Final answer:
In the reaction between zinc powder and copper (II) sulphate solution, zinc is the reducing agent as it gets oxidized, and copper (II) ions are the oxidizing agent as they are reduced to metallic copper.
Step-by-step explanation:
Oxidizing and Reducing Agents in Redox Reactions
When zinc powder reacts with copper (II) sulphate solution, a direct redox reaction occurs. In this process, zinc serves as the reducing agent because it loses electrons and undergoes oxidation to form Zn²⁺ ions:
Zn(s) → Zn²⁺(aq) + 2e⁻
Simultaneously, the copper (II) ions act as the oxidizing agent, accepting the electrons released by the zinc and being reduced to metallic copper:
Cu²⁺(aq) + 2e⁻ → Cu(s)
It is important to note that in a redox reaction, the oxidizing agent is reduced, and the reducing agent is oxidized. This can be summarized as the substance gaining electrons is the oxidizing agent, while the one losing electrons is the reducing agent. Zinc's higher reactivity compared to copper explains why it can donate electrons in this reaction, evidenced by its placement above copper in the activity series.
Complete Redox Reaction
Combining the two half-reactions, we get the overall equation for the reaction:
Zn(s) + CuSO₄(aq) → Cu(s) + ZnSO₄(aq)