1. Reaction Rates
I. Expressing Reaction Rates
-________ ____, or the ____ at which
a _________ ________ occurs, is
expressed in terms of ______ in ____________ of a ________ or
_______ per unit ____
What is the reaction rate of the following reaction, in moles/liter·second, if the concentration of NO is moles/liter at t1 = 0.00 seconds and moles/liter 2 seconds after the reaction begins?

2. Reaction Rates
I. Expressing Reaction Rates
-________ ____ can be expressed as
the ____ at which a ________ is
produced or the ____ at which a
________ is consumed
What is the reaction rate of the following reaction, in moles/liter·second, if the concentration of C4H9Cl is 0.220M at t1 = 0.00 seconds and M 4.00 seconds after the reaction begins?

3. Reaction Rates
I. Expressing Reaction Rates
What is the reaction rate of the following reaction, in moles/liter·second, expressed in moles of H2 consumed, if the concentration of H2 is 0.030M at t1 = 0.00 seconds and 0.020M 4.00 seconds after the reaction begins?

4. Reaction Rates
I. Expressing Reaction Rates
What is the reaction rate of the following reaction, in moles/liter·second, expressed in moles of HCl produced, if the concentration of HCl is 0.000M at t1 = 0.00 seconds and 0.020M 4.00 seconds after the reaction begins?

5. Reaction Rates
Name__________________
I. Expressing Reaction Rates
What is the reaction rate of the following reaction, in moles/liter·minute, expressed in moles of H2O2 consumed, if the concentration of H2O2 is 2.50M at t1 = 0.00 minutes and 2.12M 2.00 minutes after the reaction begins?
2H2O2
1O2 +
2H2O

6. Reaction Rates
I. Expressing Reaction Rates
What is the reaction rate of the following reaction, in moles/liter·minute, expressed in moles of O2 produced, if the concentration of H2O2 is 1.82M at t1 = 0.00 minutes and 1.48M 5.00 minutes after the reaction begins?
2H2O2
1O2 +
2H2O

7. Reaction Rates
II. The Collision Theory
-the _________ ______ states that, in
order for a ________ ________ to take
place, the ______, ____, or _________
must _______ in order to _____

8. Reaction Rates
II. The Collision Theory
-according to the _________ ______,
___ and ___ molecules must _______ in
order to _____, but in the reaction of
______ ________ and ________ ______,
only a _____ _______ of the _________
produce ________. ____

9. Reaction Rates
II. The Collision Theory

10. Reaction Rates
II. The Collision Theory

11. Reaction Rates
II. The Collision Theory
-according to the _________ ______,
the _________ of ________ _________
must __ _______, __ _______ with the
correct ___________, and __ _______
with sufficient ______ to form the
_________ _______

12. Reaction Rates
II. The Collision Theory
-the minimum amount of ______ that
reacting particles must have to form the
________ _______ is called the
________ ______, or ___
-a ____ _________ ______ means that
relatively ___ __________ will have
sufficient ______ to produce the
_________ _______, while a ___
_________ ______ means that _____
__________ will have the required _____ to form the __________ _______, and the
_______ ____ will be ______

13. Reaction Rates
II. The Collision Theory
-once ________ ______ has been
supplied to the ________, if the ________
end up lying at a _____ ______ _____
than the _________, then ______ is
________ by the _______, and the ______
is __________
-if the ________ end up lying at a _______
______ _____ than the _________, then
______ is ________ by the _______, and
the ________ is __________

14. Reaction Rates
III. Factors Affecting Reaction Rates
A. The Nature of the Reactants
-one factor that affects the ____
of chemical _________ is the
________ _______ of the
________

15. Reaction Rates
III. Factors Affecting Reaction Rates
B. Concentration
-when the _____________ of the _________
is _________, reactions ______ ___
-since _________ is necessary for _________ _________ to take place, __________ the
____________ of the ________ _________
increases the likelihood that the _________
of one ________ will _______ with the
_________ of the other _________

16. Reaction Rates
III. Factors Affecting Reaction Rates
B. Concentration

17. Reaction Rates
III. Factors Affecting Reaction Rates
C. Surface Area
-if the _______ _____ of the _____ _____ of
reactant is _________ by _________ particle
_____, the _______ ____ will ________, since
the greater ________ _____ allows the
_________ of one ________ to _______ with
_____ particles of the other ________ per unit
time

18. III. Factors Affecting Reaction Rates
D. Temperature
-__________ the ___________ at which a
_______ occurs _________ the _______ ____
-__________ the ___________ _________ the
average _______ _____ of the _________ that
make up a substance, causing the ________ to
_______ more ___________
According to the curve of the graph, what temperature increase, in Kelvin, doubles the rate of reaction? _______K
At what Kelvin temperature is the relative reaction rate 25?
_______K 40 35
Temperature (in K)
Relative Reaction
Rate 30 25
Relative Reaction Rate 20 15 10 5
280
290
300
310
320
330
Temperature (in K)

19. Reaction Rates
III. Factors Affecting Reaction Rates
D. Temperature
-__________ the ___________ also ________ the ____ of _______ by _________ the
_______ of _________ with _________
________ ______ to cause a _______
-__________ the ___________, then, _______
the _______ ____ by _________ the
_________ _________ and the _________
______

20. III. Factors Affecting Reaction Rates
E. Catalysts
-_________ are __________ that _______ the
_____ of ________ without being _________ by
the ________
Substrate (Reactant)
-________ are _________ ________ which cause
_________ to happen or happen ______ without
_______ the __________, which could ________
living things by __________ their ________
Enzyme
-________ increase ________ ____ by ________
the _________ ______ for a _________, so that
________ that had ____________ energy before
now have _________ energy to ______
-_________ make reactions _____ likely to _______ by ________ the __________ ______

21. Reaction Rates
III. Factors Affecting Reaction Rates
1. Hypothesis:
2. Prediction:
3. Gather Data:
A. Safety:
B. Procedure:

22. Reaction Rates
III. Factors Affecting Reaction Rates
3. Gather Data:
B. Procedure:

23. Name_________________
Reaction Rates
Name_________________
III. Factors Affecting Reaction Rates
3. Gather Data:
B. Procedure:
Temperature (in °C)
Mass of Tablet (in g)
Reaction Time (in s)
Reaction Rate (in g/s)
4. Analyze Data:

24. III. Factors Affecting Reaction Rates
4. Analyze Data:
0.10
0.09
0.08
0.07
0.06
Relative Reaction Rate (in g/s)
0.05
0.04
0.03
0.02
0.01
0.00 10 20 30 40 50 60 70 80 90
100
Temperature (in °C)

25. Reaction Rates
III. Factors Affecting Reaction Rates
4. Analyze Data:

26. Reaction Rates
III. Factors Affecting Reaction Rates
5. Draw Conclusions:
________________________________________________________________________________

27. Reaction Rates
IV. Reaction Rate Laws
-when we divide the ________ in _______
____________, __________ by the
_______ in _____, ____, we get an
________ ________ _____
-chemical reactions tend to _____ _____ as
________ are _________, because in order
for a reaction to proceed, _________ must
_______, and as _________ are _________
there are ______ ________ left to _______

28. Reaction Rates
IV. Reaction Rate Laws
-_____ ______ ________ the results of the
_________ _______ in terms of a
____________ ___________ between the
_____ of a _________ ________ and the
________ _____________
-in the reaction __ ___ __, there is only ___
_________ _______ between the ________
and ________, so the _____ ____ for the
reaction is _____ = __ ____, where ____ is
the _____________ of the _________ __
and __ is the _____________ __________ _________ ____ ________, which depends
on _________ _________, especially the
___________
-the ________ _____, then, is _________
_____________ to the _____________

29. Reaction Rates
V. Reaction Orders
-in the reaction __ ___ __, the _____ = __ ___,
and it is understood that ____ means the same
as ____, and the _________ __ is the ________
______
-the _____ ____ for the _____________
of _____ is _____ = __ ______, and the
________ is said to be _____ _____ in _____
-for _________ with _____ than _____
_______, the _____ ____ is
_____ = __ ____ ____
where __ is the _______ _____ for __ and __ is
the _______ _____ for __

30. Reaction Rates
V. Reaction Orders
-for the ________ that has the _____ ____
_________________, the reaction is described
as _______ _____ in ___, _____ _____ in ___,
and _____ _____ overall
-an ___________ _______ of evaluating
________ ______is the _______ of _______
______, in which the ______________ of the
_________ are _______ and the effect on the
________ _____ is observed

31. Reaction Rates
V. Reaction Orders
-the _____ ____ for this type of reaction is
_________________. From the data, you can
see that, while ____ was held constant, the
________ _____ has ________ in Trial 2
compared to Trial 1, at the same time ____ has
________, so the ________ ______ __ must
equal __, or because ___ = __, __ = __
-in Trial 3 compared to Trial 2, ____ is
_______, and the _______ ____ ___________,
so the ________ ______ __ must equal __, or
___ = __, and the _______ _____ ____ is
_________________
and the _______ ________ ______ is ______ _____ _______

32. Reaction Rates
V. Reaction Orders
Given the following experimental data, use the method of initial rates to
determine the rate law for the reaction and the overall reaction order.

33. Reaction Rates
V. Reaction Orders
Given the following experimental data, use the method of initial rates to
determine the rate law for the reaction and the overall reaction order.

34. Reaction Rates
V. Reaction Orders
Given the following experimental data, use the method of initial rates to
determine the rate law for the reaction, the overall reaction order, and the
value of the specific rate constant.

35. Name__________________
Reaction Rates
Name__________________
V. Reaction Orders
Given the following experimental data, use the method of initial rates to
determine the rate law for the reaction, the overall reaction order, and the
value of the specific rate constant.
2ClO2(aq) +
2OH-(aq)
1ClO3- +
1ClO2- +
1H2O(1)
Trial
Initial [ClO2] (in M)
Initial [OH-] (in M)
Initial Rate (in mol/L·min) 1
0.0500
0.200
6.90 2
0.100
0.200
27.6 3
0.100
0.100
13.8

36. value of the specific rate constant.
Reaction Rates
V. Reaction Orders
Given the following experimental data, use the method of initial rates to
determine the rate law for the reaction, the overall reaction order, and the
value of the specific rate constant. A + B 2C
Trial
Initial [A] (in M)
Initial [B] (in M)
Initial Rate (in mol/L·s) 1
0.010
0.010
0.0060 2
0.020
0.010
0.0240 3
0.020
0.020
0.0960

37. value of the specific rate constant.
Reaction Rates
V. Reaction Orders
Given the following experimental data, use the method of initial rates to
determine the rate law for the reaction, the overall reaction order, and the
value of the specific rate constant. A + B
products
Trial
Initial [A] (in M)
Initial [B] (in M)
Initial Rate (in mol/L·hr) 1
0.010
0.020
0.020 2
0.015
0.020
0.030 3
0.015
0.040
0.240

38. Reaction Rates V. Reaction Orders
A chemical reaction involving compound A and compound B as reactants is found to be first order in A and second order in B. What will the reaction rate be for Trial 2?
Trial
Initial [A] (in M)
Initial [B] (in M)
Initial Rate (in mol/L·s) 1
1.0
0.20
0.10 2
2.0
0.60 ?

39. Reaction Rates
V. Reaction Orders
-most _________ _________ obey ____ of
______ _____ ______: _____ _____, _____ _____, or _______ _____, and the ______ of
the _________ _____ ________, __, vary with
the ______ of the ________
-if a ________ with ____ or _____ _________
was ______________ __________ to be _____ ______ _______, the _____ _____ would be
_____________ or ________________
-in ______ ______ reactions, the _____ _____
is _________, and the ______ of __ are
________

40. Reaction Rates V. Reaction Orders Trial Initial [A] (in M)
Initial Rate (in mol/L·s) 1 2 3

41. -plot the data from the table on the graph below:
Reaction Rates
V. Reaction Orders
-plot the data from the table on the graph below:
10.00
9.00
8.00
7.00
6.00
Reaction Rate x (in mol/L·s)
5.00
4.00
3.00
2.00
1.00
0.00
1.00
2.00
3.00
4.00
5.00
6.00
7.00
8.00
9.00
10.00
0.00
Concentration [A] x 10-3 (in mol/L)

42. -if a ________ with ____ or _____ _________
Reaction Rates
V. Reaction Orders
-if a ________ with ____ or _____ _________
was ______________ __________ to be _____ ______ _______, the _____ _____ would be
_____________ or ________________
-in ______ ______ reactions, the _____ _____
is _____________, and the ______ of __ are
____
Trial
Initial [A] (in M)
Initial [B] (in M)
Initial Rate (in mol/L·s) 1 2 3 4

43. -plot the data from the table on the graph below:
Reaction Rates
V. Reaction Orders
-plot the data from the table on the graph below:
10.00
9.00
8.00
7.00
6.00
Reaction Rate x (in mol/L·s)
5.00
4.00
3.00
2.00
1.00
0.00
0.00
1.00
2.00
3.00
4.00
5.00
6.00
7.00
8.00
9.00
10.00
Concentration [A] x 10-3 (in mol/L)

44. -if a ________ with ____ or _____ _________
Reaction Rates
V. Reaction Orders
-if a ________ with ____ or _____ _________
was ______________ __________ to be ______ ______ _______, the _____ _____ would be
_____________ or ________________
-in ______ ______ reactions, the _____ _____
is _______________, and the ______ of __ are
_______
Trial
Initial [A] (in M)
Initial [B] (in M)
Initial Rate (in mol/L·s) 1 2 3 4

45. -plot the data from the table on the graph below:
Reaction Rates
V. Reaction Orders
-plot the data from the table on the graph below:
10.00
9.00
8.00
7.00
6.00
Reaction Rate x (in mol/L·s)
5.00
4.00
3.00
2.00
1.00
0.00
1.00
2.00
3.00
4.00
5.00
6.00
7.00
8.00
9.00
10.00
0.00
Concentration [A] x 10-3 (in mol/L)

46. VI. Instantaneous Reaction Rates -while the ________ _________
_____ gives the ________ _____
over a period of _____, the
____________ _____
shows the ________
_____ at a ________ _____
Time, t (in s)
[C4H9Cl] (in M)
Average rate (in mol/L·s)

47. VI. Instantaneous Reaction Rates -plot the data from the table on the
graph below:
0.10
0.09
0.08
0.07
0.06
[C4H9Cl (in M)
0.05
0.04
0.03
0.02
0.01
0.00
100
200
300
400
500
600
700
800
900
1000
Time (in s)

48. Reaction Rates
VI. Instantaneous Reaction Rates
-as the reaction proceeds, and the
rate of _________ goes _____
as ________ of _________ are
_________, the ______ of the
_____ ________ to the _____
goes _____ as the ________ ____
goes _____

49. Reaction Rates
VI. Instantaneous Reaction Rates
If the following equation is first order in H2 and second order in NO with a rate constant of 2.90 x 102 L2/mol2·s, what is the instantaneous rate when [NO] = M and [H2] = M ?

50. Reaction Rates
VI. Instantaneous Reaction Rates
If the following equation is first order in H2 and second order in NO with a rate constant of 2.90 x 102 L2/mol2·s, what is the instantaneous rate when [NO] = M and [H2] = M ?
2NO +
1H2
1N2O +
1H2O

51. Reaction Rates
VI. Instantaneous Reaction Rates
If the following equation is first order in H2 and second order in NO with a rate constant of 2.90 x 102 L2/mol2·s, what is the instantaneous rate when [NO] = M and [H2] = M ?
2NO +
1H2
1N2O +
1H2O

52. Reaction Rates
VI. Instantaneous Reaction Rates
If the following equation is first order in H2 and second order in NO with a rate constant of 2.90 x 102 L2/mol2·s, what is the instantaneous rate when [NO] = M and [H2] = M ?
2NO +
1H2
1N2O +
1H2O

53. Reaction Rates
VI. Instantaneous Reaction Rates
If the following equation is first order in A and second order in B with a specific rate constant of 4.75 x 10-7 L2/mol2·s, what is the instantaneous rate when [A] = M and [B] = M ? A + B
products

54. Reaction Rates
VII. Reaction Mechanisms
-_____ chemical reactions consist of a
______ of ____ or _____ simpler
_________
-a ________ ________ consists of ____
or _____ ___________ steps
-for example, the _____________ of
______, an _________ of ________, in
the ______ _____ is a ________
________ consisting of ______
___________ _________ in the
following ________ __________:

55. Reaction Rates
VII. Reaction Mechanisms
-because ____ is a _______ in the _____ __________ step and is _________ in
the _____ ___________ step, it
technically _________ the _____ of
_________ without being _________
itself, and so is a _________ to the
_____________ of ______
-because both _____ and ___ are formed in ____ ____________ step of the
_______ ________ and _________ in a
__________ step, they are ___________
1Cl +
1O3
1O2 +
1ClO
1O3
1O2 + 1O
1ClO + 1O
1O2 +
1Cl
2O3
3O2

56. VII. Rate-Determining Step in a Complex Reaction Mechanism
Reaction Rates
VII. Rate-Determining Step in a Complex
Reaction Mechanism
-the _______ elementary step in the ________ __________ of a ________ ________limits the ___________ ____ of the _______ _______, and so is called the ______________ ____
-the elementary step with
the _______ __________
______ is the _______,
and so is the
______________ ____
Energy
Reaction progress