# Question #c39c4

This happens because zinc is higher on the activity series than copper.

#### Explanation:

The type of reactions you are asking about are called single replacement reactions.

$Z n \left(s\right) + C {u}_{S} {O}_{4} \to Z n S {O}_{4} + C u \left(s\right)$ - this reaction will occur.

It happens because zinc has a higher activity than copper. I'll use an analogy to explain why this happens. The $S {O}_{4}^{2 -}$ ion decides that Zn is better looking than Cu, so it drops the copper in favor of hanging out with zinc.

$C u \left(s\right) + Z {n}_{S} {O}_{4} \to Z n S {O}_{4} + C u \left(s\right)$ - there is no change here.

This happens because copper is lower on the activity series. To continue the analogy... the $S {O}_{4}^{2 -}$ is already paired with the better looking partner, so it stays put.

This video shows an experiment which proves that zinc has a higher activity than copper.

Hope this helps!