What is the rate law for the following mechanism:2 A+B2C (fast equilibrium; rate of forward reaction: k], rate of reverse reaction: k.1)B+C -D (slow, rate: k2)D - E(fast, rate: k3)Rate= k2 (k1/k.1) [A]²[B}²OA.O B. Rate= (k1 k1) [A][B]²В.Rate= k2 [B][C]O D. Rate= k2 (k1/k1)[A]{{B]O E. Rate= k2 [A]²B]²Е.

Slow step is rate determining step and also we use equilibrium expression for removing intermediate…

Answered: What is the rate law for the following…

What is the rate law for the following mechanism: 2 A+B2C (fast equilibrium; rate of forward reaction: k1: rate of reverse reaction: k.1) B+C -D (slow, rate: k2) D -E (fast, rate: k3)

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 following mechanism has been proposed for the gas- phase reaction of chloroform (CHCI,) and chlorine: Step 1: Cl2(8) 2 CI(g) (fast) Step 2: CI(g) + CHCI3(g) , HCI(8) + CC13(8) (slow) Step 3: CI(g) + CCl;(g) , CC4 (fast) (a) What is the overall reaction? (b) What are the intermedi- ates in the mechanism? (c) What is the molecularity of each of the elementary reactions? (d) What is the rate-determining step? (e) What is the rate law predicted by this mechanism? (Hint: The overall reaction order is not an integer.)
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7. Reactions A and B were studied and found to produce the given energy diagrams. 150 150 Energy 100 (kJ/mol) 100 Energy (kJ/mol) 50 50 Reaction progress Reaction progress Reaction A Reaction B A third reaction, C was studied with a measured activation energy of 55 KJ/mol. Assume all reactions take place at the same temperature. Reaction A is slowest a. b. Reaction B is slowest c. Reaction C is slowest d. All reactions happen at the same rate.
3) For reaction A ->B All of the following statements for the value of A[A]/ At are true except: a) change as long as the reaction continues. b) The sign is always negative. c) The sign is always positive. d) It depends on the reaction rate law
Write a balanced reaction for which the following rate relationships are true. Rate = - 1 ∆[N2O5] / 2∆t = 1 ∆[NO2] / 4 ∆t = ∆[O2] / ∆t A) 1/2 N2O5 → 1/4 NO2 + O2 B) 4 NO2 + O2 → 2 N2O5 C) 2 N2O5 → 4 NO2 + O2 D) 1/4 NO2 + O2 → 1/2 N2O5 E) 2N2O5 → NO2 + 4 O2
The proposed 3-step mechanism for a reaction isStep 1) X(g) + Y(g) A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k-1 = reverse rate constant.)Step 2) A(g) + Z(g) B(g) slow (k2 = rate constant) Step 3) B(g) P(g) fast (k3 = rate constant) a) What is the overall reaction? b) What is the rate law supported by this mechanism? Explain your answer. c) The following is experimental data found for this reaction: Initial [X] (M) Initial [Y] (M) Initial [Z] (M) Initial Rate (M/day) Exp 1 0.150 0.150 0.150 0.569 Exp 2 0.250 0.150 0.150 0.948 Exp 3 0.250 0.300 0.150 3.793 Exp 4 0.300 0.350 0.200 6.196 i) What is the experimentally determined rate law? ii) Determine the rate constant and include units. d) Does your experimentally determined rate law support the proposed mechanism? Explain your answer. e) ΔΔHo = -347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism.…
9:54 AM Tue Nov 21 For the following reaction mechanism, what is the catalyst? NO(g)+O3(g) → NO2(g) + O2(g) A) O(g) O(g) +NO2(g) O2(g) + NO(g) B) O₂(g) C) O3(g) Question 20 of 20 D) NO(g) E) NO₂(g) O3(g) O2(g) + O(g) Tap here or pull up for additional resources 36% Submit
Hello, is it possible to answer all of them since they're multiple choice? Would really appreciate it. Thank you.
Which of the following mechanisms is consistent with the energy diagram shown below: Energy Progress of the reaction A+B ---> C O 2A---> C (fast) B+C -> D (slow) A+B ---> C (slow) C---> D (fast A---> B (slow) B ---> C (fast) C---> D (fast)
At equilibrium, the mechanism 2 The reaction, A + 3B-> D + F was studied and the following mechanism was established: A + B -> C (fast) C + B-> D+E (slow) E + B > F (very fast) W #3 Peaction rate equals the reverse reaction rate. E $ 4 R % 5 T MacBook Pro 6 Y & 7 The species E is properly described as a co-factor an intermediate a reactant an enzyme a catalyst The species C is properly described as a catalyst an enzyme an intermediate a co-factor a reactant U 8 ( n O