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Transcript of HCC_Presentation1a
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Reaction Order in General Chemistry and SN1 and SN2 Mechanisms in Organic Chemistry.
Present by: Professor Ambrose Okpokpo
Present to: Members of Houston Community College North West Campus Interviewing Committee
Chair of Committee: Dr. Emmanuel Ewane
Interview Presentation Room: Spring Branch Campus Room 517
Date of Presentation: Friday 15th, 2013 Time of Presentation: 1: 35 P.M.
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Acknowledgment and thanks
• I extend my greetings and thanks for giving me such a rare opportunity to be interviewed by all the distinguished faculties and committee selected for this occasion by the Houston Community College.
• I am truly grateful to be selected for this interview.
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The Rate Law and Order of Reaction
The rate law expresses the relationship of the rate of a reaction to the rate constant and the concentrations of the reactants raised to some powers.
aA + bB cC + dD
Rate = k [A]x[B]y
Reaction is xth order in A
Reaction is yth order in B
Reaction is (x +y)th order overall
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The Overall Order of a reaction is the sum of the individual orders:
Rate (Ms-1) = k [A][B] 1/2[C]2
Overall order: 1 + ½ + 2 = 3.5 = 7/2
or seven-halves order
note: when the order of a reaction is 1 (first order) exponents is written.
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First-Order Reactions
A product rate = -D[A]
Dtrate = k [A]
k = rate
[A]= 1/s or s-1
M/sM
=
D[A]
Dt= k [A]-
[A] is the concentration of A at any time t[A]0 is the concentration of A at time t=0
[A] = [A]0e−kt ln[A] = ln[A]0 - kt
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Second-Order Reactions
A product rate = -D[A]
Dtrate = k [A]2
k = rate
[A]2= 1/M•s
M/sM2
=D[A]
Dt= k [A]2-
[A] is the concentration of A at any time t[A]0 is the concentration of A at time t=0
1
[A]=
1
[A]0
+ kt
t½ = t when [A] = [A]0/2
t½ =1
k[A]0
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Zero-Order Reactions
A productrate = -
D[A]
Dtrate = k [A]0 = k
k = rate
[A]0= M/s
D[A]
Dt= k-
[A] is the concentration of A at any time t[A]0 is the concentration of A at time t = 0
t½ = t when [A] = [A]0/2
t½ =[A]0
2k
[A] = [A]0 - kt
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Orientation factors into the equation and/or reaction
The orientation of a molecule during collision can have a profound effect on whether or not a reaction occurs.
Some collisions do not lead to reaction even if there is sufficient energy.
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SN1 and SN2 Structure-Reactivity-Electrophile
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SN1 and SN2 Structure-Reactivity-Electrophile
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SN1 and SN2 Structure-Reactivity-Electrophile
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SN1 and SN2 Structure-Reactivity-Electrophile
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SN1 and SN2 Structure-Reactivity-Nucleophile
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SN1 and SN2 Structure-Reactivity-Electrophile
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SN1 and SN2 Structure-Reactivity-Nucleophile
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SN1 and SN2 Structure-Reactivity-Nucleophile
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SN1 and SN2 Structure-Reactivity-Nucleophile
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SN1 and SN2 Structure-Reactivity-Nucleophile
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SN1 and SN2 Structure-Reactivity-Nucleophile