Of moles of electrons, that's equal to two, times the log of the reaction quotient. Potential E is equal to the standard cell potential. So let's go ahead and plug in everything. Two plus is one molar, the concentration of copper We know what those concentrations are, they were given to us in the problem. We're gonna leave out the solid zinc so we have the concentration Of zinc two plus, so concentration of our product, over the concentration of our reactants. We'll leave out solid copper and we have concentration To write Q think aboutĪn equilibrium expression where you have yourĬoncentration of products over the concentration of your reactants and you leave out pure solids. So think about writing anĮquilibrium expression. Q is the reaction quotient, so Q is the reaction quotient, and Q has the same form as K but you're using Moles that are transferred, number of moles of electrons that are transferred in our redox So this 1.10 would get plugged in to here in the Nernst equation. The standard cell potential, E zero, we've already found What these things mean in the Nernst equation. The Nernst equation, this is one of the forms that we can use when our temperature is 25 degrees C. So let's go ahead and writeĭown the Nernst equation, which is the cell potential is equal to the standard cell potential, E zero, minus. So all of this we'veĬovered in earlier videos and now we're gonna see how to calculate the cell potential using Standard reduction potential and the standard oxidation potential. Overall redox reaction, and the standard cell potential is equal to positive 1.10 volts, so you just add the Gained by copper two plus, so they cancel out when you Those two electrons, theĮlectrons lost by zin, are the same electrons So zinc loses two electrons to form zinc two plus ions. They gain electrons to form solid copper. Reduction half reaction and the oxidation half reaction, copper two plus ions are reduced. Two plus ions in solution is one molar, and we're at 25 degrees C. Of zinc two plus ions and the concentration of copper The cell potential for a zinc-copper cell, where the concentration Use the Nernst equation to calculate cell potentials.
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