Given below is the standard electrode potential (Eo) of the following redox reaction. Predict the most feasible event, if the reaction occurred spontaneously.
|A||Zn2+ was reduced|
|B||Sn was oxidized|
|C||Zn lost electrons|
|D||Ether was used as the solvent medium|
Now we have a positive voltage, where the zinc is oxidized and a tin ion is reduced. Oxidation of zinc means it is losing electrons. Recall that oxidation is losing electrons, and reduction is gaining electrons.