## General Chemistry

### Electrochemistry

Question
1 out of 10

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
Ans. C A redox equation is represented in the question. The electrode potential of the reaction is also given. The question also says that the reaction occurred spontaneously. For the given direction of the reaction, the electrode potential is negative. So the reaction must have taken place in the opposite direction of what is given in the question and thus had a positive potential. A net positive potential means a negative free energy change. A negative free energy change denotes spontaneity. We can rewrite the equation:

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.