- #1
americast
- 27
- 0
Hi all,
I am facing difficulty in understanding the reason behind the fact that a liquid boils when the atmospheric pressure is equal to its vapour pressure.
We know that at the vapour pressure, the air and the liquid remain in equilibrium, so there's no net evaporation or condensation. So, why does this not hold true at the boiling point? According to me, at the boiling temperature, there should be no vaporization at all.
Gramercy...
I am facing difficulty in understanding the reason behind the fact that a liquid boils when the atmospheric pressure is equal to its vapour pressure.
We know that at the vapour pressure, the air and the liquid remain in equilibrium, so there's no net evaporation or condensation. So, why does this not hold true at the boiling point? According to me, at the boiling temperature, there should be no vaporization at all.
Gramercy...