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Consider the following gas-phase reaction: 2 SO 3(g) 2 SO₂(g) + O₂(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG° = 0) and choose whether A>Gº will increase, decrease, or not change with increasing temperature from the pulldown menu. To = K, and AG° will ---Select--- with increasing temperature. For each of the temperatures listed below calculate AG for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of To). (a) At T = 519 K AG° = (b) At T = 1037 K AG° = (c) At T = 1556 K AG⁰ kJ/mol, and the reaction is ---Select--- kJ/mol, and the reaction is ---Select--- kJ/mol, and the reaction is ---Select--- ✓under standard conditions. ✓under standard conditions. ✓under standard conditions.

Consider the following gas-phase reaction: 2 SO 3(g) 2 SO₂(g) + O₂(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG° = 0) and choose whether A>Gº will increase, decrease, or not change with increasing temperature from the pulldown menu. To = K, and AG° will ---Select--- with increasing temperature. For each of the temperatures listed below calculate AG for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of To). (a) At T = 519 K AG° = (b) At T = 1037 K AG° = (c) At T = 1556 K AG⁰ kJ/mol, and the reaction is ---Select--- kJ/mol, and the reaction is ---Select--- kJ/mol, and the reaction is ---Select--- ✓under standard conditions. ✓under standard conditions. ✓under standard conditions.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider the following gas-phase reaction: Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG° = 0) and choose whether A>Gº will increase, decrease, or not change with increasing temperature from the pulldown menu. To = K, and AG° will --Select--- with increasing temperature. For each of the temperatures listed below calculate AGº for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of To). (a) At T = 519 K AG° = 2 SO 3(g) 2 50₂(g) + O₂(g) (b) At T = 1037 K AG° = (c) At T = 1556 K AG⁰ = kJ/mol, and the reaction is ---Select--- kJ/mol, and the reaction is --Select--- kJ/mol, and the reaction is ---Select--- ✓ under standard conditions. ✓ under standard conditions. ✓ under standard conditions.
Transcribed Image Text:Consider the following gas-phase reaction: Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG° = 0) and choose whether A>Gº will increase, decrease, or not change with increasing temperature from the pulldown menu. To = K, and AG° will --Select--- with increasing temperature. For each of the temperatures listed below calculate AGº for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of To). (a) At T = 519 K AG° = 2 SO 3(g) 2 50₂(g) + O₂(g) (b) At T = 1037 K AG° = (c) At T = 1556 K AG⁰ = kJ/mol, and the reaction is ---Select--- kJ/mol, and the reaction is --Select--- kJ/mol, and the reaction is ---Select--- ✓ under standard conditions. ✓ under standard conditions. ✓ under standard conditions.
Expert Solution
Step 1

According to the criteria of spontaneity, the change in entropy is positive and the change in Gibb free energy is negative for a spontaneous process.

The reverse is true for a non-spontaneous process. Change in Gibbs free energy is zero for a process at equilibrium.

 

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