## K from delta G at different temperatures

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

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

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

Hannah Markovic 3C
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### K from delta G at different temperatures

Why do you need to calculate delta G from H and S when you're finding K at different temperatures? Why is the value you get from that equation different from using delta G of formation values? This is how the answer key solved 11.83.

Chem_Mod
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### Re: K from delta G at different temperatures

The formation value is the reaction to from the product from its own element in standard state. It it different from the reaction gibbs free energy because they are different reactions

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