How wet corrosion works
Hi there. I'm a high school student in garde 11 and I am doing an assignment on corrosion and finding it extremely difficult to understand and explain how wet corrosion works. I was wondering if oxidation actually involves the metal dissolving, as some information I have found has mentioned that it does so that the dissolved particles then react with the oxygen? I was also wondering why exactly steel rusts faster than pure iron does. and lastly why exactly does salt increase the rate of corrosion?
any help would be greatly appreciated.
student - Brisbane, Queensland, Australia
Corrosion NEEDS humidity, it NEEDS moisture ...t'other wise if it's dry, you shouldn't get any corrosion, eh?
Why does, you ask, iron corrode more quickly than steel ?
Surely that depends upon the 'ingredients', ie. the alloys in it .... ordinary iron has quite a higher Carbon content than steel and can possess some sulphur and phosphorus ... after all, steel is MADE from iron by a refining process (open hearth or electrical furnaces) to knock out the S and P and reduce the carbon content
Salt is an alkaline ... eg. seawater ... and that can eat up/reduce both steel and iron.
I hope that that helps.
White Rock, British Columbia, Canada
(It is our sad duty to
advise that Freeman passed away
April 21, 2012. R.I.P. old friend).
This public forum has 60,000 threads. If you have a question in mind which seems off topic to this thread, you might prefer to Search the Site