## 9.57

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

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

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

Ethan-Van To Dis2L
Posts: 50
Joined: Fri Sep 29, 2017 7:05 am

### 9.57

So, I got the answer for entropy and enthalpy, but when I use the Gibbs Free Energy equation, I get -753.01 X 103 kJ/mol using 298 K when the answer is -713.02 kJ/mol. Is the solution wrong, or am I doing something dumb and can't realize it?

Curtis Wong 2D
Posts: 62
Joined: Sat Jul 22, 2017 3:00 am

### Re: 9.57

In regards to that, essentially, since we know that at standard temperature, it would 298 K. So you would just need to look up the Gibbs Free Energy from the appendix and calculate it from that, not from delta G = Delta H - T * Delta S.