The decomposition of hydrogen peroxide, H2O2, is catalyzed byBr– ions according to the following mechanism:
H2O2 + H H3O2 + forward rate constant k1, reverse rateconstant k–1
H3O2 + Br –→ HOBr + H2O forward rate constantk2
HOBr + H2O2 → H+ + H2O + O2 +Br– forward rate constant k3
Assume that the first step is in rapid equilibrium, and theintermediate HOBr is in steady-state. If we
measure the rate of O2 production (the rate of the third step),predict the rate law that would be observed based on thismechanism.