## 6N.9

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

Alicia Lin 2F
Posts: 83
Joined: Wed Sep 18, 2019 12:17 am

### 6N.9

A tin electrode in 0.015 M Sn(NO3)2(aq) is connected to a hydrogen electrode in which the pressure of H2 is 1.0 bar. If the cell potential is 0.061 V at 25 °C, what is the pH of the electrolyte at the hydrogen electrode?

How do we determine which is the cathode and which is the anode? Is there a general rule or thought process for standard hydrogen electrodes?

AKhanna_3H
Posts: 104
Joined: Wed Sep 18, 2019 12:19 am

### Re: 6N.9

I'm not sure if you can use this logic with every problem, but I think you would determine which is which by calculating what would make the overall cell potential positive. So you could find the individual cell potentials for each half reaction, and then determine which would make E(cathode) - E(anode) a positive value.

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 4 guests