Hi there,
I have a general theory question.
Am I right to assume a liquid with a relatively high vapour pressure will have a relatively low heat of evaporation? Are they directly related?
Say some liquid has a (high) 40 kPa vapour pressure at 25degC it means the liquid has weak inter-molecular forces and many of the molecules can transition from the liquid to gas phase because they do not require much energy to do so. This is occuring at room temperature where the air temperature remains relatively constant. Therefore the amount of energy the liquid takes in from the air (heat of evap) must be quite low when in comparison to a liquid that has a low vapour pressure?
Thanks for any feedback.
I have a general theory question.
Am I right to assume a liquid with a relatively high vapour pressure will have a relatively low heat of evaporation? Are they directly related?
Say some liquid has a (high) 40 kPa vapour pressure at 25degC it means the liquid has weak inter-molecular forces and many of the molecules can transition from the liquid to gas phase because they do not require much energy to do so. This is occuring at room temperature where the air temperature remains relatively constant. Therefore the amount of energy the liquid takes in from the air (heat of evap) must be quite low when in comparison to a liquid that has a low vapour pressure?
Thanks for any feedback.
