(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

(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

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...

See similar textbooks

Similar questions

The balanced chemical equation and rate law for the reaction between NO(g) and H2(g) at a particular temperature are 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) Rate = k[NO] [H₂] What is the reaction order with respect to nitric oxide AND the overall order of the reaction? 2,3 2,4 4,3 1,4 0,2
10 2NO₂Cl(g)2NO₂(g) + Cl₂(g) The following mechanism is proposed: NO₂Cl(g) NO₂(g) + Cl(g) NO₂Cl(g) + Cl(g) → NO₂(g) + Cl₂(g) slow Which of the following rate laws is consistent with this mechanism? rate= K[NO₂CI]2[NO2]-1 rate = K[NO₂CI]²[NO2] rate = K[NO₂CI] rate=k[NO₂CI]² rate=k[NO₂][NO₂CI] X (no answer) Correct Answer: rate= K[NO₂CI]²[NO2] 1 fast equilibrium
Overall Reaction: A2 + BC4 → AB + AC4 The proposed mechanism is as follows: A2 ⇋ 2A (fast) A + BC4 → AB + AC3 (slow) A + AC3 ⇋ AC4 (fast) What is the rate law?
Please don't provide handwritten solution
The following reaction is observed to be second order with respect to NO and first order with respect to Br2. Br2 (g) + 2NO (g) --> 2NOBr (g)
The reaction of NOBr(g) to form NO(g) and Br2(g) is second order: 2NOBr(g) → 2NO(g) + Br₂(g) The rate constant is 0.556 L mol-¹ s¹ at some temperature. If the initial concentration of NOBr in the container is 0.21 M, how long will it take for the concentration to decrease to 0.028 M? t = S
During kinetic studies, the following reaction was determined to be second order in respect to NO and zeroth order in respect to O2. What is the rate law for the reaction? 2 NO (g) + O2(g) -----> 2NO2 (g)
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0039 M²s¯¹: 2N₂O(g) 2 N₂(g) + O₂(g) Suppose a 4.0 L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. How much is left 6.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 00 X 3
Please complete the question typed ONLY. Please do not use handwriting.
During kinetic studies, the following reaction was determined to be second order in respect to NO and zeroth order in respect to O2. What is the rate law for the reaction? 2 NO (g) + O2 (g) 2 NO2 (g) rate = k [O2]? %3D O rate = k [NO]?[O2]? rate = k [NO][O2] rate = k [NO]2[O2] %3D O rate = k [NO]? %3D
A valid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOC12 (g) + NO (g) → 2 NOCI (g) (slow) (fast) What is the rate law for this reaction? Rate = k[NO]?[Cl2] Rate = k[NO][CI] Rate = k[NO][Cl2][NOCI] Rate = k[Cl2][NOC12]
The reaction 2 NO(g) + Cl2(g) → 2 NOCl(g) is 2nd order in NO and 1st order in Cl2. 5 mol of nitric oxide and 2 mol of chlorine were brought together in a volume of 2 dm3 and the initial rate was 2.4× 10–3 mol dm3 s–1. What will be the rate when half of the chlorine has reacted?