The normal boiling point of Br2(l) is 58.8 °C, and itsmolar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol.(a) When Br2(l) boils at its normal boiling point, does itsentropy increase or decrease? (b) Calculate the value of ΔSwhen 1.00 mol of Br2(l) is vaporized at 58.8 °C.

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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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The normal boiling point of Br₂(l) is 58.8 °C, and its
molar enthalpy of vaporization is ΔH_vap = 29.6 kJ/mol.
(a) When Br₂(l) boils at its normal boiling point, does its
entropy increase or decrease? (b) Calculate the value of ΔS
when 1.00 mol of Br₂(l) is vaporized at 58.8 °C.

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