1. A reaction that is second-order in one reactant has a rate constant of 2.2×10−2 L/(mol⋅s). If the initial concentration of the reactant is 0.360 mol/L, how long will it take for the concentration to become 0.180 mol/L

 

Select one:

 a. 320 s

 b. 63 s

 c. 1300 s

 d. 32 s

 e. 130 s

 

2. Below is a proposed mechanism for the decomposition of H2O2.

 

H2O2+I– →H2O+IO– slow

H2O2+IO–→H2O+O2+I– fast

 

What is the rate law predicted by this mechanism?

Select one:

 a. 

Rate=k[H2O2][I−]

 

 b. 

Rate=k[H2O2][IO−]

 

 c. 

Rate=k[H2O2]2

 

 d. 

Rate=k[IO−]

 

 e. 

Rate=k[H2O2]

 

 

3. For a certain reaction of the general form a A→products, the experimental data plotted as 1/ [A]versus time is linear. What is the reaction order with respect to [ A]?

Select one:

 a. 0

 

 b. 1

 

 c. 2

 

 d. 3

 

 e. ½ 

 

 

 

4. For the hypothetical first-order reaction A→ products, k=0.839 s–1. If the initial concentration of A is 0.640 M, how long would it take for A to be 66.4% consumed?

Select one:

 a. 8.26 s

 b. 1.29 s

 c. 11.9 s

 d. 18.6 s

 e. 4.88 s

 

 

 

 

 

5. For a hypothetical second-order reaction, A→ products, k = 0.319 M-1s-1. If the initial concentration of A is 0.834 M, how long would it take for A to be 94.8% consumed?

Select one:

 a. 0.206 s

 b. 3.76 s

 c. 9.27 s

 d. 68.5 s

 e. 0.167 s

 

 

 

6. The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: 

 

NO (g) +NO (g) →N2O2 (g) (slow)

 

N2O2 (g) +O2 (g) →2NO2 (g) (fast)

 

 

According to this mechanism, the experimental rate law is

Select one:

 a. 

Rate=k[NO]2

 

 b. 

Rate=k[NO]2[O2]

 

 c. 

Rate=k[NO]

 

 d. 

Rate=k[O2]

 

 e. 

Rate=k[NO][O2]

 

 

7. The reaction A→ products is zero-order in A. If the concentration of A is cut in half, the half-life of the reaction will

Select one:

 a. decrease by a factor of ½ 

 b. double 

 

 c. decrease by a factor of ¼ 

 d. remain constant

 

 e. quadruple

 

 

8. Which of the following corresponds to the correct equation for the half-life of a second-order reaction?

Select one:

 a. 

t1/2=1k[A]0 

 

 b. 

t1/2=k / ln(2)

 

 c. 

t1/2=[A]0 / 2k

 

 d. 

t1/2= k / 0.5

 

 e. 

t1/2=0.693 / k

 

 

9. Which of the following statements concerning collision theory are correct.

1) Reactant molecules must collide to react.

2) Reactant molecules must collide with a certain minimum energy in order to form products.

3) Reactant molecules must collide with the correct orientation in order to form products.

 

Select one:

 a. 1 only

 b. 2 only

 c. 3 only

 d. 1 and 3

 e. 1, 2, and 3

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