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Using the information from a standard reduction potentials table (see link below), the standard cell potential for the zinc/lead cell is then: EÂºcell = EÂºcathode - EÂºanode = -0.13 - (- 0.76) = 0.63 V.
Now we have the log of K, and notice that this is the equation we talked about in an earlier video. The standard cell potential E zero is equal to .0592 over n times the log of K. So just an interesting way to think about the Nernst equation. The Nernst equation is very useful for calculating cell potentials when you have different concentrations.