At the triple point of water how do the entropies of solid, liquid, and gas compare?
I think that either they will be equal or it will be that gas > liquid > solid.
I don't know if entropy is influenced by the fact that it will be at the triple point. Can someone please elaborate?
Triple point defines a situation of simultaneous equilibrium between the solid, the liquid and the gas phases.
For such an equilibrium, you simply write:
$$ \Delta S= \frac{\Delta H}{T} $$
that rises from the fact that $\Delta G=0$.
Considering water molar ($m$) enthalpies for each phase transition at $273\,K$:
$$ \Delta H_{melting,m}=6.01\,kJ\,mol^{-1} $$ $$ \Delta H_{vaporisation,m}=45.05\,kJ\,mol^{-1} $$ $$ \Delta H_{sublimation,m}=51.06\,kJ\,mol^{-1} $$
one realises that
In this respect the triple point has no peculiar behaviour compared to other points where a two-phase equilibrium is established.
