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= 3. Using the free energy profile for a simple one-step reaction, show that at equilibrium Kp = Kforward/kreverse, where kforward and kreverse, are the rate constants for the forward and reverse -RT In(Kp) and represent kforward and kreverse using reactions. Hint: Use the relationship AG the Arrhenius equation (k = Ae-Ea /RT). Ea (forward) Reactants = AGO Ea (reverse) Reaction coordinate Products

= 3. Using the free energy profile for a simple one-step reaction, show that at equilibrium Kp = Kforward/kreverse, where kforward and kreverse, are the rate constants for the forward and reverse -RT In(Kp) and represent kforward and kreverse using reactions. Hint: Use the relationship AG the Arrhenius equation (k = Ae-Ea /RT). Ea (forward) Reactants = AGO Ea (reverse) Reaction coordinate Products

Chemistry
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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= 3. Using the free energy profile for a simple one-step reaction, show that at equilibrium Kp kforward/kreverse, where kforward and kreverse, are the rate constants for the forward and reverse reactions. Hint: Use the relationship AGⓇ -RT In(Kp) and represent kforward and kreverse using the Arrhenius equation (k G /RT). Ae-Ea /RT Ea (forward) Reactants = AGO Ea (reverse) Reaction coordinate Products
Transcribed Image Text:= 3. Using the free energy profile for a simple one-step reaction, show that at equilibrium Kp kforward/kreverse, where kforward and kreverse, are the rate constants for the forward and reverse reactions. Hint: Use the relationship AGⓇ -RT In(Kp) and represent kforward and kreverse using the Arrhenius equation (k G /RT). Ae-Ea /RT Ea (forward) Reactants = AGO Ea (reverse) Reaction coordinate Products
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Step 1: Defining activation energy

Answer:

Activation energy is the minimum energy that reactant particles require to form the product. It's an energy barrier that reactant particles need to overcome in order to form the product.

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