Insights Blog
-- Browse All Articles --
Physics Articles
Physics Tutorials
Physics Guides
Physics FAQ
Math Articles
Math Tutorials
Math Guides
Math FAQ
Education Articles
Education Guides
Bio/Chem Articles
Technology Guides
Computer Science Tutorials
Forums
Chemistry
Biology and Medical
Earth Sciences
Computer Science
Computing and Technology
DIY Projects
Trending
Featured Threads
Log in
Register
What's new
Search
Search
Search titles only
By:
Chemistry
Biology and Medical
Earth Sciences
Computer Science
Computing and Technology
DIY Projects
Menu
Log in
Register
Navigation
More options
Contact us
Close Menu
JavaScript is disabled. For a better experience, please enable JavaScript in your browser before proceeding.
You are using an out of date browser. It may not display this or other websites correctly.
You should upgrade or use an
alternative browser
.
Forums
Other Sciences
Chemistry
Vapor pressure -- How does water still boil at 100°C in an open pot?
Reply to thread
Message
[QUOTE="pisluca99, post: 6828486, member: 730550"] ok, to recap: - below boiling temperature, only evaporation occurs, involving only the surface of the liquid. In particular, if the container is open, the liquid-vapour equilibrium is established only in the 'mass' of water and not above it, because the vaporised water molecules are dispersed in the surrounding atmosphere (it is as if they became an integral part of the gases in the air), therefore evaporation never stops. If, on the other hand, the container is hermetically closed, the liquid-vapour equilibrium is also established 'above' the solution and this allows us to evaluate the vapor pressure of this saturated vapor at equilibrium. If so, evaporation stops. - At boiling temperature, vapor pressure developed in the liquid-vapour equilibrium reaches and overcomes the atmospheric pressure, so the vapor is released in the form of bubbles which rise throughout the mass of water (if the container is open). Conversely, if the container is hermetically sealed, boiling will never occur, as the vapor pressure will never be able to reach the pressure that presses on the water (it is true that as the temperature increases, the vapor pressure increases in the water, but also increases the pressure pressing on the water itself, given by the sum of the pressure of the saturated steam developed + atmospheric pressure), unless there is a vent, as in the case of the pressure cooker. [/QUOTE]
Insert quotes…
Post reply
Forums
Other Sciences
Chemistry
Vapor pressure -- How does water still boil at 100°C in an open pot?
Back
Top