nernst

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

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

nernst

When you double the equation why does the G increase the E stay the same?

Jiyoon_Hwang_2I
Posts: 101
Joined: Sat Sep 14, 2019 12:17 am

Re: nernst

E is an intensive property so it doesn’t depend on the amount of substances involved so multiplying the reaction equation does not multiply E

Rafsan Rana 1A
Posts: 55
Joined: Sat Aug 24, 2019 12:16 am

Re: nernst

When using the equation delta g = -nFe, e cell doesn't change and G does because of the n which is number of electrons transferred. Doubling the equation means increasing the number of electrons changing the value of G.

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

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