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 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.
Chemistry for Engineering Students
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ISBN:9781337398909
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Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.101PAE: 10.101 Fluorine reacts with liquid water to form gaseous hydrogen fluoride and oxygen. (a) Write a...
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The decomposition of crystalline N2O5
N2O5(s)?2NO2(g)+12O(g)
is an example of a reaction that is
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.
Transcribed Image Text: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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