Final answer:
In the given reaction, the oxidizing agent is O2 because it gains electrons (is reduced), and the reducing agent is sulfur in CS2 as it loses electrons (is oxidized).
Step-by-step explanation:
To identify the oxidizing agent and the reducing agent in the given chemical reaction, we should first assign the oxidation numbers to each atom in the reactants and products.
Once we determine which atoms have undergone changes in their oxidation states, we can establish which species are oxidized and which are reduced.
In the reaction CS2 + 3 O2 → CO2 + 2 SO2, let's assign the oxidation numbers:
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- C in CS2 = +4
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- S in CS2 = -2
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- O in O2 = 0
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- C in CO2 = +4
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- S in SO2 = +4
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- O in SO2 and CO2 = -2
Through the reaction, carbon (C) maintains its oxidation state, so there's no change. Sulfur (S) goes from -2 in CS2 to +4 in SO2, which means it is being oxidized (increase in oxidation number). Oxygen (O) goes from 0 in O2 to -2 in both SO2 and CO2, indicating it is being reduced (decrease in oxidation number).
Therefore, the oxidizing agent is oxygen (O2), since it is the species that is being reduced (accepts electrons). The reducing agent is sulfur in CS2, as it is the species that is being oxidized (loses electrons).