Thiosulphate reacts differently with iodine and bromine in the reactions given below: 2S2O2-3 + I2 → S4O2-6 + 2I- S2O32- + 2Br2 + 5H2O → 2SO2-4 + 2Br- + 10H+ Which of the following statements justifies the above dual behaviour of thiosulphate?

Question

Thiosulphate reacts differently with iodine and bromine in the reactions given below: 2S2O2-3 + I2 → S4O2-6 + 2I- S2O32- + 2Br2 + 5H2O → 2SO2-4 + 2Br- + 10H+ Which of the following statements justifies the above dual behaviour of thiosulphate? (A) Bromine is a stronger oxidant than iodine. (B) Bromine is a weaker oxidant than iodine. (C) Thiosulphate undergoes oxidation by bromine and reduction by iodine in these reactions. (D) Bromine undergoes oxidation and iodine undergoes reduction in these reactions.

Tardigrade Admin · Accepted Answer

Br2 oxidises S to a higher oxidation state

and I2 oxidises S to a lower oxidation state

. Thus, Br2 is stronger oxidising agent than I2.

Q. Thiosulphate reacts differently with iodine and bromine in the reactions given below: 2S2​O32−​+I2​→S4​O62−​+2I− S2​O32−​+2Br2​+5H2​O→2SO42−​+2Br−+10H+ Which of the following statements justifies the above dual behaviour of thiosulphate?

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.

Br2​ oxidises S to a higher oxidation state and I2​ oxidises S to a lower oxidation state . Thus, Br2​ is stronger oxidising agent than I2​.

$B r_{2}$ oxidises $S$ to a higher oxidation state and $I_{2}$ oxidises $S$ to a lower oxidation state . Thus, $B r_{2}$ is stronger oxidising agent than $I_{2}$ .