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
ID: 1087921 • Letter: E
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) 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]
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