1) 3 s 1. State the rates of
formation and consumption of A, B, and D. (b) The rate law for this reaction was reported as v = kr[A][B][C]
with the molar concentrations in mol dm 3 and the time in seconds. What are the units of kr?
(a) The reaction stoichiometry is used to determine the rates of consumption and formation of the other
participants in the reaction from the known rate of formation of C.
(b) Rearrange the rate law, , to give:
The reaction rate has dimensions of concentration/time and in this case its dimensions are mol dm 3 s1.
The units of the rate constant are therefore:
2) The initial rate of a reaction depended on the concentration of a substance J as follows:
[J]
0
/(mmol dm
3
)
5.0
10.2
17
30
v
0
/(10
7
mol dm
3
s
1
)
3.6
9.6
41
130
Find the order of the reaction with respect to J and the rate constant.
Assume that the initial rate law has the form: . In this form, we can take the natural logarithm of
both sides of the equation to yield: . j is the reaction order. We can then use this
construct the following table:
[J]
0
/(mmol dm
3
)
5.0
10.2
17
30
l
n([J]
0
/(mol dm
3
))
-
5.29
-
4.58
-
4.07
-
3.5
v
0
/(10
7
mol dm
3
s
1
)
3.6
9.6
41
130
l
n(v
0
/(mol dm
3
s
1
))
-
14.83
-
13.85
-
12.40
-
11.25
The plot of ln v0 against ln [J]0 is shown below.
