16. For the overall reaction which of the following mechanisms is consistent with the rate equation...
e . b. (- R 0.3 14 J/ k -mol) 6.4×10-4 M.'si c. 2.1 x 103 M's d. 3.6×10-3 Migl e. 2.5x 1026M''s 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]...
Question 16 of 20 > Which of the reaction mechanisms is consistent with the energy diagram? O 2A STB slow BC O A+B +C Energy slov O A+B= 0 C D O 2A slow B fast BC CFD Progress of reaction Explain your reasoning: This ungraded area will provide insight to your instructor:
* Blackboard → XCO Remaining Time: 51 minutes, 08 seconds. Question Completion Status: QUESTIONS For the overall reaction 2A-B- C which of the following mechanisms are consistent with a rate equation of rate = K[A] [B]? a. A+B=1(fast) I+A -C(slow) b. A-B-1 (slow) I-A-C(fast) C 2A-1 (slow) B+1-C(fast) d. 2A=I (fast) I-B-C (slow) e. Answers a and d are both correct. QUESTION 6 The rate law for a reaction is Rate = (AJB) - Which one of the following statements...
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]
Consider the overall reaction.... A+B--C+D which has an observed rate law of Rate=k[A12 Which of the following choices would be a sensible 2-step mechanism, given this observed rate law? O A+A-->E slow E+B-->C+D fast A+B--> 2 E --> C+D fast slow A+A-->E E+B-->C+D fast slow A+B-->E 2 E -->C+D slow fast
please explain why you chose this answer 10.For the overall reaction, 2 A+B C+ D, the rate law is: rate = k[A][M]. Which of the following mechanisms involving intermediates M and/or N would be consistent with this information? a. B M M+A N N A C+D (fast) b. A M A M C+ D (fast) (fast) (slow) (slow) c. A+A M MC+D (fast) (slow) (slow) (fast) (fast) d. B M M+A N N A C+D
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=
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)
A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step slow: F2+CIO, FCIO, + F step 2 fast: F+CIO, FCIO, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank (3) Which species acts as a reaction intermediate? Enter formula....
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...