The enthalpy of vaporization of a certain liquid is found to be 14.4 kJ mol−1 at 180 K, its normal boiling point. The molar volumes of the liquid and the vapour at the boiling point are 115 cm3 mol−1 and 14.5 dm3 mol−1, respectively. (a) Use the Clapeyron equation to estimate dp/dT at the normal boiling point. (b) If the Clausius–Clapeyron equation is used instead to estimate dp/dT, what is the percentage error in the resulting value of dp/dT?

a) dp/dT = DvapS/DvapV = DvapH/Tb.DvapV = 14.4x103 J mol-1 ( 180 K)x(14.5x10-3– 1.15x10-4) m3…

Answered: The enthalpy of vaporization of a…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The enthalpy of vaporization of a certain liquid is found to be 14.4 kJ mol⁻¹ at 180 K, its normal boiling point. The molar volumes of the liquid and the vapour at the boiling point are 115 cm³ mol⁻¹ and 14.5 dm³ mol⁻¹, respectively. (a) Use the Clapeyron equation to estimate dp/dT at the normal boiling point. (b) If the Clausius–Clapeyron equation is used instead to estimate dp/dT, what is the percentage error in the resulting value of dp/dT?

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