This discussion centers on the concept of boiling and saturated vapor pressure, emphasizing that boiling occurs when the vapor pressure of gas bubbles equals the surrounding atmospheric pressure. The formation of gas bubbles beneath the liquid surface is critical, as these bubbles must maintain pressure equal to or greater than the surrounding fluid to prevent collapse. Participants also explore the effects of liquid density and gravitational pressure on boiling, concluding that boiling can occur when vapor pressure reaches 1.1 times the atmospheric pressure, accounting for factors like bubble surface tension.
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Fightfish said:Boiling refers to the process whereby a phase change from liquid to gas takes place throughout the liquid. This would imply the formation of gas bubbles beneath the liquid surface. That is why bubbling is a characteristic of boiling liquids.
Now, the pressure in the gas bubbles must be at least equal to that of the surrounding fluid and the atmosphere/environment. Otherwise, the bubbles will collapse, and boiling does not occur. Thus, the boiling can only occur at the point where the vapour pressure (of the gas bubbles) equals the pressure of the surroundings.