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Reaction Order
Differential Rate Law
Integrated Rate Law
Linear Form
Characteristic
Kinetic Plot
Halflife
Expression
Units of
Rate Constant
Zero

d [A]
d t
= rate = k
[A] = [A]_{0}  k t
[A] = k t + [A]_{0}
[A] vs t
t_{½} =
[A]_{0}
2k
mole L^{1} sec^{1}
First

d [A]
d t
= rate = k [A]
[A] = [A]_{0} e^{ k t}
ln[A] = kt + ln[A]_{0}
ln [A] vs t
t_{½} =
ln(2)
k
sec^{1}
Second

d [A]
d t
= rate = k [A]^{2}
[A] =
[A]_{0}
1 + k t [A]_{0}
1
[A]
= k t +
1
[A]_{0}
1/[A] vs t
t_{½} =
1
k[A]_{0}
L mole^{1} sec^{1}
The series of three graphs shown below illustrate the use of the characteristic kinetic plots.
The graph on the left shows [A] vs t plots for a zeroorder (red line),
firstorder (green line), and secondorder (blue line) reaction.
The graph in the middle shows ln [A] vs t plots and the graph on the right shows 1/[A] vs t plots for each reaction order.