Name____________________________

Ch. 14 Kinetics Review1. What are the 4 factors that can affect the rate of a reaction?

Show your work for every calculation. Round your answer to the correct number of significant figures and record your final answer with correct units on the line provided.2. A reaction A + B C obeys the following rate law: Rate = k[A]

2[B].

a. If [A] is doubled, will the rate constant change? Explain.

b. If [A] is doubled, how will the rate change?

c. What are the reaction orders for A and B? A = B =

d. What is the overall reaction order?

e. What are the units of the rate constant?

3. Consider the following reaction:2 NO(g) + 2H2(g) N2(g) + 2H2O(g)

a. The rate law for this reaction is first order in H2 and second order in NO. Write the rate law.Rate =

b. If the rate constant for this reaction at 1000K is 6.0 x 104

M-2

s-1

, what is the reaction rate when [NO] = 0.025 M and [H2] = 0.015 M?

c. What is the reaction rate at 1000K when the concentration of NO is increased to 0.10 M while the concentration of H2 is 0.010 M?

4. The reaction below was studied and produced the results in the table.

2 ClO2 + 2 OH-

ClO3-

+ ClO2-

+ H2O

a. Determine the rate law for the reaction. Rate =

b. Calculate the rate constant.

c. Calculate the rate when [ClO2] = 0.010 M and [OH-] = 0.025 M.

5. A + 2B 2CThe following results were obtained in experiments designed to study the rate of the reaction above.

Experiment Initial Concentration (mol/L)[A] [B]

Initial Rate of Disappearance of A (M/s)

1 0.05 0.05 3.0 x 10 -3

2 0.05 0.10 6.0 x 10 -3

3 0.10 0.10 1.2 x 10 -2

4 0.20 0.10 2.4 x 10 -2

a) Determine the order of the reaction with respect to each of the reactants and write the rate law for the reaction.

b) Calculate the value of the rate constant, k, for the reaction. Include units.

c) If another experiment is attempted with [A] and [B] both 0.02 M, what will be the initial rate of disappearance of B?

d) The following reaction mechanism was proposed for the reaction above.A + B C + DD + B C

i) Show that the mechanism is consistent with the balanced reaction.

ii) Show which step is the rate-determining step and explain your choice.

6. 2 NO (g) + Br2 (g) 2 NOBr (g)The following results were obtained in experiments designed to study the rate of the reaction above.

Experiment Initial Concentration (mol/L)[NO] [Br2]

Initial Rate of Appearance of NOBr (M/s)

1 0.0200 0.0200 9.6 x 10 -5

2 0.0400 0.0200 3.8 x 10 -4

3 0.0200 0.0400 1.9 x 10 -4

a) Write the rate law for the reaction b) Calculate the value of the rate constant, k, for the reaction. Include the units.

b) In experiment 2, what was the concentration of NO remaining when 2/3 of the original amount of Br2 was consumed?

c) Which of the following reaction mechanisms is consistent with the rate law established in (a)? Explain your choice.

I. NO + NO N2O2 (fast)

N2O2 + Br2 2 NOBr (slow)

II. Br2 Br + Br (slow)

2NO + Br NOBr (fast)