## 14.23

$\Delta G^{\circ} = -nFE_{cell}^{\circ}$

alondra_1D
Posts: 17
Joined: Wed Sep 21, 2016 2:59 pm

### 14.23

For each reaction that is spontaneous under standard conditions, write a cell diagram, determine the standard cell potential, and calculate delta G for the reaction:

(a) $2NO_{3}^-(aq)+8H^+(aq)+6Hg(l)\rightarrow 3Hg_{2}^{2+}(aq)+2NO(g)+4H_{2}O(l)$
how do we get the moles for this reaction?

Hung_Sabrina_3N
Posts: 22
Joined: Fri Jul 22, 2016 3:00 am

### Re: 14.23

For calculating for the standard potential energy it doesn't depend on the number of moles because its an intensive property

Olivia_Chen_3E
Posts: 18
Joined: Wed Sep 21, 2016 2:59 pm

### Re: 14.23

For calculating the number of moles, I think you have to balance the half reactions in order to find out the number of electrons transferred during the reaction, which is the number of moles that you use to find Gibbs free energy.