## Problem 19.23 - Enhanced - with Feedback**The normal boiling point of Br₂(l) is 58.8 °C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol.**### Part AWhen Br₂(l) boils at its normal boiling point, does its entropy increase or decrease?- [ ] increase- [ ] decrease*Submit button followed by Request Answer button*### Part BCalculate the value of ΔS when 7.00 mol of Br₂(l) is vaporized at 58.8 °C.**Express your answer in joules per kelvin to three significant figures.**ΔS = [Input Box] J/K*Submit button followed by Request Answer button*

we have to calculate the change in entropy

The normal boiling point of Br₂ (1) is 58.8 °C, and its molar enthalpy of vaporization is AHvap = 29.6 kJ/mol Part A When Br₂ (1) boils at its normal boiling point, does its entropy increase or decrease? increase decrease Submit Part B Calculate the value of AS when 7.00 mol of Br₂ (1) is vaporized at 58.8 °C. Express your answer in joules per kelvin to three significant figures. ID ΑΣΦ AS = Request Answer Submit Request Answer ? J/K

The normal boiling point of Br₂ (1) is 58.8 °C, and its molar enthalpy of vaporization is AHvap = 29.6 kJ/mol Part A When Br₂ (1) boils at its normal boiling point, does its entropy increase or decrease? increase decrease Submit Part B Calculate the value of AS when 7.00 mol of Br₂ (1) is vaporized at 58.8 °C. Express your answer in joules per kelvin to three significant figures. ID ΑΣΦ AS = Request Answer Submit Request Answer ? J/K

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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