The correct option is D bromine is both reduced and oxidised
The balanced chemical equation is 3Br2+6CO2−3+3H2O⟶5Br⊖+BrO⊖3+6HCO⊖3.
The oxidation number of bromine decreases from 0 (in Br2) to -1 (in Br−). Thus, bromine is reduced.
The oxidation number of bromine increases from 0 (in Br2) to +5 (in BrO−3). Thus, bromine is oxidized.
Thus, in the given reaction, bromine is both reduced and oxidized.