[1] Given: CH,(g) + H2O(g) CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol. Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
[1] Given: CH,(g) + H2O(g) CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol. Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
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 10.50PAE: For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then...
Related questions
Question
I need help with these practice problems thank you!
![AG°= - RT In Keq and
In Keg =-
or Keg = 04G®/RT
[1] Given: CH4(g) + H2O(g) → CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol.
Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
[2] [a] The forward reaction is spontaneous for a particular reversible reaction. What can you conclude about the reverse
reaction?
[b] What does the sign of the free energy have to be such that a reaction is spontaneous?
AG =
[c] [i] Under what conditions of enthalpy and entropy change is a reaction always spontaneous? AH=,
[ii] Under what conditions of enthalpy and entropy change is a reaction never spontaneous?
AS =
ΔΗ-
AS =
[d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a high
temperature or a low temperature?
[e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low
temperature
more likely to lead to a spontaneous reaction?
[3] For the reaction C,H2(g) + 2H2(g) ) → C2H6(g), AG°(C,H2) = +209.2kJ/mol and AG°(C2H6) = -32.89 kJ/mol at
25.0°C. What is Keg for this reaction?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60cf892a-bc21-4928-b8d7-b5b696620db4%2F7e342af8-1ee4-4a5e-b7f3-e2ca5887f413%2Fy9rl6pe_processed.jpeg&w=3840&q=75)
Transcribed Image Text:AG°= - RT In Keq and
In Keg =-
or Keg = 04G®/RT
[1] Given: CH4(g) + H2O(g) → CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol.
Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
[2] [a] The forward reaction is spontaneous for a particular reversible reaction. What can you conclude about the reverse
reaction?
[b] What does the sign of the free energy have to be such that a reaction is spontaneous?
AG =
[c] [i] Under what conditions of enthalpy and entropy change is a reaction always spontaneous? AH=,
[ii] Under what conditions of enthalpy and entropy change is a reaction never spontaneous?
AS =
ΔΗ-
AS =
[d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a high
temperature or a low temperature?
[e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low
temperature
more likely to lead to a spontaneous reaction?
[3] For the reaction C,H2(g) + 2H2(g) ) → C2H6(g), AG°(C,H2) = +209.2kJ/mol and AG°(C2H6) = -32.89 kJ/mol at
25.0°C. What is Keg for this reaction?
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
![Chemistry for Engineering Students](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry for Engineering Students](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry: An Atoms First Approach](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning