Final answer:
In the redox reaction MnO4- + SO2 → Mn2+ + SO42-, MnO4- is the oxidizing agent as it is reduced, and SO2 is the reducing agent as it is oxidized.
Step-by-step explanation:
The question presented is related to identifying the substances that are being oxidized and reduced in a redox reaction, as well as identifying the oxidizing and reducing agents. In a redox reaction, the substance that loses electrons is considered to be the substance being oxidized and simultaneously acts as the reducing agent. Conversely, the substance that gains electrons is being reduced and acts as the oxidizing agent.
Let's examine the provided reaction: MnO4- +SO2 → Mn2+ + SO42-. To determine what is being oxidized and what is being reduced, we should look at the change in oxidation states of the elements. Manganese (Mn) goes from an oxidation state of +7 in MnO4- to +2 in Mn2+, indicating it has been reduced. Sulphur (S) goes from an oxidation state of +4 in SO2 to +6 in SO42-, indicating it has been oxidized.
Therefore, in this reaction, MnO4- acts as the oxidizing agent, because it is reduced, and SO2 acts as the reducing agent, because it is oxidized.