Estimate the boiling point of water in Leadville, Colorado, elevation 3170 m. To do this, use the barometric formula relating pressure and altitude: \(P=P_{0} \times 10^{-\mathrm{Mgh} / 2.303 \mathrm{RT}} \quad(\text { where } P=\text { pressure } \mathrm{in}\) atm; \(P_{0}=1 \mathrm{atm} ; g=\) acceleration due to gravity; molar mass of air, \(M=0.02896 \mathrm{kg} \mathrm{mol}^{-1} ; \quad R=\) \(8.3145 \mathrm{Jmol}^{-1} \mathrm{K}^{-1} ;\) and \(T\) is the Kelvin temperature). Assume the air temperature is \(10.0^{\circ} \mathrm{C}\) and that \(\Delta H_{\text {vap }}=41 \mathrm{kJ} \mathrm{mol}^{-1} \mathrm{H}_{2} \mathrm{O}\)

The barometric formula is a key concept that relates the atmospheric pressure at different altitudes. Understanding this concept is significant when it comes to predicting how certain physical phenomena, such as the boiling point of water, will differ with elevation.

At sea level, the atmospheric pressure is generally considered to be 1 atm, but this decreases with increasing altitude. This relationship is precisely described by the barometric formula, which is mathematically represented as \(P=P_{0} \times 10^{-\frac{Mgh}{2.303RT}}\). In this equation, \(P\) is the pressure at altitude, \(P_{0}\) is the reference pressure at sea level (usually 1 atm), \(M\) is the molar mass of air, \(g\) is the acceleration due to gravity, \(h\) is the altitude in meters, \(R\) is the universal gas constant, and \(T\) is the temperature in Kelvin.

The use of this formula allows us to calculate how pressure changes with altitude, which is essential for estimating boiling points and understanding meteorological patterns among other applications.

Moving onto another crucial concept, the Clausius–Clapeyron relation describes how the pressure of a substance's vapor changes with temperature, particularly at the boiling point. It forms the base for understanding how the boiling point of water changes with atmospheric pressure, which directly relates to altitude changes.

The relation is usually presented as \( ln(\frac{P_2}{P_1}) = -\frac{\Delta H_{vap}}{R} (\frac{1}{T_2} - \frac{1}{T_1}) \), where \(P_1\) and \(P_2\) are the vapor pressures at temperatures \(T_1\) and \(T_2\) respectively, \(\Delta H_{vap}\) is the enthalpy of vaporization, and \(R\) is the universal gas constant.

For a given enthalpy of vaporization and initial boiling point, this relation allows us to estimate the new boiling point of a liquid (like water) at a different pressure, such as that found at the altitude of Leadville, Colorado.

Enthalpy of vaporization (\(\Delta H_{vap}\)) is a term that might seem daunting, but it simply refers to the amount of energy required to convert one mole of a liquid into vapor at a constant temperature and pressure. It is a key ingredient in the Clausius–Clapeyron relation and is paramount in calculating the changes in boiling points due to pressure variations.

The value of \(\Delta H_{vap}\) is unique for every substance; for water, it is about 41 kJ/mol. This amount of energy must be absorbed by water to transition from its liquid state to gas at its boiling point under normal atmospheric pressure (1 atm).

Understanding the concept of enthalpy of vaporization is essential, as it is an intrinsic property that affects how we can boil water at different altitudes, for example. It also has wider applications in areas such as chemical engineering, meteorology, and the culinary arts.

Last but not least, atmospheric pressure is the force exerted by the weight of the air in the atmosphere of Earth. It is an everyday concept that affects many aspects of daily life, from weather forecasts to cooking. At sea level, atmospheric pressure is standardized at approximately 1 atm, but this decreases with altitude because there is less air above to exert pressure.

Atmospheric pressure is influenced by altitude, temperature, and local weather conditions. It is essential to consider when estimating the boiling point of liquids, as boiling occurs when the vapor pressure equals the external pressure. This means that at higher altitudes, where atmospheric pressure is lower, water will boil at a lower temperature.

Recognizing the impact of atmospheric pressure is vital for scientists and engineers who work with gases and liquids, and for outdoor enthusiasts, who may need to adjust their cooking methods when on mountains or high altitudes like those in Leadville, Colorado.