10. The experimental rate law for the decomposition of nitrous oxide (N₂O) to N₂ and O₂ is Rate = k[N₂O]². Two mechanisms are proposed: I. NO → N,+0 N₂O +0 N₂ + O₂ II. 2N₂ON40₂ N4O₂ → 2N₂ + O₂ Which of the following could be a correct mechanism? A) Mechanism I with the first step as the rate-determining step. B) Mechanism I with the second step as the rate-determining step. C) Mechanism II with the second step as the rate-determining step. Two of these could be correct. None of these could be correct. D)

10. The experimental rate law for the decomposition of nitrous oxide (N₂O) to N₂ and O₂ is Rate = k[N₂O]². Two mechanisms are proposed: I. NO → N,+0 N₂O +0 N₂ + O₂ II. 2N₂ON40₂ N4O₂ → 2N₂ + O₂ Which of the following could be a correct mechanism? A) Mechanism I with the first step as the rate-determining step. B) Mechanism I with the second step as the rate-determining step. C) Mechanism II with the second step as the rate-determining step. Two of these could be correct. None of these could be correct. D)

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

Consider the reaction below and the proposed mechanism. X2 + Y + Z → XY + XZ Step l) X2 + Y → XY + X (very slow) Step 2) X + Z → XZ (very fast) What is the rate law for this reaction if the proposed mechanism is correct?
A) In the proposed reaction mechanism below, the intermediate product is: A). NO(g) B). N2O2(g) C). H2(g) D). N2O(g) B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors A) 2 B) 3 C) 6 D) 9
Consider the reaction and its rate law. 4A + 3B What is the order with respect to A? order: products What is the order with respect to B? order: What is the overall reaction order? overall order: rate = k[A]²[B]²
16 redone
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. 1 rate = (0.471 M¹S -¹) [N₂05]² Suppose a vessel contains N₂O5 at a concentration of 0.800M. Calculate the concentration of N₂O5 in the vessel 8.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10
3. Consider the reaction below: 2NO (g) + Cl,(g)'n 2NOCI (g) A mechanism involving these steps has been proposed for the reaction: Step 1: NO (g) + Cl,(g)'n NOCI, (g) Step 2: NOCI, (g) + NO(g)'n 2NOCI (g) The rate law for the reaction is given by rate = k[NO][Cl]. (a) What is the reaction intermediate? (b) Which is the rate-determining step? (c) Is the rate-determining step unimolecular, bimolecular, or termolecular? Why?
The experimental rate law for the decomposition of nitrous oxide (N2O) and O2 is Rate = k[N2O]2. Which of the following could be a correct mechanism, explain why.
A proposed mechanism for the reaction is: - Step 1: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) Step 2: N₂O(g) + H₂(g) → N₂(g) + H₂O(g) What is the rate law? More information is needed to answer this question. Or = K[H₂][NO] Or = K[H₂]²[NO]² Or = K[H₂][NO]² Or=K[H₂]²[NO] (slow) (fast)
Ozone decomposes to oxygen gas 2O3(g) → 3O2(g) A proposed mechanism for this decomposition is shown above. What is the rate law predicted by this mechanism?
Analyze the following reaction mechanism: 1. H2O2 → H,0 + O 2. O + CF2CI2 → CIO + CF2CI 3. CIO + O3 → CI + 202 4. CI + CF2CI → CF2CI2 Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF2CI, CF2CI2 С) О, CIO, O, H,0 D) O, CIO, CI, CF2CI E) O, CIO, CI, CF2CI2
Consider this reaction: 2SO3 (g) →2SO₂ (g) + 0₂ (8) At a certain temperature it obeys this rate law. rate= (0.00626 s¹)[03] Suppose a vessel contains SO3 at a concentration of 0.250M. Calculate the concentration of SO3 in the vessel 99.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś