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ochrescorpion704Lv1

24 Jun 2020

For the reaction below,

proceeds rapidly by an inner-sphere mechanism when is replaced by in the cobalt reactant the reaction slows considerably () it is observed however that the reaction rate is inversely dependent upon the concentration of hydrogen ion provide an explanation that is consistent with these facts.

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Related questions

PLEASE EXPLAIN ALL OF THIS BETTER THAN THE BOOK AND DO EXAMPLE 14.9!!!

Ozone naturally decomposes to oxygen by this reaction: 2 O_3 (g) rightarrow 3 O_2 (g) The experimentally observed rate law for this reaction is: Rate = k [O_3]^2 [O_2]^-1 Show that this proposed mechanism is consistent with the experimentally observed rate law. O_3 (g) O_2 (g) + O (g) Fast O_3 (g) + O(g) 2 O_2 (g) Slow To determine whether the mechanism is valid, you must First determine whether the steps sum to the overall reaction. The steps do indeed sum to the overall reaction, so the first condition is met. O_3 (g) O_2 (g) + O (g) O_3 (g) + O (g) 2 O_2 (g)/2 O_3 (g) rightarrow 3 O_2 (g) The second condition is that the rate law predicted by the mechanism is consistent with the experimentally observed rate law. Because the second step is rate limiting, write the rate law based on the second step. Rate = k_2 [O_3] [O] Because the rate law contains an intermediate (O), you must express the concentration of the intermediate in terms of the concentrations of the reactants of the overall reaction. To do this, set the rates of the forward reaction and the reverse reaction of the first step equal to each other. Solve the expression from the previous step for [O], the concentration of the intermediate. Rate (forward) = Rate (backward) k_1 [O_3] = k_-1 [O_2] [O] [O] = k_1 [O_3]/k_-1 [O_2] Finally, substitute [O] into the rate law predicted by the slow step. Rate = k_2 [O_3] [O] = k_2 [O_3] k_1 [O_3]/k_-1 [O_2] = k_2 k_1 [O_3]^2/k_-1 [O_2] = k [O_3]^2 [O_2]^-1 CHECK Because the two steps in the proposed mechanism sum to the overall reaction, and because the rate law obtained from the proposed mechanism is consistent with the experimentally observed rate law, the proposed mechanism is valid. The -1 reaction order with respect to [02J indicates that the rate slows down as the concentration of oxygen increases- oxygen inhibits, or slows down, the reaction. FOR PRACTICE 14.9 Predict the overall reaction and rate law that results from the following two-step mechanism: 2 A rightarrow A_2 Slow A_2 + B rightarrow A_2 B Fast

I donât know how to do part a and b. Please show Work

Question 82a, 82b, 82c

553 CHAPTER 14 Chemical Kinetics: The Rates of Chemical Reactions trans-fColenhal.(aq) + H2O(C) â (see Section 4-8), and some data collected by that approach are given below. The initial concentrations were Iphenolphthalein] -0.0050 moUL and TOH 1 0.61 moVL (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L. Nicholson, Jourmal of Chemical Edacation, Vol 66, p. 725, 1989.) red The reaction progress is olowed by observing the of the solution. The original solution is green, and the final solution is red, but at some intermediate stage when is gray. Time ts) 0.00 0.0050 223 35.7 1.1 69.3 91.6 1204 160.9 2303 299.6 0.0035 0.0025 00015 0.0010 0.00050 000025 (a) Plot the data above as Iphenolphthalein] versus time, and determine the average rate from t15 seconds and from -125 seconds. Des the rate change? If so, why? 0 to 100 seconds to original solution intermedlate solution (b) What is the instantaneous rate at 50 seconds? (c) Use a graphical method to determine the order of the d) What is the half-life for the reaction? green, cobalt-based complex called trans-dichlorobis- reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. 82. You want to study the hydrolysis of the beautiful ethylenediamine)cobaltiIII) ion final solution Changes in color with time as CI- ion is replaced by H,O in a cobalt(Il) complex. The shape in the middle of the beaker is a vortex that arises because the solutions are being stirred us- ing a magnetic stirring bar in the bottom of the beaker Reactions such as this have been studied extensively, and that the initial, slow step in the reac- tion is the breaking of the Co-Cl bond to give a five- coordinate intermediate. The intermediate is then attacked rapidly by water Slow: trins-Co(enhal.(aq) â In this hydrolysis reaction, the green complex ion trans- Colen Cll forms the red complex ion [ColembalHO) [Co(enhci (aq) + a-(aq) cip as a Cl ion is replaced with a waser molecule on the Co- ion (en-H:NCH CHINH

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