Solution:
Nernst equation in electrochemistry is a relationship between the reduction potential of a reaction (either a half-cell or full-cell reaction) and various parameters such as the standard electrode potential, temperature, and activities (often approximated by concentrations) of the chemical species undergoing reduction and oxidation. It was given this name in honor of Walther Nernst, a German physical chemist who came up with the equation.
(i) For the given reaction, the Nernst equation can be given as:![E_{c e l l}=E_{c e l l}^{0}-\frac{0.591}{n} \log \frac{\left[ Mg ^{2+}\right]}{\left[ Cu ^{2+}\right]}=0.34-(-2.36)-\frac{0.0591}{2} \log \frac{0.001}{0.0001} 2.7-\frac{0.0591}{2} \log 10](https://www.learnatnoon.com/s/wp-content/ql-cache/quicklatex.com-921b3c71ac758e61811920183b7e50bf_l3.png "Rendered by QuickLaTeX.com")
(ii) For the given reaction, the Nernst equation can be given as:![E_{c e l l}=E_{c e l l}^{0}-\frac{0.591}{n} \log \frac{\left[F e^{2+}\right]}{\left[H^{+}\right]^{2}}](https://www.learnatnoon.com/s/wp-content/ql-cache/quicklatex.com-cf5be98ee96443690337084c000c94d4_l3.png "Rendered by QuickLaTeX.com")
