Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. Substance M3O4(s) M3O4(s) 3M(s) + 2O₂(g) M(s) O₂(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? -10.00 AGTxn = Incorrect What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? 56.57 K = Incorrect AG°f(kJ/mol) -10.00 0 0 kJ/mol
Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. Substance M3O4(s) M3O4(s) 3M(s) + 2O₂(g) M(s) O₂(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? -10.00 AGTxn = Incorrect What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? 56.57 K = Incorrect AG°f(kJ/mol) -10.00 0 0 kJ/mol
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 92QRT
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What is the equilibrium pressure of O2(g) over M(s) at 298 K?
?O2= atm
![### Decomposition of a Metal Oxide into its Elements
Consider the decomposition of a metal oxide to its elements, where \( \text{M} \) represents a generic metal. The reaction is given as:
\[ \text{M}_3\text{O}_4 (\text{s}) \rightleftharpoons 3 \text{M} (\text{s}) + 2 \text{O}_2 (\text{g}) \]
#### Standard Gibbs Energy Change
To determine the standard change in Gibbs energy for the reaction in the forward direction, we need to refer to the standard Gibbs free energy of formation (\( \Delta G_f^\circ \)) for each substance involved. The table provided includes these values:
| Substance | \( \Delta G_f^\circ \) (kJ/mol) |
|-------------|-------------------------------|
| \( \text{M}_3\text{O}_4 (\text{s}) \) | -10.00 |
| \( \text{M} (\text{s}) \) | 0 |
| \( \text{O}_2 (\text{g}) \) | 0 |
What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?
\[
\Delta G_{\text{rxn}}^\circ = \boxed{-10.00} \, \text{kJ/mol}
\]
*Status: Incorrect*
#### Equilibrium Constant
Next, we determine the equilibrium constant (\( K \)) for this reaction at 298 K using the expression:
\[
\Delta G_{\text{rxn}}^\circ = -RT \ln K
\]
Given the value:
\[
K = \boxed{56.57}
\]
*Status: Incorrect*
### Explanation of Graphs/Diagrams
There are no additional graphs or diagrams included in this example. The information is presented in a textual format supplemented with a table of Gibbs free energy of formation values. The questions require calculating Gibbs free energy change and the equilibrium constant based on provided thermodynamic data.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f33cc2f-0221-41a8-a3a2-cc96bc7960a2%2F34f4f16e-08e7-4f03-a719-a79a79060e03%2Fw0ir2os_processed.png&w=3840&q=75)
Transcribed Image Text:### Decomposition of a Metal Oxide into its Elements
Consider the decomposition of a metal oxide to its elements, where \( \text{M} \) represents a generic metal. The reaction is given as:
\[ \text{M}_3\text{O}_4 (\text{s}) \rightleftharpoons 3 \text{M} (\text{s}) + 2 \text{O}_2 (\text{g}) \]
#### Standard Gibbs Energy Change
To determine the standard change in Gibbs energy for the reaction in the forward direction, we need to refer to the standard Gibbs free energy of formation (\( \Delta G_f^\circ \)) for each substance involved. The table provided includes these values:
| Substance | \( \Delta G_f^\circ \) (kJ/mol) |
|-------------|-------------------------------|
| \( \text{M}_3\text{O}_4 (\text{s}) \) | -10.00 |
| \( \text{M} (\text{s}) \) | 0 |
| \( \text{O}_2 (\text{g}) \) | 0 |
What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?
\[
\Delta G_{\text{rxn}}^\circ = \boxed{-10.00} \, \text{kJ/mol}
\]
*Status: Incorrect*
#### Equilibrium Constant
Next, we determine the equilibrium constant (\( K \)) for this reaction at 298 K using the expression:
\[
\Delta G_{\text{rxn}}^\circ = -RT \ln K
\]
Given the value:
\[
K = \boxed{56.57}
\]
*Status: Incorrect*
### Explanation of Graphs/Diagrams
There are no additional graphs or diagrams included in this example. The information is presented in a textual format supplemented with a table of Gibbs free energy of formation values. The questions require calculating Gibbs free energy change and the equilibrium constant based on provided thermodynamic data.
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