Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
168 Chemistry: Matter and Change
Solving Problems: A Chemistry Handbook
SOLVING PROBLEMS:
A CHEMISTRY HANDBOOK
CHAPTER 16
The IO Ϫ ion is called an intermediate in the reaction. An intermediate is an atom, an ion, or a molecule produced in one step of a
reaction and consumed in a later step. In a complex reaction, one
step is always slower than the others. This step is called the ratedetermining step because it will determine how fast the reaction
forms products, no matter how fast the other steps are. In the above
reaction, the first step is the slower step, therefore, it is the ratedetermining step for the reaction 2H 2 O 2 0 2H 2 O ϩ O 2 .
Chapter 16 Review
12. Discuss two possible ways to determine the average rate of the
following reaction in the laboratory. What quantities would you
measure in each case?
H 2 (g) ϩ I 2 (g) 0 2HI(g)
13. In the reaction A ϩ B 0 C, the concentration of A decreases
from 6.27 ϫ 10 Ϫ2 mol/L to 4.75 ϫ 10 Ϫ2 mol/L in a span of
125 s. What is the rate of the reaction in terms of reactant A?
14. The collision theory says that particles must collide in order to
react. What other two requirements must be met in order for
particles to react?
15. Explain why increasing the concentration of a reactant usually
increases the rate of a chemical reaction.
16. The rate law of the reaction Q ϩ R 0 QR is rate ϭ k[Q] 2 [R].
How will the rate of the reaction change if [Q] is doubled?
Explain.
17. Explain how the rate-determining step of a complex reaction
controls the overall reaction rate.
168 Chemistry: Matter and Change
Solving Problems: A Chemistry Handbook
SOLVING PROBLEMS:
A CHEMISTRY HANDBOOK
CHAPTER 16
The IO Ϫ ion is called an intermediate in the reaction. An intermediate is an atom, an ion, or a molecule produced in one step of a
reaction and consumed in a later step. In a complex reaction, one
step is always slower than the others. This step is called the ratedetermining step because it will determine how fast the reaction
forms products, no matter how fast the other steps are. In the above
reaction, the first step is the slower step, therefore, it is the ratedetermining step for the reaction 2H 2 O 2 0 2H 2 O ϩ O 2 .
Chapter 16 Review
12. Discuss two possible ways to determine the average rate of the
following reaction in the laboratory. What quantities would you
measure in each case?
H 2 (g) ϩ I 2 (g) 0 2HI(g)
13. In the reaction A ϩ B 0 C, the concentration of A decreases
from 6.27 ϫ 10 Ϫ2 mol/L to 4.75 ϫ 10 Ϫ2 mol/L in a span of
125 s. What is the rate of the reaction in terms of reactant A?
14. The collision theory says that particles must collide in order to
react. What other two requirements must be met in order for
particles to react?
15. Explain why increasing the concentration of a reactant usually
increases the rate of a chemical reaction.
16. The rate law of the reaction Q ϩ R 0 QR is rate ϭ k[Q] 2 [R].
How will the rate of the reaction change if [Q] is doubled?
Explain.
17. Explain how the rate-determining step of a complex reaction
controls the overall reaction rate.