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The molar enthalpy of vaporization of ethanol is AvapH = 42.3 kJ/mol at its normal boiling point of 351.5 K. (a) Determine its molar entropy of vaporization at the boiling point, AvapS, in J/K. (b) The values of Cp for liquid and for gaseous ethanol for 300 < T< 400 are 112.4 and 70.85 J/mol-K, respectively. Use this information to estimate AvapH (in kJ/mol) at T = 320 K, assuming that the heat capacities of the liquid and gaseous states are constant over this temperature range. Hint: Construct a multi-step process that includes vaporization at 320 K, but includes a step with vaporization at Tvap. Is this enthalpy of vaporization larger or smaller in magnitude from the standard value?

The molar enthalpy of vaporization of ethanol is AvapH = 42.3 kJ/mol at its normal boiling point of 351.5 K. (a) Determine its molar entropy of vaporization at the boiling point, AvapS, in J/K. (b) The values of Cp for liquid and for gaseous ethanol for 300 < T< 400 are 112.4 and 70.85 J/mol-K, respectively. Use this information to estimate AvapH (in kJ/mol) at T = 320 K, assuming that the heat capacities of the liquid and gaseous states are constant over this temperature range. Hint: Construct a multi-step process that includes vaporization at 320 K, but includes a step with vaporization at Tvap. Is this enthalpy of vaporization larger or smaller in magnitude from the standard value?

Chemistry
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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The molar enthalpy of vaporization of ethanol is AvapH = 42.3 kJ/mol at its normal boiling point of 351.5 K. (a) Determine its molar entropy of vaporization at the boiling point, AvapS, in J/K. (b) The values of Cp for liquid and for gaseous ethanol for 300 < T< 400 are 112.4 and 70.85 J/mol-K, respectively. Use this information to estimate AvapH (in kJ/mol) at T = 320 K, assuming that the heat capacities of the liquid and gaseous states are constant over this temperature range. Hint: Construct a multi-step process that includes vaporization at 320 K, but includes a step with vaporization at Tvap. Is this enthalpy of vaporization larger or smaller in magnitude from the standard value?
Transcribed Image Text:The molar enthalpy of vaporization of ethanol is AvapH = 42.3 kJ/mol at its normal boiling point of 351.5 K. (a) Determine its molar entropy of vaporization at the boiling point, AvapS, in J/K. (b) The values of Cp for liquid and for gaseous ethanol for 300 < T< 400 are 112.4 and 70.85 J/mol-K, respectively. Use this information to estimate AvapH (in kJ/mol) at T = 320 K, assuming that the heat capacities of the liquid and gaseous states are constant over this temperature range. Hint: Construct a multi-step process that includes vaporization at 320 K, but includes a step with vaporization at Tvap. Is this enthalpy of vaporization larger or smaller in magnitude from the standard value?
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To determine the molar entropy of vaporization of ethanol at the boiling point given that the boiling point of ethanol is 351.5 K and the enthalpy of vaporization is 42.3 kJ/mol. 

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