Hydrogen peroxide and the iodide ion react in acidic solution as follows: 

The kinetics of this reaction were studied by following the decay of the concentration of H₂O₂ and constructing plots of ln[H₂O₂] versus time. All the plots were linear and all solutions had [H₂O₂]₀ = 8.0 × 10^-4 mol/L. The slopes of these straight lines depended on the initial concentrations of I^- and H⁺. The results follow:

The rate law for this reaction has the form 

a. Specify the order of this reaction with respect to [H₂O₂] and [I^-].

b. Calculate the values of the rate constants, k₁ and k₂.

c. What reason could there be for the two-term dependence of the rate on [H⁺]?

Transcribed Image Text:

H₂O₂(aq) +31-(aq) + 2H+ (aq) — →→→→→→→13(aq) + 2H₂O(1)