9:53 AM Tue Nov 21 Question 18 of 20 Step 1 (slow) H₂O2(aq) + (aq) H2O(l) + IO-(aq) Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I-(aq). What is the rate law for this reaction? Step 2 (fast) H₂O₂(aq) + 10-(aq) - A) rate = k[H₂O₂] B) rate = K[H₂O₂]² → H2O(I) + Oz(g) + I-(aq) C) rate = K[H₂O₂] [1] D) rate = K[H₂O₂] [10] 36% E) rate = k[H₂O₂]²[I¯]/[H₂O] Submit

9:53 AM Tue Nov 21 Question 18 of 20 Step 1 (slow) H₂O2(aq) + (aq) H2O(l) + IO-(aq) Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I-(aq). What is the rate law for this reaction? Step 2 (fast) H₂O₂(aq) + 10-(aq) - A) rate = k[H₂O₂] B) rate = K[H₂O₂]² → H2O(I) + Oz(g) + I-(aq) C) rate = K[H₂O₂] [1] D) rate = K[H₂O₂] [10] 36% E) rate = k[H₂O₂]²[I¯]/[H₂O] Submit

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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A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: (1) H₂O2(g) →>> 2OH(g) (2) H₂O2(g) + OH(g) → H₂O(g) + HO₂(g) (3) HO₂(g) + OH(g) → H₂O(g) + O₂(g) If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining step? O Step 1 O None of the steps O Step 3 O Impossible to determine Steps 1 and 2 O All of the steps O Step 2 Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can write a rate-law expression. Submit Question
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L Question 3 Moving to the next question prevents changes to this answer. esc The rate constant for the rate of decomposition of N205 to NO and O2 in the gas phase is 1.66 L/mol/s at 650 K and 7.39 L/mol/s at 700 K: 2N2O5(g) 4NO(g)+302(g) L Assuming the kinetics of this reaction are consistent with the Arrhenius equation, calculate the activation energy for this decomposition. 1.987kJ/mol 2.110kJ 3. 110 kJ/mol 4.1.1 x 10^6 kJ/mol Moving to the next question prevents changes to this answer. ! 1 Q @ 2 W a #3 E S4 $ for ICS R % 5 Bird Oue T MacBook Pro 6 Y 7 s U 8 9 O P (
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9:21 < A) s-¹ B) M-¹s-¹ The reaction, 2 NO(g) + O₂(g) → 2 NO₂(g) has a rate law, rate = k{NO] [O₂]. If the rate of the reaction is 0.60 M/s when [NO] is 1.5 M and [O₂] is 2.0 M, what are the units of the rate constant, k? C) Ms-¹ Question 5 of 20 D) M-²S-¹ E) None of these. 11 Tap here or pull up for additional resources Submit