Give the Nernst equation for the $E_{cell}$ of a Nickel-Copper galvanic cell.
(N/A) For a Nickel-Copper galvanic cell,the cell reaction is: $Ni(s) + Cu^{2+}(aq) \rightarrow Ni^{2+}(aq) + Cu(s)$.
According to the Nernst equation,the cell potential $E_{cell}$ is given by:
$E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} \log \frac{[Ni^{2+}]}{[Cu^{2+}]}$.
Here,$n = 2$ (number of electrons transferred).
Thus,the equation is: $E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{2} \log \frac{[Ni^{2+}]}{[Cu^{2+}]}$.
According to the Nernst equation,the cell potential $E_{cell}$ is given by:
$E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} \log \frac{[Ni^{2+}]}{[Cu^{2+}]}$.
Here,$n = 2$ (number of electrons transferred).
Thus,the equation is: $E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{2} \log \frac{[Ni^{2+}]}{[Cu^{2+}]}$.
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