What is the standard entropy for the given equation? Use the table as a reference.  2. What is the standard Gibbs energy for the given reaction? Is the reaction spontaneous or nonspontaneous? 3. What is the equilibrium constant for the reaction at standard conditions? (Use R = 8.31447 J/mol∙K)

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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.154QP
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1. What is the standard entropy for the given equation? Use the table as a reference. 
2. What is the standard Gibbs energy for the given reaction? Is the reaction spontaneous or nonspontaneous?
3. What is the equilibrium constant for the reaction at standard conditions? (Use R = 8.31447 J/mol∙K)

7. For items within problem 7, below is the given reaction occurring at 298.15K:
2 NO(g) + O₂(g) → 2NO₂(g)
Transcribed Image Text:7. For items within problem 7, below is the given reaction occurring at 298.15K: 2 NO(g) + O₂(g) → 2NO₂(g)
N₂ (g)
O₂ (g)
H₂(g)
NO (g)
NO₂ (g)
N2O4 (g)
H₂O(g)
So
J/mol K
191.5
205.0
130.6
210.7
240.0
304.2
188.8
S (g)
H₂S (g)
SO₂ (g)
SO3 (g)
H₂SO4 (1)
H₂SO4 (aq)
H₂O (1)
Sº
J/mol K
167.8
205.6
248.2
256.8
156.9
20.1
69.9
Transcribed Image Text:N₂ (g) O₂ (g) H₂(g) NO (g) NO₂ (g) N2O4 (g) H₂O(g) So J/mol K 191.5 205.0 130.6 210.7 240.0 304.2 188.8 S (g) H₂S (g) SO₂ (g) SO3 (g) H₂SO4 (1) H₂SO4 (aq) H₂O (1) Sº J/mol K 167.8 205.6 248.2 256.8 156.9 20.1 69.9
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