Chemical Reaction Mechanism with Rate Law Explanation

What is the two-step reaction mechanism with overall reaction 2H2O2(aq) → 2H2O(l) + O2(g)?

Given the fast step and rate law: Step 2: H2O2 + OI– → H2O + O2 + I– (fast) Rate = k[H2O2][I–]

Answer:

The correct rate-determining step would be step 1 since it would have the slower reaction rate. It would be as follows: H2O2(aq) + I-(aq) → H2O(l) + IO-(aq)

A two-step reaction mechanism with an overall reaction of 2H2O2(aq) → 2H2O(l) + O2(g) involves multiple steps. In this case, Step 2 is given as: H2O2 + OI– → H2O + O2 + I– with a rate law of Rate = k[H2O2][I–]. This information is crucial in understanding the kinetics of the reaction.

The correct rate-determining step in this mechanism is Step 1, where the reaction of H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) takes place. The rate-determining step is the slowest step in a reaction mechanism, and it determines the overall rate of the reaction.

Understanding the rate-determining step is important as it helps in identifying the key factors that influence the overall reaction rate. By determining the slowest step, we can adjust reaction conditions to optimize the rate of the desired reaction.