Solid Solubility???
Paul M. in San Diego
>I received this as a forwarded email, so I don't know the original source. It's way over my head, but perhaps some metal-heads here can make sense of it.
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Usually, whenever you form an alloy, of say nickel and copper or aluminum and copper, you end up melting these metals together in the required percentages and form an alloy. There is a upper limit governed by what is called as a Lever rule for certain percentage of one type of metal soluble in another. Copper and Nickel have unlimited solid
solubility where as iron and carbon have limited solubility. But the interesting part is iron and carbon are virtually soluble even at very low temperatures and this can be very easily seen from studying their phase diagram. Here is the link for Fe-C phase diagram. Even a very low percentage of carbon is sufficient to form an iron-carbon alloy.
http://www.matter.org.uk/steelmatter/metallurgy/6_2_4.html
Here is another link for Fe-C phase diagram and the theory behind it.
http://www.mmat.ubc.ca/courses/mmat380/lectures/2004/Lecture2-Steel(completel).pdf
Thus, the bottom line is carbon can sink into iron at even very low temperatures to form a stable Fe3C phase and even very low percentage of carbon in the range of 0.005 is sufficient to form a stable phase. When you rub diamond against iron or steel containing iron you are essentially generating some temperature at the point of contact and enabling a reaction between the two. Thus, even though diamond is the hardest material, it has to succumb to iron's natural ability to eat it.