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Lecture 24 Chemical equilibrium Equilibrium constant Dissociation of diatomic molecule Heterophase reactions

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Gibbs free energy change Chemical reaction Gibbs free energy change In equilibrium the Gibbs free energy change is zero, therefore

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Activity Chemical potential with gives

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Equilibrium constant Defining standard free energy change for the reaction And equilibrium constant for the reaction gives

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Diatomic molecule Equilibrium constant for the reaction Chemical potential for monoatomic and diatomic gas

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Diatomic molecule - equilibrium constant

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Equilibrium pressure expression Equilibrium constant for the reaction Increasing temperature increasing dissociation The major parameter controlling dissociation is D e /kT

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Heterophase reactions Consider a C =1 (activity of the pure solid phase) K a can be obtained from statistical mechanics (e.q., Einstein model of C solid) or from experiment via

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Review Of Statistical Mechanics Continued

Review Of Statistical Mechanics Continued

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