The vapor pressure of ethanol, C2 H5 OH, at 50.0 ^∘ C is 233 mm Hg, and its normal boiling poin

step 1 Hi guys, let's solve question 33. The molar enthalpy of vaporization can be determined by using

The vapor pressure of ethanol, C2 H5 OH, at 50.0 ^∘ C is 233...

The vapor pressure of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$, at $50.0{ }^{\circ} \mathrm{C}$ is $233 \mathrm{~mm} \mathrm{Hg}$, and its normal boiling point at $1 \mathrm{~atm}$ is $78.3^{\circ} \mathrm{C} .$ Calculate the $\Delta H_{\mathrm{vap}}$ of ethanol.

Key Concepts

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (liquid or solid) at a given temperature in a closed system. It is a measure of a substance's tendency to evaporate, and it increases with temperature.

Enthalpy of Vaporization

Enthalpy of vaporization is the amount of heat required to convert one mole of a liquid into a vapor at constant temperature and pressure. It reflects the energy needed to overcome intermolecular forces during the phase transition from liquid to gas.

Clausius-Clapeyron Equation

The Clausius-Clapeyron equation is a relation that describes how the vapor pressure of a substance changes with temperature. It is used to connect the vapor pressure at different temperatures with the enthalpy of vaporization, allowing for the calculation of thermodynamic properties related to phase changes.

Normal Boiling Point

The normal boiling point is the temperature at which the vapor pressure of a liquid is equal to the ambient pressure, typically 1 atm. It serves as a standard reference point to understand and compare the boiling behavior of different substances.

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