K (s) + ½Cl, (g) → KCI (s) AH° = – 437 kJ/moln 14. It is observed that the reaction producing KCl from its elements goes essentially to completion upon mixing at room temperature. Which of the following is a true statement about the thermodynamic favorability of the reaction above? A) The reaction is favorable and driven by an enthalpy change only. B) The reaction is unfavorable and driven by an entropy change only. C) The reaction is favorable and driven by both enthalpy and entropy changes. D) The reaction is unfavorable due to both enthalpy and entropy changes. Justify:
K (s) + ½Cl, (g) → KCI (s) AH° = – 437 kJ/moln 14. It is observed that the reaction producing KCl from its elements goes essentially to completion upon mixing at room temperature. Which of the following is a true statement about the thermodynamic favorability of the reaction above? A) The reaction is favorable and driven by an enthalpy change only. B) The reaction is unfavorable and driven by an entropy change only. C) The reaction is favorable and driven by both enthalpy and entropy changes. D) The reaction is unfavorable due to both enthalpy and entropy changes. Justify:
Chemistry
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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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Transcribed Image Text:K (s) + ½Cl, (g) → KCI (s)
AH° = – 437 kJ/molvn
rxn
14. It is observed that the reaction producing KCl from its elements goes essentially to completion upon
mixing at room temperature. Which of the following is a true statement about the thermodynamic
favorability of the reaction above?
A) The reaction is favorable and driven by an enthalpy change only.
B) The reaction is unfavorable and driven by an entropy change only.
C) The reaction is favorable and driven by both enthalpy and entropy changes.
D) The reaction is unfavorable due to both enthalpy and entropy changes.
Justify:
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