3. The equilibrium constant for the reaction: 250:(8) + O:(8) = 2s0,(8) is 2.8 x 10' at 25.0°C. a. Determine the Free Gibb's Energy in kJ/mol. b. Using the data provided below, determine the enthalpy of reaction (k)/mol) and entropy of reaction (J/mol K) Substance SO:() O:(8) AH, (kl/mol) S' (J/Kmol) c. Determine the entropy for the surroundings in J/mol K at 25.0°C. (3)*Os -296.4 -395.2 248.5 205.0 256.2 d. Determine the entropy of the universe in J/mol K at 25.0°C. e. Is the reaction spontaneous at 25.0°C? Explain your answer using the information calculated in part a and part d.
3. The equilibrium constant for the reaction: 250:(8) + O:(8) = 2s0,(8) is 2.8 x 10' at 25.0°C. a. Determine the Free Gibb's Energy in kJ/mol. b. Using the data provided below, determine the enthalpy of reaction (k)/mol) and entropy of reaction (J/mol K) Substance SO:() O:(8) AH, (kl/mol) S' (J/Kmol) c. Determine the entropy for the surroundings in J/mol K at 25.0°C. (3)*Os -296.4 -395.2 248.5 205.0 256.2 d. Determine the entropy of the universe in J/mol K at 25.0°C. e. Is the reaction spontaneous at 25.0°C? Explain your answer using the information calculated in part a and part d.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.104PAE: 10.104 (a) When a chemical bond forms, what happens to the entropy of the system? (b)...
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Just need help with D and E of question
Transcribed Image Text:3. The equilibrium constant for the reaction:
250:(g) + O:(g) = 2so:(g)
is 2.8 x 10° at 25.0°c.
a. Determine the Free Gibb's Energy in kJ/mol.
b. Using the data provided below, determine the enthalpy of reaction (kJ/mol) and entropy of
reaction (J/mol K)
Substance
SO:(g)
0:(g)
SO:(g)
AH; (kl/mol)
S U/Kmol)
c. Determine the entropy for the surroundings in J/mol K at 25.0°C.
-296.4
-395.2
248.5
205.0
256.2
d. Determine the entropy of the universe in J/mol K at 25.0°C.
e. Is the reaction spontaneous at 25.0°C? Explain your answer using the information calculated
in part a and part d.
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