Final answer:
In the reaction provided, MnO4⁻(aq) is the reactant that gets reduced, as it goes from an oxidation state of +7 to +4, indicating a gain of electrons.
Step-by-step explanation:
To identify the reactant that gets reduced in the reaction 2MnO4⁻(aq) + Br⁻(aq) + H₂O(l) → 2MnO2(s) + BrO3⁻(aq) + 2OH⁻(aq), we must look at the changes in oxidation numbers of the reactants. In a redox (reduction-oxidation) reaction, the substance being reduced is the one that gains electrons (decrease in oxidation state), while the one being oxidized loses electrons (increase in oxidation state).
Manganese (Mn) in permanganate ion, MnO4⁻, goes from an oxidation state of +7 in MnO4⁻ to +4 in MnO2. This change indicates a gain of three electrons, signifying reduction. On the other hand, bromine (Br) goes from an oxidation state of -1 in Br⁻ to +5 in BrO3⁻, indicating the loss of electrons, which means it is oxidized. Therefore, the reactant that gets reduced in this reaction is Option 1: MnO4⁻(aq).