Calculate the entropy of a liquid water at $100$C given de data below. Assume that the vapor is ideal. How does your answer compare to the value of $23\mathrm{.}52$ J$/$mol$*$K given in the steam tables?

Data:

State $1$: SL $(298$ K$,3168$ Pa$)=6\mathrm{.}06$ J$/$mol$*$K

State $1$: Delta H $(298$K$)=43\mathrm{.}85$ KJ$/$mol

State $2$: Psat $(375$K$)=101325$ Pa

State $2$: Delta H $(373$K$)=40\mathrm{.}62$ KJ$/$mol

The ideal gas heat capacity $($T in K$)$

Cp$/$R $=3\mathrm{.}470+0\mathrm{.}00145*$T $+(12100/$T$^2)$