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Announcement Regarding Recitations
Ë
Recitations will begin on Monday, January 14
instead of Tuesday, January 15,
as previously announced on the Schedule of Courses and in class.
Ë
Recitations on Monday, January 21 will not meet because of the MLK holiday. However,
students in Monday recitation sections may attend any other recitation section during
the week of January 21.
Learning Objectives 1/10/08
You should
1. understand that integration of rate laws yields expressions for reactant concentrations
as a function of time for zeroth, first, and secondorder reactions.
2. be able to apply integrated rate law equations to determine the rate constant for a
reaction from the time dependence of reactant or product concentration and to pre

dict the concentration of reactant remaining or product formed specified times using a
rate constant.
3. be able to apply graphical methods to determine the reaction order and rate constant
from concentration data collected as a function of time.
4. know how to find halflife(
t
1
ê
2
) expressions for zeroth, first, and secondorder reactions.
5. know what the halflife(
t
1
ê
2
) for a firstorder reaction represents, how
t
1
ê
2
is related to
the first order rate constant
k
, and how
t
1
ê
2
can be determined graphically from a plot
of reactant concentration vs. time.
2
ProblemMethod of Initial RatesLoose ends from 1/8/08
In the reduction of nitric oxide by hydrogen:
2 NO
+
2 H
2
ö
N
2
+
2 H
2
O
three experiments were done using different initial concentrations
Experiment
[NO], M
[H
2 ], M
Observed Initial Rate,
mol N
2 L

1
s

1
1
5.0
μ
10

4
5.0
μ
10

4
2.5
μ
10

5
2
5.0
μ
10

4
1.0
μ
10

3
5.0
μ
10

5
3
1.0
μ
10

3
1.0
μ
10

3
2.0
μ
10

4
General rate law equation: Rate
=
k
@
NO
D
m
@
H
2
D
n
(a) Find order with respect to NO.
m
=
2
(b) Find order with respect to H
2
.
5.0
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 Spring '08
 A.POLLOCK

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