The oxidation of iron (II) ions by iodine in aqueous solution occurs as shown below
2 Fe2+ (aq) + l2 (aq) → 2 Fe3+ (aq) + 2 l - (aq)
and the experimental rate law is found to be:
Rate = k [Fe2+][I2]
The proposed mechanism shown below is a valid choice for this reaction:
Fe2+ (aq) + I2 (aq) → Fe3+ (aq) + I2 - (aq)
Fe2+ (aq) + I2 - (aq) → Fe3+ (aq) + 2 I - (aq)
Which of the following statements is true about the proposed reaction mechanism?
a. I2- is the catalyst in this mechanism.
b. Fe3+ is the intermediate in this mechanism
c. The second step is the rate determing step.
d. The rate determining step is bimolecular
e. The reaction is first order overall.
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