## Delta G for diatomic molecules [ENDORSED]

$\Delta G^{\circ}= \Delta H^{\circ} - T \Delta S^{\circ}$

$\Delta G^{\circ}= -RT\ln K$

$\Delta G^{\circ}= \sum \Delta G_{f}^{\circ}(products) - \sum \Delta G_{f}^{\circ}(reactants)$

Rakhi Ratanjee 1D
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### Delta G for diatomic molecules

Is the Gibbs free energy for diatomic molecules always equal to zero? Why?

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### Re: Delta G for diatomic molecules

It is only 0 if you are looking at the Gibbs Free Energy of formation due to the standard states of Br, Cl, N, O, and F being diatomic. It is the same for standard enthalpy of formation.

Chem_Mod
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### Re: Delta G for diatomic molecules  [ENDORSED]

As discussed in class:

Gibbs Free Energy of formation of F2g means what is the Gibbs free energy for:

F2g ---> F2g which has to be zero because both reactant and product are identical.

Hope this helps.