Calculate cell potential when concentrations aren't 1M, but are the same.

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SUMMARY

The discussion centers on calculating the standard cell potential for a galvanic cell involving Cu2+ at 0.5M and Zn2+ at 0.5M concentrations. The formula used is Ecell = E0cell - (RT/nF)lnQ, where the standard potentials are ECu = 0.340V and EZn = -0.763V, resulting in a calculated Ecell of 1.103V. The discussion clarifies that when the concentrations of both ions are equal, the reaction quotient Q equals 1, leading to lnQ = 0, which indicates that the concentrations do not affect the final cell potential in this specific case.

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Homework Statement


Calculate standard potential for a Cu2+ 0.5M, Zn2+ 0.5M cell.

Homework Equations


Ecell = E0cell - (RT/nF)lnQ

The Attempt at a Solution


So, I know at standard conditions it would simply be
Ecell = 0.340 - (-0.763)
Ecell = 1.103

It's the concentrations that are confusing me. If they are the same and no half reactions are multiplied, I get a Q value of 1.
lnQ = ln(1) = 0.
So in this case does it not matter what the concentrations are as long as they are the same?
 
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In this case potentials of both half reactions are shifted by the same amount, so the final result stays the same. It doesn't have to be always this way.
 
Sorry for the delayed thank you, but thank you :)
 

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