What is the rate law derived from the following mechanism? Step 1: 2 NO(g) N2O2(g) (fast)...
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[02] Rate = k[N202][02] Rate = k[N202] Rate = k[NO]2
For the following two-step mechanism: Step 1: NO (g) + NO (g) --K1--> N2O2 (g) (fast, equilibrium) <------- Step 2: N2O2 (g) + Br2 (g) ------> 2 NOBr (g) (slow) (a) Write the equation for the overall reaction. (b) Write the raw law for the overall reaction.
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....
If molecular oxygen is reacting at a rate of 0.024 M/s in the following reaction; 4 NO2(g) + O2(g) → 2 N205(8) at what rate is N2O5 being formed? O 0.048 M/s 0.096 M/S 0.024 M/s 0.012 M/s The rate law for the reaction 2 NO, +O3 -- N2O5 + O, is rate - k[NO][03]. Which one of the following mechanisms is consistent with this rate law? NO2 + NO2-N202 + O2 (slow) N2O2 +O3-N20s (fast) NO2+O3 -NO3 + O2...
Consider the following mechanism. step 1 2A > B slow B+ C D fast step 2 overall: 2A+C D Determine the rate law for the overall reaction (where the overall rate constant is represented as k) rate=
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
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...
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...
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
QUESTION 9 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? k[N2O][H2] k[NO]2[H2] k[NO]2[H2]2 k[NO]1/2[H2] k[NO]2