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Life is all about combating the
inevitable increase in Entropy! Two factors determine the
spontaneity of a reaction:
• Enthalpy: ∆ H (or energy released or required)
• Entropy: ∆ S (increase or decrease in order of
system) • The spontaneity of a reaction is
expressed as the Gibbs Free Energy or
∆ G (the energy available to do work) Does this reaction occur?
Does it occur spontaneously?
• Entropy (∆ S) : is it increasing?
• Enthalpy (∆ H): is it giving off heat
energy? ∆ G = ∆ H - T∆ S
∆ G is Gibbs Free Energy Free Energy
• Will the following reaction occur?
C6H12O6 + 6O2 ---> 6CO2 + 6 H2O + energy
∆ G or Gibbs Free Energy is negative for
this reaction - thus it will be spontaneous Gibbs Free Energy
for a spontaneous reaction
∆G = ∆H - T ∆S
exothermic Positive &
More disordered STOP: explain this to a
• See nex...
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