- #1
Silvius
- 13
- 0
Hey guys,
I was just hoping to clear something up regarding enthalpies of vaporization.
The idea of the heat of vaporization for a substance being "temperature dependent" is confusing me, as I had been under the impression that these quantities were only considered at the boiling point of a substance. That is, you impart a certain amount of energy to raise the temperature of liquid water at some pressure to 100°C, and then the ΔH[itex]_{vap}[/itex] represents the extra energy which needed to be imparted to then convert that liquid water to water vapour (without any raise in temperature).
What, then, would a ΔH[itex]_{vap}[/itex] at some other temperature represent, given that you are not at a sufficiently high temperature for vaporization to occur...?
Thanks!
I was just hoping to clear something up regarding enthalpies of vaporization.
The idea of the heat of vaporization for a substance being "temperature dependent" is confusing me, as I had been under the impression that these quantities were only considered at the boiling point of a substance. That is, you impart a certain amount of energy to raise the temperature of liquid water at some pressure to 100°C, and then the ΔH[itex]_{vap}[/itex] represents the extra energy which needed to be imparted to then convert that liquid water to water vapour (without any raise in temperature).
What, then, would a ΔH[itex]_{vap}[/itex] at some other temperature represent, given that you are not at a sufficiently high temperature for vaporization to occur...?
Thanks!