6M 2

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

MariaJohn1D
Posts: 50
Joined: Wed Nov 08, 2017 3:01 am

6M 2

For the equation deltaG= -nFE, why can’t you add up the E’s of both half reaction to get Ecell?

Posts: 81
Joined: Fri Aug 09, 2019 12:17 am

Re: 6M 2

Ecell should be E(cathode/reduced) - E(anode/oxidation). If the negatives worked out that way, there should be scenarios in which you could add the potentials of the half reactions to find the total potential

Bella Townsend
Posts: 50
Joined: Wed Feb 20, 2019 12:18 am

Re: 6M 2

In the overall reaction the electrons in the cathode and anode half reactions cancel out.

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 1 guest