Calculating Cell Potential using the Nernst Equation

In electrochemistry, the relationship between the cell potential and the concentration of reactants and products can be described by the Nernst equation. Consider a galvanic cell where copper(II) ions ( ext{Cu}^{2+}) are reduced to solid copper (Cu) at the cathode, and zinc (Zn) is oxidized to zinc ions ( ext{Zn}^{2+}) at the anode. The standard reduction potentials ( ext{E}^ ext{o}) for the half-reactions are as follows:

Cu}^{2+} + 2e^{-} → Cu : ext{E}^ ext{o} = +0.34 ext{ V}

Zn}^{2+} + 2e^{-} → Zn : ext{E}^ ext{o} = -0.76 ext{ V}

If you have a solution where the concentration of ext{Cu}^{2+} is 1.0 M and the concentration of ext{Zn}^{2+} is 0.01 M at 25°C, what is the cell potential (E) for this galvanic cell?