A chemical reaction proceeds via a two-step mechanism: (slow step) and (fast step). How many transition states will be observed in its reaction coordinate diagram?

Question

A chemical reaction proceeds via a two-step mechanism: $A \rightarrow B$ (slow step) and $B \rightarrow C$ (fast step). How many transition states will be observed in its reaction coordinate diagram?

Prashant Kotian · Accepted Answer

Correct answer: B. A two-step mechanism implies the formation of one intermediate (B). Each distinct step requires surmounting its own activation energy barrier, representing one transition state per step. Therefore, a two-step reaction has exactly 2 transition states.

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