## Homework 9.65 6th Edition

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

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

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

Tamera Scott 1G
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### Homework 9.65 6th Edition

For 9.65 in the 6th edition, would you determine if compounds become less stable with respect to the elements as the temperature is raised by looking at their entropy? Or does it have to do with Gibbs free energy?

Grace Kim 1J
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### Re: Homework 9.65 6th Edition

You can use delta S (entropy) to find out whether it is stable or unstable as T increases. Using the equation delta G= delta H - TdeltaS, if delta S is negative, then -TdeltaS will be positive as T increases, resulting in a positive delta G, which causes the compound to be less stable. If delta S is positive, then -TdeltaS will be negative, resulting in a -deltaG, which causes the compound to be more stable.

Hope this helped!

Camille Marangi 2E
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Joined: Fri Sep 28, 2018 12:26 am

### Re: Homework 9.65 6th Edition

It also depends on the sign of enthalpy- if the reaction is exothermic with a positive entropy, the reaction will without a doubt be more stable. If endothermic with a negative entropy the reaction will be less stable. Any variation in these signs are solely dependent on temperature to find the stability.