LDC3 | When I watch a pot boil, I see 2 types of bubbles. Ones that rise to the surface (dissolved gases) and ones that disappear rising to the surface. What would be in those bubbles if it is not water vapor? | |
| Aug 5, 2014 at 6:42 | history | answered | Whelp | CC BY-SA 3.0 |