Consider the reaction.
This three-step mechanism is proposed.
a. Show that the mechanism sums to the overall reaction.
b. What is the rate law predicted by this mechanism?
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Principles of Chemistry: A Molecular Approach (3rd Edition)
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- Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forwardBecause carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?arrow_forward7-31 Here are equilibrium constants for several reactions. Which of them favor the formation of products, and which favor the formation of reactants? (a) (b) 32 (c) 4.5 (d) (e) 0.0032arrow_forward
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