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Consider the reactions 2S2O3(aq)+I2(s)-->S4O6(aq)+2I(aq) & S2O3(aq)+2Br2(l)+5H2O(l)-->2SO4^2-(aq)+4Br^-(aq)+10H^+ why does the same

8.14  Consider the reactions :
2S_{2}O_{3}^{2-}(aq)+I_{2}(s)\rightarrow S_{4}O_{6}^{2-}(aq)+2I^{-}(aq)

2S_{2}O_{3}^{2-}(aq)+2Br_{2}(l)+5H_{2}O(l)\rightarrow SO_{4}^{2-}(aq)+4Br^{-}(aq)+10H^{+}(aq)

 Why does the same reductant, thiosulphate react differently with iodine and bromine? 

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Answer-

F_{2}>Cl_{2}>Br_{2}>I_{2}  oxidizing power order

Bromine is a stronger oxidizing agent than iodine. So in the case of bromine (avg. oxidation number of sulphur is changed from +2 to +6)

and in case of iodine it (+2 to +2.5). So that's why thiosulphate reacts differently with bromine and iodine.

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