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I was wondering if it is correct to calculate the Gibbs free energy of reaction at $P = \pu{1 atm}$ and $T = \pu{1100 K}$ using the NIST-JANAF thermochemical tables. For example, for the reaction of ammonia and nitrous oxide:

$$\ce{NH3(g) + 1.5 N2O(g) -> 2 N2(g) + 1.5 H2O(g)}$$

Can I later use this result to calculate the electric potential knowing the amount of electrons transferred?

I'm no electrochemist, I'm just trying to estimate the open circuit voltage for a fuel cell.

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    $\begingroup$ You should always be able to compute open-circuit potentials from free energies. I gather you know this and are asking about the appropriateness of your approach for computing free energies. Is that what your question really is? $\endgroup$
    – Curt F.
    Jul 15, 2019 at 17:51
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    $\begingroup$ Yes, I am familiar with the formula and learnt how to use it. I would like to know if the way I am computing the free energies is correct. $\endgroup$ Jul 16, 2019 at 14:49

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