Assuming that the latent heat of vaporization of water \(L_{\mathrm{V}}=2260 \mathrm{~kJ} / \mathrm{kg}\) is independent of temperature and the specific volume of the liquid phase is negligible compared to the specific volume of the vapor phase, \(v_{\text {vapor }}=k T / P_{\sigma}(T)\), integrate the Clausius-Clapeyron equation (4.7.7) to obtain the coexistence pressure as a function of temperature. Compare your result to the experimental vapor pressure of water from the triple point to \(200^{\circ} \mathrm{C}\). The equilibrium vapor pressure at \(373 \mathrm{~K}\) is \(101 \mathrm{kPa}=1 \mathrm{~atm}\).