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### Nernst

Posted: Sat Mar 02, 2019 12:53 pm
Where does the 0.0592 come from in the nernst equation?

E = E (standard) — (0.0592/n) log Q

### Re: Nernst

Posted: Sat Mar 02, 2019 1:07 pm
The 0.0592 comes from changing the natural log in the original equation ( E=E(standard)-(RT/nF)lnQ ) to log base 10, which yields E=E(standard)-(2.303RT/nF)logQ. At standard temperature (298K), 2.303RT/F = 0.0592, which gives you the representation of the Nernst equation that first mentioned, E = E (standard) — (0.0592/n) log Q.

### Re: Nernst

Posted: Sat Mar 02, 2019 3:15 pm
0.0592 comes from changing the equation from terms of natural log (ln) to log base ten.

### Re: Nernst

Posted: Sat Mar 02, 2019 3:26 pm
What sort of energy/cell potential does Nernst equation tell us?

### Re: Nernst

Posted: Sat Mar 02, 2019 3:34 pm
MadelineHlobik wrote:What sort of energy/cell potential does Nernst equation tell us?

I believe the Nernst equation tells us the equilibrium potentials of the cell. For each ion, the equilibrium potential is the membrane potential where the net flow is zero through any open channel.