For the reaction at 298 K, the values of Δ°H and Δ°S are -67.8 kJ and -186.6 J/K*mol respectively. 2NO2(g) <-> N2)4(g) a) What is the value of Δ°G at 298K? Show work b.) Assuming Δ°H and Δ°S do not depend on temperature, at what temperature is Δ°G=0? Show work c.) Is Δ°G negative above this temperature or below this temperature?
For the reaction at 298 K, the values of Δ°H and Δ°S are -67.8 kJ and -186.6 J/K*mol respectively. 2NO2(g) <-> N2)4(g) a) What is the value of Δ°G at 298K? Show work b.) Assuming Δ°H and Δ°S do not depend on temperature, at what temperature is Δ°G=0? Show work c.) Is Δ°G negative above this temperature or below this temperature?
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.90QP
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For the reaction at 298 K, the values of Δ°H and Δ°S are -67.8 kJ and -186.6 J/K*mol respectively.
2NO2(g) <-> N2)4(g)
a) What is the value of Δ°G at 298K? Show work
b.) Assuming Δ°H and Δ°S do not depend on temperature, at what temperature is Δ°G=0? Show work
c.) Is Δ°G negative above this temperature or below this temperature?
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