Die normale kookpunt van water is 100.0 °C en sy molêreverdampingsentalpie is 40.67 kJ/mol. Wat is die verandering in entropie (inJ/K) in die sisteem indien 39.3 gram stoom by 1 atm kondenseer omvloeistof te vorm by die normale kookpunt?The normal boiling point of water is 100.0 °C and its molar enthalpy ofvaporisation is 40.67 kJ/mol. What is the change in entropy (in J/K) in thesystem when 39.3 grams of steam at 1 atm condenses to a liquid at thenormal boiling point?

Given: The molar enthalpy of vaporization (Hvap∘) is 40.67 kJ/mol. The mass of steam is 39.3 g. The…

The normal boiling point of water is 100.0 °C and its molar enthalpy of vaporisation is 40.67 kJ/mol. What is the change in entropy (in J/K) in the system when 39.3 grams of steam at 1 atm condenses to a liquid at the normal boiling point?

The normal boiling point of water is 100.0 °C and its molar enthalpy of vaporisation is 40.67 kJ/mol. What is the change in entropy (in J/K) in the system when 39.3 grams of steam at 1 atm condenses to a liquid at the normal boiling point?

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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Question

Die normale kookpunt van water is 100.0 °C en sy molêre
verdampingsentalpie is 40.67 kJ/mol. Wat is die verandering in entropie (in
J/K) in die sisteem indien 39.3 gram stoom by 1 atm kondenseer om
vloeistof te vorm by die normale kookpunt?
The normal boiling point of water is 100.0 °C and its molar enthalpy of
vaporisation is 40.67 kJ/mol. What is the change in entropy (in J/K) in the
system when 39.3 grams of steam at 1 atm condenses to a liquid at the
normal boiling point?

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