Sol: when these two equations (slow and fast) combines it give the overall reaction between NO2 and CO.
The slowest step is the rate determining step. Hence,
Rrxn = Rslow step= k[NO2]2
Hence rate of reaction is k[NO2]2
Correct option is C.
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1-...
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....
The reaction 2 NO2 --> 2 N2 + O2 follows the mechanism: Step 1: NO2 --NO NO3 NO2 SLOW + + Step 2: NO3 CO FAST NO2 CO2 -> + What is the intermediate in the reaction? none of these NO2 ONO3 OOOO
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)
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)
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...
For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g)+O2(g) Step 1: O3(g)+NO2(g)→NO3(g)+O2(g) slow Step 2: NO3(g)+NO2(g)→N2O5(g) fast View Available Hint(s) For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: Step 1: slow Step 2: fast A.] Rate=k[O3][NO2]2 B.] Rate=k[O3][NO2] C.] Rate=k[NO3][NO2] D.] Rate=k[O3][NO2]2[N2O5][O2]
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...
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...
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...
The rate of the reaction: CO (g) + NO2 (g) à CO2 (g) + NO (g) was measured at several temperatures, and the following data were collected: Temp (oC) K (M-1s-1) 35 0.184 45 0.322 Using this data determine the value of Ea (energy of activation)