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Summary Exam notes
- Module
- Pharmacy - Physical pharmacy
- Institution
- University Of East Anglia
Pharmacy - physical pharmacy 1st and 2nd semester summaries Bullet points, key notes, images and diagrams
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Kinetics 1 Kinetic stability is energy barrier between product and reactants
Transition state is the high energy state between reactants and products
Reaction aA+bBcC+dD
Rate v=-1/a d[A]/dt
Measuring rate of reactions:
Quenching-stopping the reaction after sampling
Immersion probe-continuous monitoring
Flow- continuous flow of reactants into mixing chamber with spectrometer
Stopped flow- flow stopped after given volume with spectrometer
Rate v=k[A]α[B]β
Elementary reactions: single step, molecularity is unimolecular or bimolecular
Arrhenius equation plot lnk vs 1/T so lnk=C+mx1/T or lnk=lnA-Ea/RT
C=lnA and m=-Ea/R (how many molecules have the energy to react
Kinetics 2
First Order- reaction rate is proportional to concentration v=k[A]=-d[A]/dt
-ln[A]+C=kt or C=ln[A]0
Linear equation ln[A]=ln[A]0-kt where C=ln[A]0 and m=-k (ln[A] vs T)
[A]=[A]0e-kt
First order half life t1/2=ln2/k
Zero Order- reaction is independent of reaction concentrations v=k= -d[A]/dt
-[A]+C=kt or C=[A]0
Linear equation [A]=[A]0-kt where C=[A]0 and m=-k ([A] vs T)
Zero Order half life t1/2=[A]0/2k
Second Order v=k[A]2 or v=k[A][B]
1/[A]+C=kt or C=-1/[A]0
1/[A]=kt+1/[A]0 where C=1/[A]0 and m=k (1/[A] vs T)
[A]=[A]0/kt[A]0+1 ([A] vs T)
Second order half life t1/2=1/k[A]0
Kinetics 3
Isolation method using pseudo order reactions
Non-integer orders are possible for complex reactions and some don’t have
orders
Steady state approximation- assume concentration of intermediate doesn’t
change
Pharmaceutical Solutions
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