Chemistry for Biology Students (CHEM0010) Notes - Chemical and Enzyme Kinetics
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Course
Chemistry for Biology Students (CHEM0010)
Institution
University College London (UCL)
Explore Chemistry for Biology Students with these tailored notes, designed for Year 1 students at University College London. Within this document, delve into the intricacies of cell biology, where discussions on rates of reaction, measuring rates, reaction mechanisms, temperature effects, diffusion...
E1: Defining Rates of Reaction
Introduction
Aims and objectives
o Understand the factors that determine how fast reactions
o Understand the dependence of chemical reactions on concentration
o Understand the terms rate law and order for a reaction
o Analyse simple kinetic data
o Use kinetics to infer reaction mechanisms
o Understand the temperature dependence of reaction rates
o Understand the kinetics of simple enzymes
o Distinguish between different kinds of enzyme inhibition
o Understand the mechanisms underlying biological pattern formation and control
Why bother with kinetics?
o Understanding biological issues
How enzymes/proteins work
Rates of binding/release
Inhibition
How drugs behave
How toxins and poisons work
o Understanding complex systems
Oscillating reactions
Population dynamics
Pattern formation
Morphogenesis
o Understanding industrial reactions
Catalysts
Efficiencies
o Understanding global issues
Ozone hole + climate change
Rate of reaction – rate at which reagents are used up and products are formed
o Rate of reaction
Concentration of reactants decrease over time – gradient = -1
Concentration of products increase over time – gradient = +1
o Reaction: R P
o Reaction: 2R P
Because reactants will be used up twice as fast as the product are formed
o General reaction: aA + bB cC + dD
o Empirical rate law and the order of reaction
Reaction rates depend on concentration
Rate ∝ [A]m[B]n
Rate = k[A]m[B]n
Partial orders are m and n
o Reaction is mth order in A
,E1: Defining Rates of Reaction
o Reaction is nth order in B
Overall reaction order = m+n
k = rate constant for the reaction
o Depends only on temperature
o Integrated rate equations
Integrate rate equations to predict the concentration of each component as a function of
time
Zero Order Reactions
Zero order reactions
o Definition
Rate of reaction does not depend on concentration of reagent
o Zero order rate
o
Rate remains constant with time
Concentration decreases linearly with time
o Integrated zero order rate equation
o RadiRa
First Order Reactions
First order reactions
o Definition
Rate of reaction is proportional to the concentration of reagent
o First order rate
, E1: Defining Rates of Reaction
o
o Integrated first order rate equation
o Half-life
t1/2 = time required for the concentration to drop to half its original value
o t1/2 – independent of concentration
o Higher k = lower t1/2
o First order processes
Excretion of drugs and metabolites
Renal excretion of drugs and metabolites follows 1 st order kinetics
o
2 processes – excretion of drugs > drugs converted to metabolites
o k1 and k2
Rate constants for the 2 processes
o a and b
Weighting factors
o
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