This reaction takes place at 486. °C and is NOT at equilibrium initially. The initial non-equilibrium pressures are given below the ingredients in the reaction. CO2 (g) + H₂ (g) = CO (g) + Initially 1 atm 1 atm 1 atm H₂O (g) 1 atm When equilibrium is established the equilibrium pressure of CO2 is 1. 81 atm. Find AG° for this reaction. Please notice temperature is in ºC. (A) 25. 8 kJ/mol (B) 29. 5 kJ/mol (C) 27.5 kJ/mol (D) 28. 4 kJ/mol (E) 24. 7 kJ/mol Hint: You know the initial non-equilibrium partial pressures and 1 equilibrium partial pressure. From that information you can fill out the ICE table. No unknowns (x) should be used. K. can then be calculated from the equilibrium row of the ICE table. Look over the example in the notes. Submit
This reaction takes place at 486. °C and is NOT at equilibrium initially. The initial non-equilibrium pressures are given below the ingredients in the reaction. CO2 (g) + H₂ (g) = CO (g) + Initially 1 atm 1 atm 1 atm H₂O (g) 1 atm When equilibrium is established the equilibrium pressure of CO2 is 1. 81 atm. Find AG° for this reaction. Please notice temperature is in ºC. (A) 25. 8 kJ/mol (B) 29. 5 kJ/mol (C) 27.5 kJ/mol (D) 28. 4 kJ/mol (E) 24. 7 kJ/mol Hint: You know the initial non-equilibrium partial pressures and 1 equilibrium partial pressure. From that information you can fill out the ICE table. No unknowns (x) should be used. K. can then be calculated from the equilibrium row of the ICE table. Look over the example in the notes. Submit
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 34A
Related questions
Question
![This reaction takes place at 486. °C and is NOT at equilibrium initially. The initial non-equilibrium
pressures are given below the ingredients in the reaction.
CO2 (g) +
H₂ (g)
=
CO (g)
+
Initially 1 atm
1 atm
1 atm
H₂O (g)
1 atm
When equilibrium is established the equilibrium pressure of CO2 is 1. 81 atm. Find AG° for this
reaction. Please notice temperature is in ºC.
(A) 25. 8 kJ/mol
(B) 29. 5 kJ/mol
(C) 27.5 kJ/mol
(D) 28. 4 kJ/mol
(E) 24. 7 kJ/mol
Hint: You know the initial non-equilibrium partial
pressures and 1 equilibrium partial pressure. From that
information you can fill out the ICE table. No unknowns
(x) should be used. K. can then be calculated from the
equilibrium row of the ICE table. Look over the example
in the notes.
Submit](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9966adb6-7e86-421b-a673-5883e55a3125%2F3fb70f4e-aff9-45e9-98f5-cfb695a27e85%2F4t0g1el_processed.jpeg&w=3840&q=75)
Transcribed Image Text:This reaction takes place at 486. °C and is NOT at equilibrium initially. The initial non-equilibrium
pressures are given below the ingredients in the reaction.
CO2 (g) +
H₂ (g)
=
CO (g)
+
Initially 1 atm
1 atm
1 atm
H₂O (g)
1 atm
When equilibrium is established the equilibrium pressure of CO2 is 1. 81 atm. Find AG° for this
reaction. Please notice temperature is in ºC.
(A) 25. 8 kJ/mol
(B) 29. 5 kJ/mol
(C) 27.5 kJ/mol
(D) 28. 4 kJ/mol
(E) 24. 7 kJ/mol
Hint: You know the initial non-equilibrium partial
pressures and 1 equilibrium partial pressure. From that
information you can fill out the ICE table. No unknowns
(x) should be used. K. can then be calculated from the
equilibrium row of the ICE table. Look over the example
in the notes.
Submit
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