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Question
Thiosulphate reacts differently with iodine and bromine in the reactions given below:
\[\ce{2S2O^{2-}3 + I2 -> S4O^{2-}6 + 2I-}\]
\[\ce{S2O^{2-}3 + 2Br2 + 5H2O -> 2SO^{2-}4 + 2Br- + 10H+}\]
Which of the following statements justifies the above dual behaviour of thiosulphate?
Options
Bromine is a stronger oxidant than iodine.
Bromine is a weaker oxidant than iodine.
Thiosulphate undergoes oxidation by bromine and reduction by iodine in these reactions.
Bromine undergoes oxidation and iodine undergoes reduction in these reactions.
Solution
Bromine is a stronger oxidant than iodine.
Explanation:
Standard reduction potential of bromine is higher than Iodine, hence Bromine is a stronger oxidant than iodine.
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