## 14.93.a

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

manasa933
Posts: 72
Joined: Fri Sep 29, 2017 7:04 am

### 14.93.a

If you were to construct a concentration cell in which one half-cell contains 1.0 m CrCl3 and the other half-cell contains 0.0010 m CrCl3, and both electrodes were chromium, at which electrode would reduction take place spontaneously?

Why does reduction take place at the electrode with the higher concentration?

Ashin_Jose_1H
Posts: 51
Joined: Fri Sep 29, 2017 7:04 am

### Re: 14.93.a

The reaction is trying to reach equilibrium. In order to do that, the concentrations must be the same. When the electrode with the higher concentration starts to get reduced, the amount of substance available for reduction decreases. Eventually, this will lead the reaction to equilibrium.

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

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