In a lab expirement you add copper(II)nitrate to pure zinc. Write a balanced equation for this expirement and predict if a reaction will occur.
Zinc is more active than copper, so zinc will donate electrons to the copper ions, precipating it as copper.
Cu(NO3)2 (aq) + Zn (s) = Cu (s) + Zn(NO3)2
To balance the equation, you need to ensure that you have an equal number of each type of atom on both sides of the equation. Here's the balanced equation for this experiment:
Cu(NO3)2 (aq) + Zn (s) → Cu (s) + Zn(NO3)2 (aq)
Regarding the prediction if a reaction will occur, copper(II) nitrate is an aqueous solution (indicated by the "(aq)") and zinc is a solid (indicated by the "(s)").
Since zinc is more active than copper, it can displace copper from copper(II) nitrate. This means the zinc atoms will donate electrons to the copper ions, resulting in the formation of solid copper.
Therefore, a reaction will occur and you will observe the precipitation of copper as a solid.