[Olya315]

In the iodine clock reaction with S2O3 ion I have found that one of the exponents in the reaction rate is 1.55. Can I round it to 2? Or shoud I write it as a fruction 3/2?

I know that reaction rate can be a fraction. But it is a fraction in this case?

Thank you! :)

[mirna sherry]

For sure it can be 1.55 you must leave it as it is.

[mirna sherry]

Thank you but iodine doesn't react with oxygen

[Perito]

This is in the wrong thread. Here is the original thread.

https://www.askmehelpdesk.com/chemis...rs-351397.html

Iodine certainly won't react with oxygen, but will it react with iodide? It certainly doesn't do it very often, but it can happen (the Winkler test requires a Manganese catalyst). Oxygen is a sufficiently strong oxidizer.

Winkler test for dissolved oxygen - Wikipedia, the free encyclopedia

Time-resolved reaction of oxygen(1.DELTA.) with iodide in aqueous solution - The Journal of Physical Chemistry (ACS Publications)

E = - 0.54 volts

E = 1.23 V

ΔE = +.69 volts

You can see that the electrochemical potential is there (which says nothing about kinetics). In addition, it only takes a tiny amount of iodine to turn starch blue. The last thing is that it's the only thing I can think of that's present that could oxidize iodide to iodine. Iodine has to be present or the starch wouldn't turn blue. I'm open to other suggestions.