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

Question

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] 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+BC(fast) 2B1 (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,

Explanation / Answer

23)

rate depends on the slowest step
Here 2nd step is slowest
So, rate law is:
rate = k2[NO3][CO]

We need to remove intermediate which is NO3.
we will use 1st step:
Kc = [NO3][NO]/[NO2]^2
[NO3] = Kc[NO2]^2[NO]-1

rate law is:
rate = k2[NO3][CO]
rate = k2Kc[NO2]^2[NO]-1[CO]

writing k2Kc = k
rate = k[NO2]^2[NO]-1[CO]
Answer: c

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