* The reactivity series: Copper is less reactive than zinc. This means that copper cannot displace zinc from its salt solution.
* Electrochemical potential: Zinc has a more negative standard electrode potential than copper. This means that zinc is more likely to lose electrons and become oxidized, while copper is more likely to gain electrons and become reduced.
In summary, the reaction between copper and zinc nitrate is not thermodynamically favorable, and no visible changes will be observed.
What would happen if the situation were reversed?
If zinc metal were placed in a copper nitrate solution, a reaction would occur:
* Zinc displaces copper: Zinc, being more reactive, would displace copper from the solution. This would result in the formation of zinc nitrate in solution and the deposition of solid copper metal on the zinc surface.
Equation for the reaction:
Zn(s) + Cu(NO₃)₂(aq) → Zn(NO₃)₂(aq) + Cu(s)
