Hey guys!
I was wondering if anyone could help me understand the relationship between standard cell potential and equilibrium constant of a reaction?
Thank you!
Standard Cell Potential
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Re: Standard Cell Potential
Sometimes, a picture is worth a thousand words. I believe the equation I have attached best summarizes the relationship between standard cell potential and the equilibrium constant of a reaction.
Re: Standard Cell Potential
Hey! So there is just an equation relating the two for a redox reaction that is, Eo=(RT/nF)ln(K) or if you solve for K, K=e^(nFEo/RT), but the equation isn't super intuitive or give you much insight as to why the standard cell potential is related to K. We can start by saying that nFEcell is an expression that gives that maximum amount of work that can be done by the transfer of electrons in the reaction, which is related to delta G. Delta Go is equal to -nFEocell but it is also equal to -RT Ln(K). We can then set these equal to each other and get the original equation relating Eo and K. So basically they are related because both of them are related to delta G and as such they can be related to each other. Hope this helps!
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Re: Standard Cell Potential
Isolating each of the variables, Increasing T increases cell potential, decreasing it decreases cell potential. If nF is increased E of the cell decreases whereas if nF decreases Ecell increases.Same thing for ln(K) because ultimately it is a value that you are multiplying your fraction by.
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