The decomposition of crystalline N2O5N2O5(s)?2NO2(g)+12O(g)is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ?C we have the following values for the standard state enthalpy and free energy changes of the reaction:Delta H = +109.6 kJ/molDelta Standard Gibbs Free Energy = -30.5 kJ/mol C) Calculate delta U for this reaction at 25 C. The decomposition of crystalline N¿O5NeOs(S)→ 2NO2(g) + 어(미)is an example of a reaction that is thermodynamically favored eventhough it absorbs heat. At 25 °C we have the following values for thestandard state enthalpy and free energy changes of the reaction:AH° = +109.6 kJ/molAG° = -30.5 kJ/mol(a) Calculate AS° at 25 °C.(b) Why is the entropy change so favorable for this reaction?(c) Calculate AU° for this reaction at 25 °C.(d) Why is AH° greater than AU?

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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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The decomposition of crystalline N2O5

N2O5(s)?2NO2(g)+12O(g)

is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ?C we have the following values for the standard state enthalpy and free energy changes of the reaction:

Delta H = +109.6 kJ/mol

Delta Standard Gibbs Free Energy = -30.5 kJ/mol

C) Calculate delta U for this reaction at 25 C.

The decomposition of crystalline N¿O5
NeOs(S)→ 2NO2(g) + 어(미)
is an example of a reaction that is thermodynamically favored even
though it absorbs heat. At 25 °C we have the following values for the
standard state enthalpy and free energy changes of the reaction:
AH° = +109.6 kJ/mol
AG° = -30.5 kJ/mol
(a) Calculate AS° at 25 °C.
(b) Why is the entropy change so favorable for this reaction?
(c) Calculate AU° for this reaction at 25 °C.
(d) Why is AH° greater than AU?

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