Calculate the entropy change of 47.7 g of steam that condenses to liquid water at 373.15 K. The heat of condensation for water is - 40.79 kJ/mol. (Enter your answer in J/K). Without doing further calculations, which of the following statements apply to the entropy change of the surroundings for the problem above? ΔSsurroundings will not change. ΔSsurroundings will be positive. |ΔSsurroundings| = |ΔSsteam| |ΔSsurroundings| < |ΔSsteam| ΔSsurroundings will be negative. |ΔSsurroundings| > |ΔSsteam|
Calculate the entropy change of 47.7 g of steam that condenses to liquid water at 373.15 K. The heat of condensation for water is - 40.79 kJ/mol. (Enter your answer in J/K). Without doing further calculations, which of the following statements apply to the entropy change of the surroundings for the problem above? ΔSsurroundings will not change. ΔSsurroundings will be positive. |ΔSsurroundings| = |ΔSsteam| |ΔSsurroundings| < |ΔSsteam| ΔSsurroundings will be negative. |ΔSsurroundings| > |ΔSsteam|
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter13: Spontaneous Processes And Thermodynamic Equilibrium
Section: Chapter Questions
Problem 25P
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Calculate the entropy change of 47.7 g of steam that condenses to liquid water at 373.15 K. The heat of condensation for water is - 40.79 kJ/mol. (Enter your answer in J/K).
Without doing further calculations, which of the following statements apply to the entropy change of the surroundings for the problem above?
ΔSsurroundings will not change.
ΔSsurroundings will be positive.
|ΔSsurroundings| = |ΔSsteam|
|ΔSsurroundings| < |ΔSsteam|
ΔSsurroundings will be negative.
|ΔSsurroundings| > |ΔSsteam|
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