Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. AG°(kJ/mol) Substance M20(s) -10.00 M,0(s) = 2 M(s) + 0,(g) M(s) What is the standard change in Gibbs energy for the reaction, as written, in the O2(g) forward direction? kJ/mol
Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. AG°(kJ/mol) Substance M20(s) -10.00 M,0(s) = 2 M(s) + 0,(g) M(s) What is the standard change in Gibbs energy for the reaction, as written, in the O2(g) forward direction? kJ/mol
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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![### Equilibrium Constant and Pressure Calculation
1. **Equilibrium Constant (K)**
_What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K?_
\( K = \)
[Input area for numerical value]
2. **Equilibrium Pressure**
_What is the equilibrium pressure of \( \text{O}_2(g) \) over \( \text{M}(s) \) at 298 K?_
\( P_{\text{O}_2} = \)
[Input area for numerical value] atm
**Note**: The equations or expressions for K and \( P_{\text{O}_2} \) should be derived from the specific reaction conditions and stoichiometry. Ensure to provide proper context and calculations as necessary.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff32c3ee5-84ad-4b8f-a5ee-9f2098075ae5%2F1f6c7580-4b39-4aa3-bc9c-43c02dee7acc%2Fnod3u7j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Equilibrium Constant and Pressure Calculation
1. **Equilibrium Constant (K)**
_What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K?_
\( K = \)
[Input area for numerical value]
2. **Equilibrium Pressure**
_What is the equilibrium pressure of \( \text{O}_2(g) \) over \( \text{M}(s) \) at 298 K?_
\( P_{\text{O}_2} = \)
[Input area for numerical value] atm
**Note**: The equations or expressions for K and \( P_{\text{O}_2} \) should be derived from the specific reaction conditions and stoichiometry. Ensure to provide proper context and calculations as necessary.
![**Title: Thermodynamics of Metal Oxide Decomposition**
**Introduction**
Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. The chemical reaction is as follows:
\[ \text{M}_2\text{O}(s) \rightleftharpoons 2\text{M}(s) + \frac{1}{2}\text{O}_2(g) \]
**Question**
What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?
**Data Table**
The table below provides the standard Gibbs energy of formation (\( \Delta G^\circ_f \)) for the substances involved in the reaction:
| Substance | \( \Delta G^\circ_f \) (kJ/mol) |
|-----------|---------------------------|
| \(\text{M}_2\text{O}(s)\) | \(-10.00\) |
| \(\text{M}(s)\) | \(0\) |
| \(\text{O}_2(g)\) | \(0\) |
**Calculation**
The standard change in Gibbs energy for the reaction (\( \Delta G^\circ_{rxn} \)) can be calculated using the formula:
\[
\Delta G^\circ_{rxn} = \left( \sum \Delta G^\circ_f \text{(products)} \right) - \left( \sum \Delta G^\circ_f \text{(reactants)} \right)
\]
**Result**
\[ \Delta G^\circ_{rxn} = \boxed{kJ/mol} \]
**Note:** Complete the calculation by substituting the given values into the formula to find the numerical result for \( \Delta G^\circ_{rxn} \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff32c3ee5-84ad-4b8f-a5ee-9f2098075ae5%2F1f6c7580-4b39-4aa3-bc9c-43c02dee7acc%2Ftc9w1rg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Thermodynamics of Metal Oxide Decomposition**
**Introduction**
Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. The chemical reaction is as follows:
\[ \text{M}_2\text{O}(s) \rightleftharpoons 2\text{M}(s) + \frac{1}{2}\text{O}_2(g) \]
**Question**
What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?
**Data Table**
The table below provides the standard Gibbs energy of formation (\( \Delta G^\circ_f \)) for the substances involved in the reaction:
| Substance | \( \Delta G^\circ_f \) (kJ/mol) |
|-----------|---------------------------|
| \(\text{M}_2\text{O}(s)\) | \(-10.00\) |
| \(\text{M}(s)\) | \(0\) |
| \(\text{O}_2(g)\) | \(0\) |
**Calculation**
The standard change in Gibbs energy for the reaction (\( \Delta G^\circ_{rxn} \)) can be calculated using the formula:
\[
\Delta G^\circ_{rxn} = \left( \sum \Delta G^\circ_f \text{(products)} \right) - \left( \sum \Delta G^\circ_f \text{(reactants)} \right)
\]
**Result**
\[ \Delta G^\circ_{rxn} = \boxed{kJ/mol} \]
**Note:** Complete the calculation by substituting the given values into the formula to find the numerical result for \( \Delta G^\circ_{rxn} \).
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