For the reaction N2(g) + 20,(g)→2NO,(g) AH° = 66.4 kJ and AS° =-121.6 J/K The equilibrium constant for this reaction at 314.0 K is Assume that AH° and AS° are independent of temperature.
For the reaction N2(g) + 20,(g)→2NO,(g) AH° = 66.4 kJ and AS° =-121.6 J/K The equilibrium constant for this reaction at 314.0 K is Assume that AH° and AS° are independent of temperature.
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Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.79QP: Use thermochemical data (Appendix C) to decide whether the equilibrium constant for the following...
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![to access important values if needed
For the reaction
N() + 20,(g)2NO,(g)
AH° = 66.4 kJ and AS° =-121.6 J/K
The equilibrium constant for this reaction at 314.0 K is
Assume that AH° and AS° are independent of temperature.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcdf080d6-723a-4d5e-ab30-2a8c95f72f87%2Fa6f9a5f9-bfb7-4780-a0ac-3178934a9b53%2Fueqxq1f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:to access important values if needed
For the reaction
N() + 20,(g)2NO,(g)
AH° = 66.4 kJ and AS° =-121.6 J/K
The equilibrium constant for this reaction at 314.0 K is
Assume that AH° and AS° are independent of temperature.
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