- #1
mayer
- 38
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So I understand that you get boiling when the vapor pressure equals atmospheric pressure so that the vapor within the medium can overcome the atmospheric pressure pressing on the surface of the liquid, but how do the bubbles overcome the hydrostatic pressure from the water above the bubble. If the vapor in the bubble is only at atmospheric pressure, wouldn't it collapse under the weight of the water above it? Is it because, if being boiled over a stove-top, the temperature source is heating the vapor in the bubbles to a pressure above atmospheric? If so, how come bubbles still form under the surface when you are boiling under a vacuum at room temperature, where the liquid is actually getting colder?
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