5. At its normal boiling point (337.3 K), methanol (CH3OH) has AvapH = 25.79 kJ/mol, and thedensities of its liquid and vapor states at that temperature are 0.7486 g/mL and 0.0.001206g/mL, respectively.%3DData fromdT(a) Use the Clapeyron equation to determine the value of () for methanol at T = 337.3 K.dP.Report your answer in units of K/bar.(b) Use your result to estimate its boiling point (in K) at a pressure of 2 bars.3.

As per Clausius-Clapeyron equation, dPdT=∆HT∆V

5. At its normal boiling point (337.3 K), methanol (CH3OH) has AvapH = 25.79 kJ/mol, and the densities of its liquid and vapor states at that temperature are 0.7486 g/mL and 0.0.001206 g/mL, respectively. Data from (a) Use the Clapeyron equation to determine the value of for methanol at T = 337.3 K. dP, Report your answer in units of K/bar. (b) Use your result to estimate its boiling point (in K) at a pressure of 2 bars.

5. At its normal boiling point (337.3 K), methanol (CH3OH) has AvapH = 25.79 kJ/mol, and the densities of its liquid and vapor states at that temperature are 0.7486 g/mL and 0.0.001206 g/mL, respectively. Data from (a) Use the Clapeyron equation to determine the value of for methanol at T = 337.3 K. dP, Report your answer in units of K/bar. (b) Use your result to estimate its boiling point (in K) at a pressure of 2 bars.

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

Section: Chapter Questions

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

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