🤓 Based on our data, we think this question is relevant for Professor Hemmes' class at TXSTATE.
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.