Vapour Pressure & Liquid Phase: Explained

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If the vapor pressure of a component exceeds the system pressure, it indicates that the component will exist entirely in the vapor phase, with no liquid phase present. If a liquid phase is already present, it will start to boil away as the vapor pressure increases. When the partial pressure of a component matches its vapor pressure, any additional mass will be in the vapor phase, eliminating the liquid phase. This relationship highlights the critical balance between vapor pressure and system pressure in determining phase states. Understanding these principles is essential for applications involving phase transitions in various scientific fields.
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If the vapour pressure of a component is bigger than the system pressure, does it means it will fully in vapour phase and no liquid phase are formed??
 
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Yes, or if a liquid phase was already existing then it will begin to boil away.
 
the moment the partial pressure of a component is equal to its vapor pressure, any additional mass of that component formed must be in the vapor phase (and no longer in the liquid phase).
 

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