Question:
Consider the reactions :

2 S₂O^2–_{3 (aq)} + I_2(s) → S₄ O^2– _6(aq) + 2I^– _(aq)

S₂O^2–_3(aq) + 2Br_2(l) + 5 H₂O_(l) → 2SO^2–_4(aq)+ 4Br^–_(aq) + 10H⁺_(aq)

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

Answer:

The average oxidation number (O.N.) of S in S₂O^2–₃ is +2. Being a stronger oxidising agent than I₂, Br₂oxidises S₂O^2–₃ to SO^2-₄ , in which the O.N. of S is +6. However, I₂ is a weak oxidising agent.

Therefore, it oxidises S₂O^2–₃to S₄O^2–₆ , in which the average O.N. of S is only +2.5. As a result, S₂O^2– ₃ reacts differently with iodine and bromine.

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Question:
Consider the reactions :

2 S₂O^2–_{3 (aq)} + I_2(s) → S₄ O^2– _6(aq) + 2I^– _(aq)

S₂O^2–_3(aq) + 2Br_2(l) + 5 H₂O_(l) → 2SO^2–_4(aq)+ 4Br^–_(aq) + 10H⁺_(aq)

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

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Question: Consider the reactions : 2 S2O2– 3 (aq) + I2(s) → S4 O2– 6(aq) + 2I – (aq) S2O2– 3(aq) + 2Br2(l) + 5 H2O(l) → 2SO2–4(aq) + 4Br–(aq) + 10H+(aq) Why does the same reductant, thiosulphate react differently with iodine and bromine ?

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Question:
Consider the reactions :

2 S₂O^2–_{3 (aq)} + I_2(s) → S₄ O^2– _6(aq) + 2I^– _(aq)

S₂O^2–_3(aq) + 2Br_2(l) + 5 H₂O_(l) → 2SO^2–_4(aq)+ 4Br^–_(aq) + 10H⁺_(aq)

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