Gibbs

• ∆S = S(products) - S(reactants)

  More positive entropy change = more disorder
• Gibb's free energy ∆G = ∆H -T∆S

  ∆G is Gibbs free energy

  ∆H is the enthalpy change is J/mol

  T is temperature in Kelvin

  ∆S is the entropy change measured J/K/mol
• Gibb's free energy is the measure of feasibility of a chemical reaction so 0 is greater than or equal to ∆G
• If 0 is greater or equal to ∆G then the reaction is feasible
• When the reaction is feasible then

  0> ∆H -T∆S which can be T∆S >∆H