Which statement correctly describes the relative redox behaviour of halogens or halide ions?
In the reaction of solid NaBr\text{NaBr}NaBr with concentrated H2SO4\text{H}_2\text{SO}_4H2SO4, the bromide ions are oxidised to Br2\text{Br}_2Br2 because they are stronger reducing agents than chloride ions.
In the reaction of solid NaCl\text{NaCl}NaCl with concentrated H2SO4\text{H}_2\text{SO}_4H2SO4, the chloride ions are oxidised to Cl2\text{Cl}_2Cl2 because they are stronger reducing agents than fluoride ions.
Bromine water can oxidise chloride ions in aqueous solution because bromine is a stronger oxidising agent than chlorine.
Iodine can reduce bromide ions in aqueous solution because iodine is a stronger reducing agent than bromine.