Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074



Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Estimate the vapor pressure of ethanol at 37 °C using thermodynamic data. Express the result in millimeters of mercury.

Interpretation Introduction


The vapour pressure of ethanol at 37 °C should be estimated using thermodynamic data which then has to be expressed in millimeters of mercury.

Concept introduction:

The vapor pressure of a substance is related to its enthalpy of vaporisation by the



Here, p1 and p2 are the vapour pressures at two different temperatures T1 and T2.

This equation is known as Clausius-Clapeyron equation and is used to estimate the vapour pressure of a substance at a particular temperature.


The vapor pressure of ethanol at 37 °C is calculated below.

The Appendix L referred for the values of standard enthalpies of ethanol to calculate the value of ΔHvap.

The given reaction is,


The ΔHvap for the above reaction is,

ΔHvap=(235.3 kJ/mol)(277.0 kJ/mol)=41.7 kJ/mol=41700 J/mol

The normal boling point of ethanol is 78 °C under the standard condition of pressure of 760 mmHg.


The value of T1 is,

T1=37+273=310 K

The value of T2 is,

T2=78+273=351 K

The value of p2 is 760 mmHg

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