In a message dated 7/11/2005 12:02:39 AM Eastern Daylight Time, LISTSERV**At_Symbol_Here**LIST.UVM.EDU writes: > I fail to see how gaseous HF can react with steel to produce an excessive > hydrogen pressure and burst a cylinder: > 6HF + 2Fe yields 2FeF3 + 3H2 > The product would be FeF3, not FeF2, because fluorine is an excellent > oxidizing agent. Consequently, if anything, the gas pressure inside the > cylinder would necessarily be reduced as the HF attacks the iron of the > cylinder. > > It's obvious that the cause of the explosion was the thinning of the > cylinder wall at one or more locations, NOT the pressure of the hydrogen. > > Jay Young Hey Older (oldest?) Guy, If Fluorine is such a good oxidizer why doesn't it oxidize iron to the more oxidized state (+3) just as peroxides do when you kill them with +2 iron (ferrous sulfate) to make ferric sulfate and reduced peroxides? Why do you believe that it will stop at the +2 state? Not quite as old but working on it ... slowly. James A. Kaufman, Ph.D. President/CEO jimkaufman**At_Symbol_Here**labsafety.org The Laboratory Safety Institute A Nonprofit International Organization for Safety in Science and Science Education 192 Worcester Road, Natick, MA 01760-2252 508-647-1900 Fax: 508-647-0062 Cell: 508-574-6264 Res: 781-237-1335 info**At_Symbol_Here**labsafety.org www.labsafety.org
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