For a liquid, why is it when the vapour pressure is equal to atmospheric pressure, the liquid starts to boil?
- Anonymous1 decade agoFavorite Answer
Vapor pressure= strength of liquid pushing up.
Atmospheric pressure= strength of force pushing down on it.
Boiling is where they are equal to each other because the Vapor pressure (force pushing up) is equal to the atmospheric pressure (force pushing down). Some liquids are more volatile (evaporate easily; have low boiling points) than others because their vapor pressure is extremely strong. The weaker a vapor pressure, the harder it is for it to become a gas. Water has an extremely weak vapor pressure, making it's boiling point 100ºC. If you go over this temperature, the water turns into it's gaseous form, steam. The reason steam always turns back to liquid so quickly is because once it gets away from the heat, it's temperature decreases and the force pushing it upwards is no longer as great as the force pushing down on it.
- grandpreLv 44 years ago
via very reality the vapor stress wont truly be such as atm stress so its attempting to stability the equilibrium by skill of boiling. there's a eq consistent for this such as pka so u can imagine of of this via very reality the ph is above the pka of an acid so the acid will provide its proton