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The conventional equilibrium considerations do not apply when a reaction is being driven by light absorption. Thus the steady state concentrations of products and reactions might differ significantly from equilibrium values. For instance, suppose the reaction A B is driven by light absorption and that its rate is la, but the reverse reaction B A is bimolecular and second order with a rate k[B]2. What is the stationary state concentration of B? Why does the photostationary state differ from the equilibrium state?

The conventional equilibrium considerations do not apply when a reaction is being driven by light absorption. Thus the steady state concentrations of products and reactions might differ significantly from equilibrium values. For instance, suppose the reaction A B is driven by light absorption and that its rate is la, but the reverse reaction B A is bimolecular and second order with a rate k[B]2. What is the stationary state concentration of B? Why does the photostationary state differ from the equilibrium state?

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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The conventional equilibrium considerations do not apply when a reaction is being driven by light absorption. Thus the steady state concentrations of products and reactions might differ significantly from equilibrium values. For instance, suppose the reaction A B is driven by light absorption and that its rate is la, but the reverse reaction B A is bimolecular and second order with a rate k[B]2. What is the stationary state concentration of B? Why does the photostationary state differ from the equilibrium state?
Transcribed Image Text:The conventional equilibrium considerations do not apply when a reaction is being driven by light absorption. Thus the steady state concentrations of products and reactions might differ significantly from equilibrium values. For instance, suppose the reaction A B is driven by light absorption and that its rate is la, but the reverse reaction B A is bimolecular and second order with a rate k[B]2. What is the stationary state concentration of B? Why does the photostationary state differ from the equilibrium state?
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