Question

1) The decomposition of hydrogen peroxide in solution and in the presence of iodide ion was studied in laboratory, and the following mechanism proposed based on the experimental data.

H2O2 + I - = H2O + IO - (slow)
H2O2 + IO - = H2O + O2 + I - (fast)


Which one of the following statements is false? Choose answer (E) if more than one or none are false.

a. The reaction is first order with respect to H2O2.
b. The reaction is first order with respect to I -
c. I - is a catalyst.
d. IO - is an intermediate.
e. More than one the above statements is false (or none of the statements are false).

I chose that more than one of the statements are correct because I think that statements 1 and 2 regarding the order are correct.

2) The equation A + 2 B = C + D describes an elementary reaction, which takes place in a single step. Thus, the rate law must be

a. rate = k(A)2
b. rate = k(B)2
c. rate = k(A)(B)
d. rate = k(A)(B)2
e. none of the above represents the rate law for this elementary reaction.

I am not sure about this one. I think that the answer is either k(A)(B)^2 or none of these.

Are these correct?