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I read in my textbook that one of the standard conditions we should use when calculating the standard Gibbs free energy is having a concentration of 1 M of all the reagents and the products in the reaction. But if you use the formula $G = -RT\ln K_\mathrm e$ and you use 1 M to calculate it, you would always get zero.

So that means 1 M would be the initial concentration of reagents and products before reaching equilibrium?

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$\Delta G = \Delta G^\circ - RT \ln(K)$

It isn't directly $G$, but formula for change in free energy. Also, in standard conditions $\Delta G = \Delta G^\circ$, so it isn't necessarily 0.

Relevant reading on a website

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  • $\begingroup$ That link helped a lot!! Thank you so much ((: $\endgroup$ – Ewelin Machado Apr 15 '18 at 13:25
  • $\begingroup$ @EwelinMachado If his helped a lot, you can press the V button next to his answer. $\endgroup$ – KYHSGeekCode Apr 15 '18 at 15:29

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