Consider the following mechanism.
(1) ClO-(aq) + H2O(l) ---> HClO(aq) + OH -(aq) [fast]
(2) I -(aq) + HClO(aq) ---> HIO(aq) + Cl -(aq) [slow]
(3) OH -(aq) + HIO(aq) ---> H2O(l) + IO-(aq) [fast]

(a) What is the overall equation? (Type your answer using the format [NH4]+ for NH4+. Use the lowest possible coefficients. Enter 0 if necessary. Do not leave any box blank.)
(aq) + I -(aq) Cl -(aq) + (aq) (b) Identify the intermediates, if any.
(Select all that apply.)

IO-
I -(aq)
ClO-(aq)
H2O(l)
HClO(aq)
no intermediates
OH -(aq)
Cl -(aq)
HIO(aq)

(c) What are the molecularity and the rate law for each step?
Step (1) (forward step only)
unimolecular or bimolecular or trimolecular
rate = k[H2O]
rate = k[ClO-][H2O]
rate = k([OH-][H2O]
rate = k[ClO-]

Step (2)
unimolecular or bimolecular or trimolecular
rate = k[I-]
rate = k[HClO]
rate = k[I-][HClO]
rate = k[I-]2[HClO]

Step (3)
unimolecular or bimolecular or trimolecular
rate = k[OH-]
rate = k[OH-][HIO]2
rate = k[OH-][HIO]
rate = k[HIO]

(d) Is the mechanism consistent with the actual rate law: rate = k[ClO-][I -]?
yes
no