BIO1011 Lecture Notes - Lecture 11: Endergonic Reaction, Exergonic Process, Enthalpy

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11 May 2018
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GIBB’S FREE ENERGY
Molecules contain different atoms which are held together by specific internal chemical
bonds
Each of these bonds has a particular amount of energy associated with it
Every molecule has a certain level of internal energy
which depends on the molecule and the bonds within it
When a chemical reaction takes place, bonds are
broken and new bonds are formed - consequently,
reactants have a different internal energy to products.
If you have a jar of glucose, over time it will
spontaneously degrade into CO2 and H2O.
Energy will be released because the total amount of
energy maintained in bonds is higher in glucose than
CO2 and H2O.
Glucose has a higher enthalpy while CO2 and H2O have a higher entropy.
-Enthalpy = overall amount of energy
-Entropy = amount of freedom or randomness in a system
It is generally the case that larger, more ordered molecules have a higher free energy
and smaller more chaotic molecules have a lower free energy.
Chemical reactions are associated with a change in free energy
If the products of a reaction have a higher energy content than the reactants, then
energy has to be put into the system to drive the reaction (pushing it uphill)
If the products of a reaction have a lower energy content than the reactants, then energy
can be obtained from the system as the reaction takes place (flowing downhill)
Energy releasing reactions are EXOTHERMIC or EXERGONIC
Energy demanding reactions are ENDOTHERMIC or ENDERGONIC
The difference in energy between reactants and products is referred to as ΔG, Gibb’s
Free Energy.
If the ΔG value is negative the reaction is spontaneous, and if it is positive it requires an
energy input
Exergonic Endergonic
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