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Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2 M(s) +20₂(g) →→→ M₂O4(s) For this reaction, AH = -4.961 kJ/mol and A.Sixn = 12.12 J/(mol-K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction?

Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2 M(s) +20₂(g) →→→ M₂O4(s) For this reaction, AH = -4.961 kJ/mol and A.Sixn = 12.12 J/(mol-K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction?

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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
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Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2M(s) +20₂(g) →→ M₂O4(s) - For this reaction, AH = -4.961 kJ/mol and ASixn = 12.12 J/(mol-K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction? AGrxn= What is the equilibrium constant of this reaction at 298 K? Kp = What is the equilibrium pressure of O₂(g) over M(s) at 298 K? kJ/mol
Transcribed Image Text:Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2M(s) +20₂(g) →→ M₂O4(s) - For this reaction, AH = -4.961 kJ/mol and ASixn = 12.12 J/(mol-K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction? AGrxn= What is the equilibrium constant of this reaction at 298 K? Kp = What is the equilibrium pressure of O₂(g) over M(s) at 298 K? kJ/mol
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