Currently the rate equation I found was the one by Burdett et al (1984) Rate [SO3] = k[SO2]*[O2]/RT ; k = (2.6+/-1.3 e 12)*exp(-23000 +/- 1200/T). I hope someone can help me with something that contains H2O or OH in the rate equation.
This is a complex reaction contains many elementary steps,
burt you can get informations on the most important ones from NIST database:
http://kinetics.nist.gov/kinetics/index.jsp
With all best wishes: Béla
Thank you Bela. I hope I could find even multiple ones. I have tried using NIST before. I might try giving it another go.
The gas-phase atmospheric mechanism for oxidation of SO2 is thought to be:
SO2 + OH + M -> HOSO2 + M where M is any molecule (N2, O2, Ar)
HOSO2 + O2 -> HO2 + SO3
SO3 + H2O -> H2SO4
The first step is usually rate limiting.
In aqueous aerosols:
SO2 + H2O2 -> H2SO4 (via a complex mechanism)
You can find it on page 356 of the textbook "Atmospheric Chemistry and Global Change", Edited by Guy Brasseur, John Orlando and Geoffrey Tyndall, Oxford University Press, 1999. The atmospheric oxidation of SO2 is described in other atmospheric chemistry textbooks as well.
This reaction is catalyzed by metal ions like Fe(II/III) and Mg. See detailed reaction mechanisms in Inorg Chem 1993, 32(21), 4527-4538 and 1998, 37(19), 4939-4944.
Good luck!
Thank you very much Sir John Birks and Sir Lars Elding.
Mr. Elding, I was able to check the 1993 but I cannot access the 1998. The 1993 is a very big help for me. Thanks so much.
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