The vapor pressure of methanol at 25 $\circ$ C is 123 Torr and its enthalpy of vaporization is 35.3 kJ.mol^-1.Estimate the normal boiling point of methanol.Assume the enthalpy of vaporization is independent of temperature.

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Quizplus · Accepted Answer

The normal boiling point is when the vapor pressure equals 1 atm (760 Torr). Using the Clausius-Clapeyron equation, we can estimate the boiling point. Given the vapor pressure at 25°C (298 K) is 123 Torr, and the enthalpy of vaporization is 35.3 kJ/mol, solving the equation gives approximately 342 K.

The Vapor Pressure of Methanol at 25 ∘\circ∘ C Is 123 Torr and Its Enthalpy of Vaporization Is

The Vapor Pressure of Methanol at 25^$\circ$C Is 123 Torr and Its Enthalpy of Vaporization Is