Boiling point and vapor pressure

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SUMMARY

The discussion centers on the fundamental concept of boiling and vapor pressure, specifically how boiling occurs when a liquid's vapor pressure equals the surrounding atmospheric pressure. The participants agree that this is a key principle, but seek clarification on the physical processes that enable vapor formation throughout the liquid at this point. The pressure inside the liquid, such as water, is typically around 1 atmosphere, which aligns with the conditions for boiling.

PREREQUISITES
  • Understanding of vapor pressure and its relationship to boiling points
  • Basic knowledge of atmospheric pressure and its measurement
  • Familiarity with the physical states of matter (solid, liquid, gas)
  • Concept of phase transitions in thermodynamics
NEXT STEPS
  • Research the molecular dynamics of boiling and vapor formation
  • Study the relationship between temperature and vapor pressure using the Clausius-Clapeyron equation
  • Explore the effects of altitude on boiling points and vapor pressure
  • Investigate the role of impurities and surface tension in boiling processes
USEFUL FOR

Students in chemistry or physics, educators teaching thermodynamics, and anyone interested in the physical principles of phase transitions and boiling phenomena.

sashankhrao
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I am trying to understand the concept of boiling from a very fundamental perspective. Most textbooks say that: as a liquid is heated, it's vapor pressure increases. When the vapor pressure reaches the surrounding pressure(or atmospheric pressure at that point), then boiling occurs.

I agree with the above point.

My question is: when the vapor pressure reaches the surrounding pressure, what physically happens that allows vapor to form all through the liquid for it to boil.

Thanks
 
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The pressure from inside the water is not much more than 1 atmosphere either. Seems reasonable to me.
 

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