![e . b. (- R 0.3 14 J/ k -mol) 6.4×10-4 M.si c. 2.1 x 103 Ms d. 3.6×10-3 Migl e. 2.5x 1026Ms 23. Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide NO2(g) + CO(g) → NO(g) + CO2(g) A proposed mechanism for this reaction is 2 NO2(g) → NO2(g) + NO(g) (fast, equilibrium) N03(g) + CO(g) → NO2(g) + CO2(g) (slow) What is a rate law that is consistent with the proposed mechanism? a. rate = k[NO2][CO] b. rate kIINO ICO] c. rate =k[[NO2]2[CO]/[NO] d. rate kNO JICO] e. rate kINO2] For the overall reaction A +2B->C which of the following mechanisms is consistent with the rate equation below rate KA] [B] 24. I (fast) 2A + B → I + B → C + A (slow) A + B → I (slow) l+B→C(fast) 2B→1 (slow) A + 1 → C (fast) 2B fI (fast) 1 + A → C (slow) A + 2B → 1 (fast) I + B → C + B (slow) a. b) c. d. e,](http://img.homeworklib.com/questions/4ad492c0-a7ff-11eb-8bfd-832abec0c3e9.png?x-oss-process=image/resize,w_560)
Homework Answers
23) According to chemical dynamics, rate of a reaction always depends upon the slowest step or, in otherwords slowest step is the rate determining step. In this context the second step of the mechanism presented being the slowest step, it is the rate determing step and rate of reaction can be presented as,
d. Rate = k[NO3][CO]
After your selection in a if more than one mechanism is still plausible propose possible experiment...
After your selection in a if more than one mechanism is still
plausible propose possible experiment that could help determine
which of the remaining mechanisms might be further validated
The macro rate law for conversion of nitrogen monoxide from auto exhausts into the brown smog pollutant nitrogen dioxide, 2 NO (g) + O2 (g) → 2 NO2 (g) is: rate-k[NOF [02] Six mechanisms proposed. When艹appears, means elementary step is an equilibrium reaction: Mech A NO (g) + NO (g) N2O2...
16. For the overall reaction which of the following mechanisms is consistent with the rate equation...
16. For the overall reaction which of the following mechanisms is consistent with the rate equation below? rate = k[A] [B]2 a. 2A + B →I (fast) I + B → C + A (slow) A + B → 1 (slow) 1 + B → C (fast) 2B → 1 (slow) A + 1 → C (fast) 2B→1(fast) 1 + A → C (slow) A + 2B → 1 (fast) 1 + B → C + B (slow) b, d....
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1-...
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
57.) The ozone, O3, of the stratosphere can be decomposed by reac- tion with nitrogen oxide...
57.) The ozone, O3, of the stratosphere can be decomposed by reac- tion with nitrogen oxide (commonly called nitric oxide), NO, from high-flying jet aircraft. O3(g) + NO(g) → NO2(g) + O2(g) The rate expression is rate = k[O3][NO]. Which of the following mechanisms are consistent with the observed rate expression? (a) NO + 03 - NO3 + 0 (slow) NO3 +0 - NO2 + O2 (fast) O3 + NO → NO2 + O2 overall (b) NO + O3 ->...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step...
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....
Please answer questions 14, and 15!! The rate constant for a particular reaction is 0.47 M^-1...
Please answer questions 14, and 15!!
The rate constant for a particular reaction is 0.47 M^-1 s^-1. If the initial concentration of reactant is 0.25 mol/L, it takes _____ s for the concentration to decrease to 0.20 mol/L. A) 2.1 B) 1.4 C) 1.0 D) 0.47 E) 0.20 Use the mechanism below to answer the next question NO + Br_2 doubleheadarrow NOBr_2 (fast) NOBr_2 + NO rightarrow 2NOBr (slow) Which of the following reaction mechanisms is consistent with the proposed...
I Man energy is Thul Is Its half-life at 815 K? = 226x 10 Jmol-1 (...
I Man energy is Thul Is Its half-life at 815 K? = 226x 10 Jmol-1 ( t al 14. Се — 7 aaa x 10 • то 2.314 I morical 315k - 1 Two mechanisms are proposed for the reaction 7201 =.960 2NO(g) + O2(g) + 2NO2(g) 1: NO + O2 + NO3 (fast) 2: NO + NO + N20 (fast) NO3 + NO + 2NO2 (slow) N202 + 02 → 2NO (slow) Which of these mechanisms is consistent with...
4. For the reaction A+B → C+D we find that the rate law is v=k[A]”[B]° Which...
4. For the reaction A+B → C+D we find that the rate law is v=k[A]”[B]° Which of the following mechanisms is consistent with the rate law? Explain in detail. a) A+B → C+D b) A+A ~ A2 (fast step) A2 +B → C+D (slow step) c) A+A → A2 (slow step) A2+B → C+D (fast step) d) A+A → A2 (fast equilibrium) A2+B → C+D (slow step)
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate =...
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
10. Consider the reaction that takes place via the mechanism below; STEP I: NO2(g) + CO(g) - NO(g) + CO2(e) (fast)...
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)
After your selection in a if more than one mechanism is still
plausible propose possible experiment that could help determine
which of the remaining mechanisms might be further validated
The macro rate law for conversion of nitrogen monoxide from auto exhausts into the brown smog pollutant nitrogen dioxide, 2 NO (g) + O2 (g) → 2 NO2 (g) is: rate-k[NOF [02] Six mechanisms proposed. When艹appears, means elementary step is an equilibrium reaction: Mech A NO (g) + NO (g) N2O2...
16. For the overall reaction which of the following mechanisms is consistent with the rate equation below? rate = k[A] [B]2 a. 2A + B →I (fast) I + B → C + A (slow) A + B → 1 (slow) 1 + B → C (fast) 2B → 1 (slow) A + 1 → C (fast) 2B→1(fast) 1 + A → C (slow) A + 2B → 1 (fast) 1 + B → C + B (slow) b, d....
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
57.) The ozone, O3, of the stratosphere can be decomposed by reac- tion with nitrogen oxide (commonly called nitric oxide), NO, from high-flying jet aircraft. O3(g) + NO(g) → NO2(g) + O2(g) The rate expression is rate = k[O3][NO]. Which of the following mechanisms are consistent with the observed rate expression? (a) NO + 03 - NO3 + 0 (slow) NO3 +0 - NO2 + O2 (fast) O3 + NO → NO2 + O2 overall (b) NO + O3 ->...
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....
Please answer questions 14, and 15!!
The rate constant for a particular reaction is 0.47 M^-1 s^-1. If the initial concentration of reactant is 0.25 mol/L, it takes _____ s for the concentration to decrease to 0.20 mol/L. A) 2.1 B) 1.4 C) 1.0 D) 0.47 E) 0.20 Use the mechanism below to answer the next question NO + Br_2 doubleheadarrow NOBr_2 (fast) NOBr_2 + NO rightarrow 2NOBr (slow) Which of the following reaction mechanisms is consistent with the proposed...
I Man energy is Thul Is Its half-life at 815 K? = 226x 10 Jmol-1 ( t al 14. Се — 7 aaa x 10 • то 2.314 I morical 315k - 1 Two mechanisms are proposed for the reaction 7201 =.960 2NO(g) + O2(g) + 2NO2(g) 1: NO + O2 + NO3 (fast) 2: NO + NO + N20 (fast) NO3 + NO + 2NO2 (slow) N202 + 02 → 2NO (slow) Which of these mechanisms is consistent with...
4. For the reaction A+B → C+D we find that the rate law is v=k[A]”[B]° Which of the following mechanisms is consistent with the rate law? Explain in detail. a) A+B → C+D b) A+A ~ A2 (fast step) A2 +B → C+D (slow step) c) A+A → A2 (slow step) A2+B → C+D (fast step) d) A+A → A2 (fast equilibrium) A2+B → C+D (slow step)
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)
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