Name _____________________
1. You are trying to determine the rate law for the reaction A  Products. You measure [A] t
at 5 s intervals for 20 s (the data is shown in the table below. You will need to construct three graphs to determine if the reaction is zero, first or second order with respect to A. a) For a zero order reaction a graph of _________ versus
____________ will be a straight line. The slope of the line is equal to _________. b) For a first order reaction a graph of _________ versus
____________ will be a straight line. The slope of the line is equal to _________. c) For a second order reaction a graph of _________ versus
____________ will be a straight line. The slope of the line is equal to _________.
2. In order to determine experimentally determine the activation energy of a reaction, what variables should be plotted against each other?
3. The following data were collected for a reaction of type: A 
Complete the last two columns and determine graphically what the order for this reaction is
Time (s) [A] (M) ln[A] 1/[A]
10
15
20
0
5
1.00x10
-3
6.07x10
-4
3.68x10
-4
2.23x10
-4
1.35x10
-4
1

a) What is order with respect to A? b) Explain why you concluded this c) What is the rate constant for the reaction? (D on’t forget the units)
4. Consider the initial rate data below
.
a) Determine the order with respect to F
2
(show your calculations) b) Determine the order with respect to the ClO
2
(show your calculations) c) What is the overall order of the reaction? d) Determine the value of k in the experiments and pay attention to the units e) Write the overall rate law for the reaction f) Could this reaction occur in one elementary step? Explain g) What would the initial rate be if [F2] = 0.30 M and [ClO
2
] = 0.30 M?
2

5. Decomposition of NO
2
Cl
Below is a proposed mechanism for this reaction
NO
2 k
1
Cl ( g )
®
NO
2
( g )
+
Cl ( g ) (slow)
NO
2 k
2
Cl(g)
+
Cl ( g )
®
NO
2
( g )
+
Cl
2
( g ) (fast)
Overall reaction _________________________________________________
Reactive intermediate(s) __________________________________________
Overall Rate Law ________________________________________________
Write an expression for the rate in terms of

[NO
2
Cl] and
 t
The overall rate law is found experimentally to be
Rate = k
1
[NO
2
Cl]
Does the above mechanism agree with the experiment? __________________
3

6. Synthesis of Hydrogen Iodide from hydrogen and iodine
Below is the proposed mechanism for this reaction
Overall reaction _________________________________________________
Write an expression for the rate in terms of

[I
2
] and
 t
Reactive intermediate(s) __________________________________________
Overall Rate Law ________________________________________________
The overall rate law is found experimentally to be
Rate = k[I
2
][H
2
]
Does the above mechanism agree with experiment? _____________________
If the mechanism does agree with the experimental rate law, how does k relate to k
1
, k
-1
and k
2
?
4

7. Synthesis of bromoacetone
Below is the proposed mechanism for bromoacetone
Overall reaction _________________________________________________
Reactive intermediate(s) __________________________________________
Overall Rate Law ________________________________________________
Write an expression for the rate in terms of

[Br
2
] and
 t
The overall rate R is found experimentally to be consistent with the following rate law
Does the above mechanism agree with experiment? _____________________
If so how does k relate to k
1
, k
-1
and k
2
?
5

8. What is the integrated rate law for the concentration of a reactant A when the reaction is second order in A?
( a )
[
1
A ]
( d ) [ A ] t t
= kt
+
1
[ A ]
= kt
+ [ ]
0
; ( b )
1
[ A ] t
= kt
+
0
; ( e ) ln[ A ] t
1
[ A ]
0
; ( c ) ln[ A ] t
= kt
+ ln[ A ]
0
;
= kt
+ ln[ A ]
0
;
9. The data below were collected for the following first-order reaction:
N
2
O
5
( g )
NO
3
( g )
NO
2
( g )
Temperature (K) Rate Constant (1/s)
800 3.24x10
-5
900
1000
1100
0.00214
0.0614
0.955
A graph of ln(Rate Constant) versus 1/Temperature gives a straight line graph of slope = -30189K and an intercept of 29.967 a) What is the activation energy E a for this reaction? (don’t forget the units) b) What is the collision factor A for this reaction? (What are the units for A assuming that the reaction is first order?) c) What would be the value for the rate constant at 555 o C?
6