[H2O]

I have been working on this question for a while. I need some help with it.

"Calculate the equilibrium constant (K) of the following redox reaction:
2S₂O₃^2– + I₂--> S₄O₆ ^2– + 2I^1–

I have found that S, +4-->+2.5 in oxidation number; my problem is with iodine.

I think that the problem would be solved as: I^-1I¹⁺ and then we could say I, +1-->-1

this does not make any sense. Can you help?

[mike]

The oxidation number for I₂ is 0.

[H2O]

thank you! that really helps

[jdurg]

I have been working on this question for a while. I need some help with it.

"Calculate the equilibrium constant (K) of the following redox reaction:
2S₂O₃^2– + I₂--> S₄O₆ ^2– + 2I^1–

I have found that S, +4-->+2.5 in oxidation number; my problem is with iodine.

I think that the problem would be solved as: I^-1I¹⁺ and then we could say I, +1-->-1

this does not make any sense. Can you help?

I'd take a further look at your oxidation number there for Sulfur.  (Hint:  Ignore the 2 before the molecule and focus on the S2O3 (2-) portion of it).