## 9.53 Homework Problem

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

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

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

Samantha Jimenez 4k
Posts: 29
Joined: Fri Sep 28, 2018 12:21 am

### 9.53 Homework Problem

9.53 Calculate the change in molar Gibbs free energy for the process NH3(l) S NH3(g) at 1 atm and (a) 15.0 C; (b) 45. C (see Tables 8.3 and 9.1). In each case, indicate whether vaporization would be spontaneous.

I'm confused as to how would we approach this question? Would we just be getting values from tables and then using the Gibbs free energy equation?

PranitKumaran1F
Posts: 30
Joined: Thu Nov 08, 2018 12:17 am

### Re: 9.53 Homework Problem

You would have to find the standard reaction entropy and enthalpy of the reaction using the values from the tables given for each compound in the reaction. Then you would use the different T values along with the calculated deltaS and deltaH values to find the Gibbs free energy if the reaction using the Gibbs free energy equation. If deltaG < 0 then vaporization is spontaneous at that temperature.