Question

A two-step reaction mechanism that has an overall reaction of 2H2O2(aq) mc012-1.jpg 2H2O(l) + O2(g) has the following fast step and rate law. Step 2: H2O2 + OI– mc012-2.jpg H2O + O2 + I– (fast) Rate = k[H2O2][I–] Which is the correct rate-determining step given the information in the reaction above?

Answer 1

D maybe not 100%

Step-by-step explanation:

Answer 2

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)

The slow step in a reaction mechanism would always be the rate-determining since it is at this rate everything follows through. Hope this helps.