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?

1) To determine which statement is false, let's analyze each statement:

a. The reaction is first order with respect to H2O2.
To determine if this statement is true, we need to look at the rate-determining step of the reaction. In the proposed mechanism, the slow step is the reaction between H2O2 and I-. Since H2O2 is consumed in this step, we can conclude that the rate of the reaction is dependent on the concentration of H2O2, making it first order. So, statement a is true.

b. The reaction is first order with respect to I-.
Similar to the analysis for statement a, we need to examine the slow step. In this case, the slow step involves the reaction between H2O2 and I-. Since I- is also consumed in this step, the rate of the reaction is dependent on the concentration of I-, confirming that it is first order. Thus, statement b is true.

c. I- is a catalyst.
A catalyst is a substance that increases the rate of a reaction without being consumed in the process. Looking at the mechanism, we see that I- is involved in the slow step and is consumed, indicating that it is not acting as a catalyst. Therefore, statement c is false.

d. IO- is an intermediate.
An intermediate is a species that forms during the course of a reaction but is later consumed in a subsequent step. In this mechanism, IO- is formed in the slow step but is then consumed in the fast step. Thus, IO- is an intermediate. Therefore, statement d is true.

From the analysis above, we can conclude that statement c is false. Therefore, the correct answer is (c).

2) To determine the correct rate law, we need to examine the stoichiometry of the reaction:

A + 2B = C + D

The coefficients in the balanced equation indicate the number of molecules or moles involved in the reaction. Based on this equation, we can determine that the rate of the reaction is dependent on the concentration of both A and B, but not on C or D.

Therefore, the correct rate law is given by:

rate = k(A)(B)

So, the correct answer is (c).

Your analysis for question 1 is correct, and for question 2, the correct answer is (c). Well done!