BIOC 2300 Lecture Notes - Lecture 17: Exergonic Reaction, Equilibrium Constant, Chemical Equilibrium
Thermodynamics, Control of Directionality and Flux
February 24, 2016
Thermodynamics – energy changes in metabolic pathway
• Endergonic vs exergonic
• Energy needed/released
Directionality – reaction proceeds in a specific direction
• How is direction achieved?
Flux – rate of the overall pathway
• Substrate product
Gibb’s Free Energy:
• H = enthalphy (energy) * favoured if change is negative
• S = entropy (disorder) * favoured if change is positive
• Reaction is spontaneous of Gibb’s Free Energy is decreased
• (change of)G = (change of)H – T(change of)S
The chemical equilibrium is dynamic
• system is at equilibrium when forward and reverse reactions are equal
• does not mean the products and substrates have the same concentration
• Keq = equilibrium constant
o K = [C][D] / [A][B]
• Standard free energy change: G’ = - RT ln Keq *know for exam
o force when all reactants are present at equal concentrations equilibrium state
o set characteristic of the reaction; driving force
o R – gas constant *do not need to memorize
o T – temperature
G’ reflects the free energy change for a system with standard concentration to react
equilibrium
• Keq is inherent property
• A reaction with K=3 is as equilibrium when there is 3 times as much product as substrate
• Standard conditions are defined as 1M for all reactants
• G’ described for of a system moving from its standard conditions to equilibrium
G’ is defined as G under standard conditions.
• T = 298K = 25C
• Pressure = 1 atm
• Concentration of reactant = 1 M
• pH = 7.0
• water concentration = 55.5 M
G’ can be calculated from Keq
• G’ = -RT ln K
• Ex 1. What is G’ is K=3
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