In our last post, we looked at the overview of electrode potentials, where we discussed metal ions/metal systems or half-cells, standard electrode potential and electrochemical cells in depth. Here, we will focus on the calculations involving electrode potentials, which include calculations of the electromotive force (e.m.f) of electrochemical cells , the relationship between e .m.f & free energy and the relationship between e .m.f & equilibrium constant. Half-Cell Reactions Std Reduction Potential , E° (V) K+(aq) + e- <----> K(s) -2.92 Ca2+(aq) + 2e- <----> Ca(s) -2.87 Na+(aq) + e- <----> Na(s) -2.71 Mg2+(aq) + 2e- <----> Mg(s) -2.37 Al3+(aq) + 3e- <----> Al(s) -1.66 Zn2+(aq) + 2e- <----> Zn(s) -0.76 Fe2+(aq) + 2e- <----> Fe(s) -0.44 Sn2+(aq) + 2e- <
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