### Equilibrium Constant and Pressure Calculation1. **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 \( \Delta G^\circ_{rxn} \).

The value of ∆G°f is -10.00 kJ/mol. The temperature of reaction is 298 K.

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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c
Consider the following reaction: A (g) + B(g) ↔ 2C(g) Kp = 0.0825 at 298 K Calculate ΔG (J/mol) at 25°C when P(A) = 1.50 atm, P(B) = 3.20 atm and P(C) = 4.00 atm Enter your answer with the correct number of sig figs, without any units. If you want to use scientific notation, use the #e# format.
https://www.webassign.net/blb12/a-table-c.pdf ^ | Just copy and paste this in the search bar into google
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