The vapor pressure of cyclohexane at 61°C is 0.527 atm. If the molar heat of evaporation of this compound is 35.9 kJ/mol, what is the normal boiling point of cyclohexane in °C?

Question

15-10-2024
Chemistry

High School

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The vapor pressure of cyclohexane at 61°C is 0.527 atm. If the molar heat of evaporation of this compound is 35.9 kJ/mol, what is the normal boiling point of cyclohexane in °C?

Answer :

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akriti3545 akriti3545 · Answer 1 · 2025-02-16T16:14:50-05:00

Final answer:

The normal boiling point of Cyclohexane is the temperature at which its vapor pressure equals 1 atmosphere. Using the Clausius Clapeyron Equation, we can calculate the normal boiling point to be approximately 80°C.

Explanation:

The normal boiling point of a substance is the temperature at which the vapor pressure equals 1 atmosphere. Thus, to find the normal boiling point of Cyclohexane, we have to calculate for the temperature where its vapor pressure is 1 atm. We can make use of the Clausius Clapeyron equation for this problem:

ΔvapH= -R(lnP2 - lnP1) / (1/T2 - 1/T1)

Where P1 is the initial pressure (0.527 atm), P2 is the final pressure (1 atm), T1 is the initial temp in Kelvin (334 K), T2 is the unknown final temperature, and R is the gas constant (8.314 x [tex]10^-3[/tex] kJ/K•mol).

Solving for T2 gives us 353 K, which is approximately 80°C when converted from Kelvin to Celsius.

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