The evaporation of one mole of water at $298 \mathrm{~K}$ has a standard free energy change of $8.58 \mathrm{~kJ}$. $\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(g) \quad \Delta G^{\circ}=8.58 \mathrm{~kJ}$
(a) Is the evaporation of water under standard thermodynamic conditions spontaneous?
(b) Determine the equilibrium constant, $K_{p}$, for this physical process.
(c) By calculating $\Delta G,$ determine if the evaporation of water at $298 \mathrm{~K}$ is spontaneous when the partial pressure of water, $P_{\mathrm{H}_{2} \mathrm{O}},$ is $0.011 \mathrm{~atm} .$
(d) If the evaporation of water were always nonspontaneous at room temperature, wet laundry would never dry when placed outside. In order for laundry to dry, what must be the value of $P_{\mathrm{H}_{2}} \mathrm{O}$ in the air?