Appendix B lists the vapor pressure of water at various external pressures. (c) A city at an altitude of 5000 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?

Key Concepts

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid or solid form at a given temperature. It indicates how readily a substance will evaporate; higher vapor pressure means a substance will boil at a lower temperature. Understanding vapor pressure is crucial for determining boiling points under varying external pressures.

Boiling Point

The boiling point of a liquid is the temperature at which its vapor pressure equals the external pressure surrounding the liquid. At higher altitudes, the atmospheric pressure is lower, which decreases the boiling point of water. This concept is essential for calculating the temperature needed to boil water in locations with different barometric pressures.

Barometric Pressure

Barometric pressure, or atmospheric pressure, is the pressure exerted by the weight of the atmosphere above a given point. It varies with altitude; as altitude increases, barometric pressure decreases. This relationship is important for understanding how boiling points change in different geographical locations, such as cities at high elevations.