The following table gives the vapor pressure of hexafluorobenzene \(\left(\mathrm{C}_{6} \mathrm{~F}_{6}\right)\) as a function of temperature: $$ \begin{array}{lc} \text { Temperature (K) } & \text { Vapor Pressure (torr) } \\ \hline 280.0 & 32.42 \\ 300.0 & 92.47 \\ 320.0 & 225.1 \\ 330.0 & 334.4 \\ 340.0 & 482.9 \end{array} $$ (a) By plotting these data in a suitable fashion, determine whether the Clausius-Clapeyron equation (Equation 11.1 ) is obeyed. If it is obeyed, use your plot to determine \(\Delta H_{\text {vap }}\) for \(\mathrm{C}_{6} \mathrm{~F}_{6}\) (b) Use these data to determine the boiling point of the compound.

The enthalpy of vaporization for hexafluorobenzene, \(\Delta H_{vap}\), can be found by plotting the natural logarithm of vapor pressure versus the inverse of temperature. Since the plot is a straight line, the Clausius-Clapeyron equation is obeyed. The slope of the plot can be used to calculate the enthalpy of vaporization as \(\Delta H_{vap} = -slope \times R\), where \(R\) is the ideal gas constant. The boiling point of hexafluorobenzene can be found using the Clausius-Clapeyron equation with the atmospheric pressure set to 760 torr. The boiling point temperature, \(T_{BP}\), is given by \(T_{BP}=\frac{1}{\frac{1}{T_1}+\frac{R}{\Delta H_{vap}}ln\frac{760}{P_1}}\). Plug in the appropriate values to calculate the boiling point temperature.