## 9.69 in Sixth Edition

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

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

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

Alexa Tabakian 1A
Posts: 38
Joined: Fri Sep 28, 2018 12:20 am

### 9.69 in Sixth Edition

What amount (in moles) of ATP could be formed if all the Gibbs free energy released in the oxidation of 3.00 mol NADH were used to generate ATP?

I do not know how to approach this problem given just three equations and delta G. Can anyone help me out?

Sophia Ding 1B
Posts: 62
Joined: Fri Sep 28, 2018 12:16 am

### Re: 9.69 in Sixth Edition

Since reactions 2 and 3 are the ones used to drive the regeneration of ATP, I would first use them with the Hess's Law-like method to figure out the ∆G of the reaction, taking into account 3 moles of NADH. Then to get it with respect to ATP, divide by the ∆G you calculated divded by the ∆G for the reaction with ATP do get the amount of moles regenerated if all of the free energy released was used to drive the reaction.