Hi Pat...can you just explain elaborately that why at boiling the vapour pressure need to be greater than equal to the surrounding pressure? I mean what is happening at microscopic level? Can you make a video on this specific question?
As I understand it when the external pressure is greater than the vapor pressure it prevents molecules from breaking free of one another inside the liquid, forming gas bubbles. Remember that a gas is highly compressible and the external pressure inhibits formation of gas bubbles inside the liquid. This is no longer the case once the vapor pressure exceeds the external pressure and boiling occurs.
Hi Pat...can you just explain elaborately that why at boiling the vapour pressure need to be greater than equal to the surrounding pressure? I mean what is happening at microscopic level? Can you make a video on this specific question?
As I understand it when the external pressure is greater than the vapor pressure it prevents molecules from breaking free of one another inside the liquid, forming gas bubbles. Remember that a gas is highly compressible and the external pressure inhibits formation of gas bubbles inside the liquid. This is no longer the case once the vapor pressure exceeds the external pressure and boiling occurs.