## 9.103

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

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

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

Dahriel Aron 3A
Posts: 60
Joined: Fri Sep 25, 2015 3:00 am

### 9.103

In question 9.103 it asks
A scientist proposed the following two reactions to produce ethanol, a liquid fuel:

C2H4 (g) + H20 (g) -> CH3CH2OH (l)
C2H6 (g) + H20 (g) -> CH3CH2OH (l) + H2 (g)

Assume standard-state conditions and determine if either reaction is thermodynamically spontaneous.

I initially thought to solve this problem with products-reactants and find which one had a negative delta G, however in appendix 2A there are no values for CH3CH2OH (l) listed and the solutions manual just subtracts 3 large numbers from each other. I was wondering where these numbers come from and what equation is used.

Chem_Mod
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### Re: 9.103

It is listed on page A15 since it is an organic compound.

Tschlener 1E
Posts: 20
Joined: Mon Jan 26, 2015 2:17 pm

### Re: 9.103

I did not find that compound on page A15 and I'm still confused as to why the solutions manual shows products minus reactants, but the reactants were substracted from eachother and not added.

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