Appendix B lists the vapor pressure of water at various external pressures. (a) Plot the data in Appendix B, vapor pressure (torr) versus temperature \(\left({ }^{\circ} \mathrm{C}\right) .\) From your plot, estimate the vapor pressure of water at body temperature, \(37^{\circ} \mathrm{C}\). (b) Explain the significance of the data point at 760.0 torr, \(100^{\circ} \mathrm{C}\) (c) A city at an altitude of \(5000 \mathrm{ft}\) above sea level has a barometric pressure of 633 torr. To what temperature would you have to heat water to boil it in this city? (d) A city at an altitude of \(500 \mathrm{ft}\) below sea level would have a barometric pressure of 774 torr. To what temperature would you have to heat water to boil it in this city? (e) For the two cities in parts \((\mathrm{c})\) and \((\mathrm{d}),\) compare the average kinetic energies of the water molecules at their boiling points. Are the kinetic energies the same or different? Explain.

(a) After plotting the data from Appendix B, we can estimate the vapor pressure of water at body temperature ($37^{\circ} \mathrm{C}$) to be approximately 47 torr. (b) The data point at 760.0 torr and $100^{\circ} \mathrm{C}$ is significant because it represents the boiling point of water at standard atmospheric pressure (1 atm), where water changes from its liquid phase to its gas phase. (c) In the city at an altitude of $5000 \mathrm{ft}$ with a barometric pressure of 633 torr, you would have to heat water to approximately $94^{\circ} \mathrm{C}$ to boil it. (d) In the city at an altitude of $500 \mathrm{ft}$ below sea level with a barometric pressure of 774 torr, you would have to heat water to approximately $102^{\circ} \mathrm{C}$ to boil it. (e) The average kinetic energies of the water molecules at boiling points in the two cities are the same, as the kinetic energy needed to change water from liquid to gas (boiling point) remains constant regardless of external pressure.