## 14.43

$E_{cell} = E_{cell}^{\circ}-\frac{RT}{nF}\ln Q$

Sarah Rutzick 1L
Posts: 50
Joined: Tue Oct 10, 2017 7:13 am

### 14.43

In 14.43, why are we able to mix the concentrations and the pressures given to us when calculating Q?

Chloe1K
Posts: 23
Joined: Fri Sep 29, 2017 7:05 am

### Re: 14.43

I don't think we've discussed how this works yet but it does!

Chem_Mod wrote:The exact reasons for this are quite technical and relate to the concept of standard states. In the end, if you want to use a "mixed" equilibrium expression, containing both concentrations and pressures, then the pressures must be in bars, and concentrations in molarity.

Return to “Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)”

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