For the reaction H_2O_2 + 2H^+ + 2I^-rightarrow l_2 + 2H_2O in acidic aqueous so

Question

For the reaction H_2O_2 + 2H^+ + 2I^-rightarrow l_2 + 2H_2O in acidic aqueous solution, a proposed mechanism is H^+ + I^-irreversible HI HI + H_2O_2 rightarrow H_2O + HOI HOI +I^- rightarrow I_2 + OH^- OH^- + H^+ rightarrow H_2O Verify that this mechanism adds to the correct overall reaction. Using the rate determining step approximation and assuming that the first step is in rapid equilibrium, the second step is slow, and the last two steps are fast determine the overall rate law predicted by this mechanism. Apply the steady-state approximation for the above mechanism. Drop the assumptions about the speed of each step and determine the overall rate law predicted by the steady-state approximation. Under what conditions the rate law predicted by this approximation coincides with the rate law obtained in Problem 1?

Explanation / Answer

Slowest step is rate determining step.

rate = k2(H2O2)(HI) -------------(1)

Given that step-1 is in equilibrium.

so,

k1/k-1  = (HI) / (H*)(I*)

K1 = (HI) / (H*)(I*) -------------(2)

Solve equations (1) and (2) for (HI)

rate = k2K1 (H*)(I*)(H2O2)

RATE = k (H*)(I*)(H2O2)

Post other question separately. only one should be answered according t guidelines

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.