Chemca Chemistry Made Easy
Vapor Pressure & Boiling Simulation
Concept Quiz
Vapor Pressure & Clausius-Clapeyron
Liquids constantly evaporate as high-energy molecules escape the surface. In a closed container, these gas molecules collide with the walls, exerting a pressure known as Vapor Pressure ($P_{vap}$). As temperature increases, more molecules escape, and vapor pressure rises exponentially according to the Clausius-Clapeyron equation:
$$\ln(P_{vap}) = -\frac{\Delta H_{vap}}{R} \left( \frac{1}{T} \right) + C$$
Definition of Boiling:
A liquid boils only when its Vapor Pressure equals or exceeds the external Atmospheric Pressure ($P_{vap} \ge P_{atm}$). At this point, gas bubbles can form inside the liquid body and rise to the surface without being crushed by atmospheric weight.
A liquid boils only when its Vapor Pressure equals or exceeds the external Atmospheric Pressure ($P_{vap} \ge P_{atm}$). At this point, gas bubbles can form inside the liquid body and rise to the surface without being crushed by atmospheric weight.
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