A reaction is observed to proceed with a rate constant of 1000s -1 at 50 ̊C. At 70 ̊C thereaction is found to have a rate constant of 4000s -1 . Assuming that A is temperature-independent, what is the activation barrier for this reaction?2. Most of the medications that we ingest are removed from our bodies via a first orderprocess. It is the aim of the physician to keep the concentration of medication (in ourbody) more or less constant over the treatment period. If a 10% variation inconcentration is the largest acceptable swing, and if the patient is required to take twodoses of the medication per day (i.e. once every 12 hours), what is the largest acceptablerate constant for the disappearance of the medication and what is the associated half-life?

Consider the mechanism. step 1: step 2: overall: Which species is an intermediate? O AB A B3 B2 A + B₂ → AB + B₂ 2 2B₂ B AB + B B3 + A B3 + B Which species is a catalyst? B3 AB B₁ 2 B A

Part A MISSED THIS? Read Section 15.5 (Pages 650 - 656), 15.7 (Pages 661 - 666) .Suppose that a catalyst lowers the activation barrier of a reaction from 123 kJ/mol to 55 kJ/mol. By what factor would you expect the reaction rate to increase at 25.00 ° C? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are identical.) Express your answer to two significant figures. > View Available Hint(s) ? |X| X•10n k2 1.03 • 1013 k1 Submit Previous Answers X Incorrect; Try Again; One attempt remaining Since the reaction rate is directly proportional to the rate constant, apply the Arrhenius equation to the two different activation energies. Then divide the rate constant for the catalyzed reaction by the rate constant for the uncatalyzed reaction to determine the factor by which the rate increased. You may want to review Hint 1. Express the ratio of the rate constants at different activation energies. 國 國

Relate the breaking and forming of bonds to the release of or requirement for energy. H. -H + 0=0 H. 0=0 o=0 Course of Reaction (time) 1) How energetic (H) is the transition state for the reaction? Why does this molecule contain more or less energy? 2) Sketch the energetics of this reaction, label the delta G, label the activation energy Free Energy (G)