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The concept of second order kinetics, focusing on the time-dependence of a second order reaction, the integrated rate law, and the relationship between initial concentrations and half-life. It also covers specific examples of SN2 reactions and their rate laws, as well as the significance of the NO-O2 reaction.
Typology: Study notes
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A second order reaction in component A has a time-dependence given by d[A]/dt = -k[A] 2 The integrated rate law is given by
2 [Α] 0 [Α]
0 t
0
This can be expressed as [A] = [A] 0 /(1 + [A] 0 kt)
The half life, τ 1/ occurs when [A]= [A] 0 /
0
0
1 / 2
1 / 2
0 For a second order process, the half life depends on the initial concentration [A] 0 .
The time course for the appearance of product is given the integrated rate law: Note that the half-life for a second order process depends on the initial concentration of A and B.
0
0 1 – exp{([ B ] 0
0 ) kt } [ A ] 0
0 exp{([ B ] 0
0 ) kt }
N
The net effect of a S N 2 reaction is that a leaving group is displaced by an attacking group (nucleophile). The process is inherently second order since the nucleophile must collide with the substrate in the rate-limiting step (labeled as slow above).
N
The reaction of NO with O 2
. The reaction is important since the ratio of is a crucial indicator of health. If this ratio is > 4 an individual is healthy. As this ratio falls to < 1 it indicates poor health.