In the following reaction: 3Br2+6CO2−3+3H2O→5Br−+BrO−3+6HCO−3
A
bromine is oxidised and carbonate is reduced
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B
bromine is oxidised
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C
bromine is neither oxidised nor reduced
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D
bromine is reduced
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Solution
The correct options are C bromine is oxidised D bromine is reduced 3Br2+6CO2−3+3H2O→5Br−+BrO−3+6HCO−3 0 +4 -1 +5 +4 Therefore, this is a disproportionation reaction in which bromine is oxidised as well as reduced.