Classify the following reaction: Zn + CuSO4 = ZnSO4 + Cu.
The Correct Answer and Explanation is :
The reaction ( \text{Zn} + \text{CuSO}_4 \rightarrow \text{ZnSO}_4 + \text{Cu} ) is classified as a single displacement (or single replacement) reaction. In this type of reaction, one element replaces another in a compound, resulting in the formation of a new compound and the release of a different element.
Explanation:
- Reactants and Products: In this reaction, zinc (Zn) is a more reactive metal compared to copper (Cu). Copper sulfate (( \text{CuSO}_4 )) serves as the compound containing copper. When zinc is introduced to this solution, it displaces the copper from the copper sulfate, leading to the formation of zinc sulfate (( \text{ZnSO}_4 )) and the liberation of copper metal.
- Reactivity Series: The reactivity series is a list of metals arranged in order of decreasing reactivity. Zinc is positioned above copper in this series, indicating that zinc has a greater tendency to lose electrons and form positive ions. As a result, zinc can effectively displace copper from its compound.
- Electron Transfer: This reaction involves the transfer of electrons. Zinc, when it reacts, loses two electrons to form ( \text{Zn}^{2+} ), while copper ions (( \text{Cu}^{2+} )) in the copper sulfate solution gain these electrons to become elemental copper (Cu). The overall electron transfer process underlies the underlying chemistry of single displacement reactions.
- Applications: Single displacement reactions, like the one between zinc and copper sulfate, are commonly encountered in various applications, including galvanization (the process of applying a protective zinc coating to steel or iron) and in electrochemical cells, where metal displacement reactions can generate electrical energy.
In summary, the reaction ( \text{Zn} + \text{CuSO}_4 \rightarrow \text{ZnSO}_4 + \text{Cu} ) exemplifies a single displacement reaction, showcasing the fundamental principles of reactivity, electron transfer, and metal behavior in chemical processes.