## 6.N.15 7th Ed

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

Ahmed Mahmood 4D
Posts: 72
Joined: Fri Sep 28, 2018 12:28 am

### 6.N.15 7th Ed

"Calculate the potential of a cell constructed with two nickel electrodes. The electrolyte in one compartment is 1.0 M Ni(NO3)2. In the other compartment, NaOH has been added to a Ni(NO3)2 solution until the pH = 11 at 298 K. Use Table 6I.1"

I’ve found the concentrations of both nickel ion. When setting up ln(Q), how do I find out which nickel is the product and which one is the reactant?

David S
Posts: 54
Joined: Fri Sep 28, 2018 12:15 am

### Re: 6.N.15 7th Ed

Looks like a concentration cell to me. If we want our concentration cell to do work, Ecell has to be positive.

Since Ecell = -(RT/nF)lnQ (E° = 0 for conc. cell), and the ln of numbers less than 1 is negative, we know that we want a Q that is less than one. For Q to be less than one, [P]<[R]. Thus, make the side with lower conc the P, and the higher conc the R.

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

### Who is online

Users browsing this forum: No registered users and 2 guests