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IS gibbs free energy change at constant pressure zero?

ΔS = q / T. At constant pressure q = ΔH so ΔS = ΔH / T

So ΔG = ΔH - ΔH/T . T

= 0

I think i am wrong but where? My friend tells me that q involved in enetropy is different from the one we consider in ΔH. I dont understand this. IS heat due to entropy different from the one involved in enthalpy change

I'm all messed up

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# Gibbs free energy change at constant pressure is zero?

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