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In thermodynamics, the Gibbs free energy (IUPAC recommended name: Gibbs energy or Gibbs function; also known as free enthalpy[1] to distinguish it from Helmholtz free energy) is a thermodynamic potential that measures the "useful" or process-initiating work obtainable from a thermodynamic system at aconstant temperature and pressure(isothermal, isobaric).

So is gibbs free energy only valid for constant pressure and temperature?

I tried to find change in gibbs free energy of a chemical reaction under these conditions and it always comes zero.

ΔG = ΔH - TΔS ..... temperature is constant

ΔG = ΔH - TΔH/T..... at constant pressure q = ΔH

ΔG = 0

there is something wrong in this as reactions do happen at constant pressure and temperature adn gibbs free energy change is not zero

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# Confused about gibbs free energy

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