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Chemistry & Chemical Reactivity

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

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

The vapor pressure of pure heptane is 361.5 mm Hg at 75.0 °C and its normal boiling point is 98.4 °C. Use the Clausius-Clapeyron equation (page 512) to determine the enthalpy of vaporization of heptane.

Interpretation Introduction

Interpretation: The enthalpy of vaporization of heptane has to be determined using Clausius-Clapeyron equation.

Concept introduction:

  • Enthalpy of vaporization (ΔHvap ) is the amount of energy required to change one mole of a substance from the liquid phase to the gas phase at constant temperature and pressure.
  • Clausius-Clapeyron equation is used to estimate the vapor pressure at another temperature, if the vapor pressure is known at some temperature, and if the enthalpy of vaporization is known.

            ln(P2P1)=ΔHvapR(1T2-1T1)

    ΔHvap is the enthalpy of vaporization.

  R is the gas constant (8.3145Jmol1K1 )

  P1andP2 are the vapor pressures at two temperatures T1andT2.

Explanation

Given data:

Vaporpressureofheptane=361.5mmHgT1=98.4°C=371.55KT2=75°C=348.15K

Clausius-Clapeyron equation is used to estimate the vapor pressure at another temperature, if the vapor pressure is known at some temperature, and if the enthalpy of vaporization is known.

            ln(P2P1)=ΔHvapR(1T2-1T1)

Substituting the given values of pressure and temperatures in the above equation,

            ln(361

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