Consider the vaporization of some liquid (call it X): X(l) → X(g)
At 298K, the enthalpy of vaporization of X, $\Delta H^{\circ}$ is 41.60 kJ/mol, and its entropy of vaporization, $\Delta S^{\circ}$, is 124.13 J mol$^{-1}$ K$^{-1}$. The graphs are the vaporization curve for X, and the free energy as a function of composition of X at 298K. Determine the following for X.
a) What is the standard free energy of vaporization of X at 298K?
$\Delta G^{\circ}$ = 4.61 kJ/mol
b) What is the value of the equilibrium constant for the vaporization of X at 298K?
K = 0.156
c) What is the vapor pressure of X at 298K in torr ($P_A$ on the graph)?
$p^{\circ}$ = 118.3 torr
The pressure of X vapor in a closed container at 298K was found to be 57.3 torr. What is the value of $\Delta G$ for the process X(l) → X(g) at the time the pressure was measured?
d) $\Delta G$ = 2.81 kJ
e) Which point on the G vs Composition graph most closely matches the point at which this measurement is taken?
f) Which point on the same graph does the measurement in part c correspond?
