
The reaction 2 NO2 --> 2 N2 + O2 follows the mechanism: Step 1: NO2 --NO...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 + O2 slow; rate determining step Step 2 NO3 + NO2 --> N2O5 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. Write the rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates...
What is the rate law derived from the following mechanism? Step 1: 2 NO(g) N2O2(g) (fast) Step 2: N2O2(g) + O2(g) —>2 NO2 (g) (slow) Rate = k[NO]2 Rate = k[NO]2[02] Rate = K[N2021 Rate = K[N202][02]
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1- 2NO2(g) à 2NO(g) + O2(g) (slow) 2- NO(g) + CO(g) + O2(g) à NO2(g) + CO2(g) (fast) Then its rate law is: A) Rate = k [NO2] . [CO] B) Rate = k [NO2] . [CO2] C) Rate = k [NO 212 D) Rate = k [co]2
10. Consider the reaction that takes place via the mechanism below; STEP I: NO2(g) + CO(g) - NO(g) + CO2(e) (fast) STEP II: NO) + Cl2(e) - NOC12(e) (slow) Determine; (a) The reaction intermediate(s) (2 points) command (b) The rate determining step (2 points)
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2 2Br fast Step 2 Br + H2 H2Br fast Step 3 H2Br + Br 2HBr slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate law for each step including any reversible steps? d. What is the predicted rate law expression for this reaction. Be sure to only list reactants from the overall equation and...
For the reaction 2 NO (g) + O2 (g) → 2 NO2 (g) it is found that the rate doubles when the O2 concentration is doubled, but the rate increases by a factor of 4 when the NO concentration is doubled. Which of the following mechanisms is/are consistent with this? 1. (i) NO + O2 ⇋ NO3 (fast) (ii) NO + NO3 → 2 NO2 (slow) 2. (i) 2 NO → N2O2 (slow) (ii) O2 + N2O2 → N2O4 (fast)...
Suppose that for the reaction of nitrogen dioxide and carbon monoxide NO2 + CO → NO + CO2 the following mechanism has been proposed at high temperatures: (1) NO2 + CO → O-N-O-C-O (slow) (2) O-N-O-C-O → NO + CO2 (fast) Check the box for each species that is an intermediate in this mechanism and explain why? NO2 O-N-O-C-O NO CO2 CO None of the above
Problem B. For the mechanism Step 1 2NO:N20s+ 0 Step 2 CO+O→CO2 Step 3 N:0> NO+NO ki fast equilibrium s slow ks fast Draw a reaction coordinate for the mechanism below, keeping in mind that the following must be included Reagents, intermediates (if present) and products a. b. Relative magnitude of activation energy c. Endo/exothermicity of each step and of the overall reaction (Hint: Think about bond enthalpies)
10. Consider the reaction that takes place via the mechanism below; STEPI: NO2(g) + CO(g) → NO(g) + CO2(e) (fast) STEP II: NO(8) + Cl2(e) → NOCl2(g) (slow) Determine; (a) The reaction intermediate(s) (2 points) (b) The rate determining step (2 points)