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Lecture notes

Kinetics

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  • January 30, 2024
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  • 2022/2023
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Kinetics- what is rate and why do we care?
Why do we care about kineti cs (in biology)?

Biochemical reactions- e.g. Enzymes

 Metabolic differences- people, different species → treat diseases
 Engineering biochemical reactions

Receptor-ligand interactions

 Which things bind faster/ slower? Why?
 People, different species → understand and treat disease

What happens to drugs in body?

 Where do they go?
 How quickly they absorbed, distributed, metabolised, excreted (ADME)?
 Drug effectiveness and toxicity

What is rate and why measure it?

 Rate- change in something with respect to time
- e.g. Speed= Distance/ Time or m/s
 In biology- amount, concentration or location change with respect time
-e.g. mmol/s, mmol-1dm-3min-1, μM min-1… etc
 ‘Thermodynamics’- tells us whether reaction can process spontaneously but doesn’t inform us about rate at
which reaction will proceed
- This information must be obtained experimentally

How do we measure reacti on rates?

Some form of change in product/reactant with time?

 Spectroscopic- e.g. absorbance, fluorescence
 Temperature changes- e.g. ITC
 Mass changes- e.g. SPR
 Conductivity
 Electrochemical

For very fast reactions- used stopped flow or quench flow

 Stopped flow continuous- Quench flow, discontinuous

Rates in context of equilibria

 For unimolecular reaction or protein and
ligand interaction:
 At equilibrium:

But how quickly do we get to equilibrium? Even at equilibrium- reaction hasn’t stopped. We use rate constants (k)
to tell us how quickly each reaction can occur:

Define rate constant of forward reaction as k1 and reverse reaction as k-1
small k is used for rate constant. Big K is used for equilibrium constant

 For unimolecular reaction- converted from A to products
 How quickly does amount of [A] changes?
 Rate at which A is converted to products is proportional to concentration
of A and rate constant k where x= order

, If we measure change in [A] over ti me for this reacti on:




This example follows zero order kineti cs

For zero-order kinetics- rate of reaction is independent of concentration of reactants
Reaction rate is constant- regardless of concentration of reactants present

Why? What does it mean?

X= order, which here= 0. Therefore:



Through the rearrangement and integration, equation of line:

Ethanol Metabolism exhibits zero order kineti cs




If we plot rate as functi on of concentrati on for zero order reacti on




Many reacti ons are dependent on concentrati on

For unimolecular reaction dependent on concentration:

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