The normal boiling point for acetone is 56.5^∘ C. At an...

The normal boiling point for acetone is $56.5^{\circ} \mathrm{C}$. At an elevation of $5300 \mathrm{ft}$ the atmospheric pressure is $630 .$ torr. What would be the boiling point of acetone $\left(\Delta H_{\text {vap }}=32.0 \mathrm{~kJ} / \mathrm{mol}\right)$ at this elevation? What would be the vapor pressure of acetone at $25.0^{\circ} \mathrm{C}$ at this elevation?

Key Concepts

Enthalpy of Vaporization

Enthalpy of vaporization is the amount of energy required to convert one mole of a liquid into vapor at a constant temperature and pressure. It is a critical parameter in the Clausius-Clapeyron equation, helping to quantify the relationship between temperature and vapor pressure during phase transitions.

Boiling Point and Pressure Relationship

The boiling point of a liquid is defined as the temperature at which its vapor pressure equals the surrounding atmospheric pressure. When atmospheric pressure changes, so does the boiling point. This concept is widely used in understanding how substances behave at high altitudes where atmospheric pressure is lower.

Clausius-Clapeyron Equation

This equation relates the vapor pressure of a substance to its temperature and enthalpy of vaporization. It allows us to predict the change in vapor pressure with a change in temperature by integrating the differential form, and it is crucial for calculating boiling points and vapor pressures under different atmospheric pressures.

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid (or solid) phase at a given temperature. It reflects the tendency of molecules to escape from the liquid and is a key variable in determining whether a liquid will boil at a given temperature under specific pressure conditions.

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