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Nilanjan Bhowmick AIR 3, CSIR NET (Earth Science)
- IIT JAM
- Chemistry (CY)
For the eqn dg = dg' +rt lnq , at eqlbm dg is taken to be 0 but dg' is not taken to be 0. why so? .
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Dinesh khalmaniya 1 Best Answer
Explaination:- The difference between ∆G and ∆G° is that ∆G is change is Gibbs energy for a reaction at any time, at any conditions we want to find, while ∆G° is change in Gibbs energy of reaction at standard condition( here standard condition means 1 Barr pressure, no comment on temperature), which means that all the reactants and products, are at 1 Barr at than instant. If reaction is at equilibrium(at standard condition), then ∆G° =0. And if ∆G°=0 then ∆G=∆G° wherever ∆G=0 ( i.e. at equilibrium .) Another time when ∆G=∆G° is the moment when Q for any reaction becomes equal to 1, reaction might be at equilibrium or not. check this link https://www.adriandingleschemistrypages.com/ap/making-sense-of-delta-g-and-delta-g-standard-when-it-comes-to-equilibrium/