Trying to figure out the other (or additional ones I missed) episode where someone retroactively lost points for an answer.
I recall it was one WITH Dara in it because he commented on how he lost points via that mechanism already. I think the guest lost points from an earlier episode in the same series because Dara one-upped the guest by saying he already lost points from a different series.
The triple point is the temperature and pressure at which solid, liquid, and vapor may exist in equilibrium with one another. However, at this pressure and temperature there are still infinite values of specific enthalpy for this 3-phase mixture, because it requires heat to melt/vaporize the components.
If we are heating ice at 611.2 Pa, then we can define the enthalpy of pure ice at 611.2 Pa and 273.16 K to be some value H. If we add heat until it is completely vapor, then the pressure will still be 611.2 Pa and the temperature will be 273.16 K, but the enthalpy will be some value H + ΞH.
At any given enthalpy between H and H + ΞH, there will be 3 phases in equilibrium - solid, liquid, and vapor. I'd like to figure out the composition (i.e. %solid, %liquid, %vapor) as a function of enthalpy between these two values and I'm very much struggling with this. Does anybody have insight into this?
I'm presuming that at first, ~100% of the added heat goes into melting the solid and as the amount of solid approaches zero, ~100% of the added heat goes into vaporizing the liquid. What happens in the middle is much more complicated. I made a graph of what I think it would look like, but this definitely isn't a state function by any means. If somebody could give me an equation or an article about this, I'd be super grateful. Thanks!
To add clarity, it would be equivalent to calculating composition as you move left-to-right on the triple point line of this plot:
