Question

Consider this reaction mechanism: Step 1: C₄H₉Br C₄H₉+ + Br- (slow) Step 2: C₄H₉+ + OH- C₄H₉OH (fast) Which rate law is consistent with the mechanism? A. rate = k[C₄H₉Br][OH-] B. rate = k[C₄H₉+][OH-] C. rate = k[C₄H₉Br] D. rate = k[C₄H₉Br][OH-][Br-]-1 E. rate = k[C₄H₉+]2

A. rate = k[C₄H₉Br][OH-]
B. rate = k[C₄H₉+][OH-]
C. rate = k[C₄H₉Br]
D. rate = k[C₄H₉Br][OH-][Br-]⁻1
E. rate = k[C₄H₉+]²

Answer 1

The correct rate law that is consistent with the given reaction mechanism is option B: rate = k[C₄H₉+][OH-].

Step-by-step explanation:

The correct rate law that is consistent with the given reaction mechanism is option B: rate = k[C₄H₉+][OH-].

In the given mechanism, step 1 is the slow step. According to the rate-determining step, the rate law for the overall reaction will be the same as the rate law for the slow step. So, the rate law for the overall reaction is rate = k[C₄H₉+][OH-].