The Clausius-Clapeyron equation can be used to estimate how the boiling point changes with pressure, or how the vapor pressure changes with temperature.
I knew the Clausius-Clapeyron equation was important, but I didn't realize it had life-or-death consequences! In any case, I'm honored to have been your lifeline.
Thank you very much for upoading these great lectures. I am a bit confused about the dew example. Even if the temperature goes down the water should still be under 1 atm, right? I interpreted the pressure to be the total pressure on the substance. Like in the 'Phase Diagrams' video you described the behaviour of water as a function of temperature and you considered the pressure over water to be 1 atm. That made sense to me. Now when talking about the formation of dew why do we consider the vapor pressure of water? Like I get that the drop in temperature would lower the vapor pressure of water, but why do we use that to conclude that water has to condense? I would have thought that it should still be under 1 atm pressure. I am a bit confused with that.
Thank you again, still fascinated by your lecturing techniques! My question is how the phase diagram of water would look if the gas phase is pure CO2 gas, light hydrocarbon gases, or any other pure gases instead of atmospheric gas, i.e., composed of mainly N2 and O2. I am assuming that the phase diagram of water you discussed here uses atmospheric gas as a gas phase to find the molar enthalpy of the vaporization of water. I would like to discuss this with you further in relation to my research question.
This is a single-component phase diagram, which means it only considers water (steam) in the vapor phase. The presence of any other gases (CO2, N2, whatever) will not change the phase diagram. The enthalpy of vaporization likewise is an inherent property of water, and is not affected by the presence of other gases
@@PhysicalChemistry thank you for your answer and i would like to come with little detailed information and question, is there way to reach you by email then? Thanks
Sir for significant change in temp. or pressure latent heat also changes ( i mean deltaH is vriable). Is there any relation for deltaH in the function of temp or pressure?
Yes, that's definitely correct: ΔH is *not* constant. Here's a video with some information on how ΔH depends on T: ru-vid.com/video/%D0%B2%D0%B8%D0%B4%D0%B5%D0%BE-Sl3o9z9X9cI.html
