In the redox reaction, which substance acts as the oxidizing agent?

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Multiple Choice

In the redox reaction, which substance acts as the oxidizing agent?

In redox reactions, the oxidizing agent is the species that gains electrons (is reduced) and thus drives the oxidation of another substance. Tin(IV) oxide can accept electrons and be reduced to a lower oxidation state, for example SnO2 + 4 H+ + 2 e- → Sn2+ + 2 H2O. Since SnO2 undergoes reduction by taking electrons, it acts as the oxidizing agent in the reaction. The other options would themselves be the species donating or accepting electrons in different half-reactions (Cl- would be oxidized to Cl2, H+ would be reduced to H2, etc.), not the reducer in this particular process.

In redox reactions, the oxidizing agent is the species that gains electrons (is reduced) and thus drives the oxidation of another substance. Tin(IV) oxide can accept electrons and be reduced to a lower oxidation state, for example SnO2 + 4 H+ + 2 e- → Sn2+ + 2 H2O. Since SnO2 undergoes reduction by taking electrons, it acts as the oxidizing agent in the reaction. The other options would themselves be the species donating or accepting electrons in different half-reactions (Cl- would be oxidized to Cl2, H+ would be reduced to H2, etc.), not the reducer in this particular process.

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