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Chemistry for Biology Students (CHEM0010) Notes - Chemical and Enzyme Kinetics CA$12.11   Add to cart
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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...

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Document information

  • November 30, 2023
  • 17
  • 2020/2021
  • Class notes
  • Professor andrea sella
  • All classes

Subjects

  • rates of reaction
  • measuring rates
  • mechanisms
  • temperature
  • diffusion
  • catalysis
  • enzyme kinetics

Written for

  • University College London (UCL)
  • Unknown
  • Chemistry for Biology Students (CHEM0010)
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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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